17.2 measuring and expressing enthalpy changes 1 > copyright © pearson education, inc., or its...
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgt
Chapter 17Thermochemistry
171 The Flow of Energy
172 Measuring and Expressing Enthalpy Changes
173 Heat in Changes of State174 Calculating Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgt
How can you measure the amount of heat released when a match burns
CHEMISTRY amp YOUCHEMISTRY amp YOU
Remember The concept of specific heat allows you to measure heat flow in chemical and physical processes
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
3
gtgt CalorimetryCalorimetry
Calorimetry
How can you measure the change in enthalpy of a reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
4
gtgt CalorimetryCalorimetry
Calorimetry is the measurement of the heat flow into or out of a system for chemical and physical processes
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
5
gtgt
Calorimetry is the measurement of the heat flow into or out of a system for chemical and physical processesbull In a calorimetry experiment involving an
endothermic process the heat absorbed by the system is equal to the heat released by its surroundings
bull In an exothermic process the heat released by the system is equal to the heat absorbed by its surroundings
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgt
Calorimetry is the measurement of the heat flow into or out of a system for chemical and physical processesbull The insulated device used to measure the
absorption or release of heat in chemical or physical processes is called a calorimeter
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgt
Constant-Pressure Calorimeters
Foam cups can be used as simple calorimeters because they do not let much heat in or out
bull Most chemical reactions and physical changes carried out in the laboratory are open to the atmosphere and thus occur at constant pressure
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgt
Constant-Pressure Calorimeters
The enthalpy (H) of a system accounts for the heat flow of the system at constant pressure
bull The heat absorbed or released by a reaction at constant pressure is the same as the change in enthalpy symbolized as ΔH
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
9
gtgt
Constant-Pressure Calorimeters
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at constant pressure
bull In this textbook the terms heat and enthalpy change are used interchangeably
bull In other words q = ΔH
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
10
gtgt
Constant-Pressure Calorimeters
bull To measure the enthalpy change for a reaction in aqueous solution in a foam cup calorimeter dissolve the reacting chemicals (the system) in known volumes of water (the surroundings)
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
11
gtgt
Constant-Pressure Calorimeters
bull Measure the initial temperature of each solution and mix the solutions in the foam cup
bull After the reaction is complete measure the final temperature of the mixed solutions
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
12
gtgt
Constant-Pressure Calorimeters
You can calculate the heat absorbed or released by the surroundings (qsurr) using the formula for the specific heat the initial and final temperatures and the heat capacity of water
qsurr = m C ΔT
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgt
Constant-Pressure Calorimeters
qsurr = m C ΔT
bull m is the mass of the water
bull C is the specific heat of water
bull ΔT = Tf ndash Ti
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgt
Constant-Pressure Calorimeters
The heat absorbed by the surroundings is equal to but has the opposite sign of the heat released by the system
qsurr = ndashqsys
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgt
Constant-Pressure Calorimeters
The enthalpy change for the reaction (ΔH) can be written as follows
qsys = ΔH = ndashqsurr = ndashm C ΔT
bull The sign of ΔH is positive for an endothermic reaction and negative for an exothermic reaction
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgt
Constant-Volume Calorimeters
Calorimetry experiments can also be performed at a constant volume using a device called a bomb calorimeter
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgt
Constant-Volume CalorimetersIn a bomb calorimeter a sample of a compound is burned in a constant-volume chamber in the presence of oxygen at high pressure
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgt CalorimetryCalorimetry
Constant-Volume Calorimetersbull The heat that is
released warms the water surrounding the chamber
bull By measuring the temperature increase of the water it is possible to calculate the quantity of heat released during the combustion reaction
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gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
A constant-volume or bomb calorimeter would be used to measure the heat released when a match burns The match would be ignited in the chamber By measuring the temperature increase in the water and using the equation q = ndashm C ΔT the heat released q can be calculated
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gtgt
When 250 mL of water containing 0025 mol HCl at 250degC is added to 250 mL of water containing 0025 mol NaOH at 250degC in a foam-cup calorimeter a reaction occurs Calculate the enthalpy change (in kJ) during this reaction if the highest temperature observed is 320degC Assume that the densities of the solutions are 100 gmL and the volume of the final solution is equal to the sum of the volumes of the reacting solutions
Sample Problem 173Sample Problem 173
Enthalpy Change in a Calorimetry Experiment
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gtgt
Analyze List the knowns and the unknown1
bull Use dimensional analysis to determine the mass of the water
bull You must also calculate ΔT
bull Use ΔH = ndashqsurr = ndashm C ΔT to solve for ΔH
Sample Problem 173Sample Problem 173
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gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
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gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
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gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
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gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
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gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
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gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
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gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
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32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
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gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
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gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
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gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
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gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
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gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
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gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
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gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
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45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
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gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
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gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
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gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
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gtgt
END OF 172END OF 172
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
2
gtgt
How can you measure the amount of heat released when a match burns
CHEMISTRY amp YOUCHEMISTRY amp YOU
Remember The concept of specific heat allows you to measure heat flow in chemical and physical processes
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
3
gtgt CalorimetryCalorimetry
Calorimetry
How can you measure the change in enthalpy of a reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
4
gtgt CalorimetryCalorimetry
Calorimetry is the measurement of the heat flow into or out of a system for chemical and physical processes
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
5
gtgt
Calorimetry is the measurement of the heat flow into or out of a system for chemical and physical processesbull In a calorimetry experiment involving an
endothermic process the heat absorbed by the system is equal to the heat released by its surroundings
bull In an exothermic process the heat released by the system is equal to the heat absorbed by its surroundings
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
6
gtgt
Calorimetry is the measurement of the heat flow into or out of a system for chemical and physical processesbull The insulated device used to measure the
absorption or release of heat in chemical or physical processes is called a calorimeter
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
7
gtgt
Constant-Pressure Calorimeters
Foam cups can be used as simple calorimeters because they do not let much heat in or out
bull Most chemical reactions and physical changes carried out in the laboratory are open to the atmosphere and thus occur at constant pressure
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
8
gtgt
Constant-Pressure Calorimeters
The enthalpy (H) of a system accounts for the heat flow of the system at constant pressure
bull The heat absorbed or released by a reaction at constant pressure is the same as the change in enthalpy symbolized as ΔH
CalorimetryCalorimetry
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
9
gtgt
Constant-Pressure Calorimeters
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at constant pressure
bull In this textbook the terms heat and enthalpy change are used interchangeably
bull In other words q = ΔH
CalorimetryCalorimetry
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
10
gtgt
Constant-Pressure Calorimeters
bull To measure the enthalpy change for a reaction in aqueous solution in a foam cup calorimeter dissolve the reacting chemicals (the system) in known volumes of water (the surroundings)
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
11
gtgt
Constant-Pressure Calorimeters
bull Measure the initial temperature of each solution and mix the solutions in the foam cup
bull After the reaction is complete measure the final temperature of the mixed solutions
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
12
gtgt
Constant-Pressure Calorimeters
You can calculate the heat absorbed or released by the surroundings (qsurr) using the formula for the specific heat the initial and final temperatures and the heat capacity of water
qsurr = m C ΔT
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
13
gtgt
Constant-Pressure Calorimeters
qsurr = m C ΔT
bull m is the mass of the water
bull C is the specific heat of water
bull ΔT = Tf ndash Ti
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
14
gtgt
Constant-Pressure Calorimeters
The heat absorbed by the surroundings is equal to but has the opposite sign of the heat released by the system
qsurr = ndashqsys
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
15
gtgt
Constant-Pressure Calorimeters
The enthalpy change for the reaction (ΔH) can be written as follows
qsys = ΔH = ndashqsurr = ndashm C ΔT
bull The sign of ΔH is positive for an endothermic reaction and negative for an exothermic reaction
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
16
gtgt
Constant-Volume Calorimeters
Calorimetry experiments can also be performed at a constant volume using a device called a bomb calorimeter
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
17
gtgt
Constant-Volume CalorimetersIn a bomb calorimeter a sample of a compound is burned in a constant-volume chamber in the presence of oxygen at high pressure
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
18
gtgt CalorimetryCalorimetry
Constant-Volume Calorimetersbull The heat that is
released warms the water surrounding the chamber
bull By measuring the temperature increase of the water it is possible to calculate the quantity of heat released during the combustion reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
19
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
20
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
A constant-volume or bomb calorimeter would be used to measure the heat released when a match burns The match would be ignited in the chamber By measuring the temperature increase in the water and using the equation q = ndashm C ΔT the heat released q can be calculated
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
21
gtgt
When 250 mL of water containing 0025 mol HCl at 250degC is added to 250 mL of water containing 0025 mol NaOH at 250degC in a foam-cup calorimeter a reaction occurs Calculate the enthalpy change (in kJ) during this reaction if the highest temperature observed is 320degC Assume that the densities of the solutions are 100 gmL and the volume of the final solution is equal to the sum of the volumes of the reacting solutions
Sample Problem 173Sample Problem 173
Enthalpy Change in a Calorimetry Experiment
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22
gtgt
Analyze List the knowns and the unknown1
bull Use dimensional analysis to determine the mass of the water
bull You must also calculate ΔT
bull Use ΔH = ndashqsurr = ndashm C ΔT to solve for ΔH
Sample Problem 173Sample Problem 173
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23
gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
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25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
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26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
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27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
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39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
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44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
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47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
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48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
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52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
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53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
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54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
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55
gtgt
END OF 172END OF 172
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3
gtgt CalorimetryCalorimetry
Calorimetry
How can you measure the change in enthalpy of a reaction
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4
gtgt CalorimetryCalorimetry
Calorimetry is the measurement of the heat flow into or out of a system for chemical and physical processes
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
5
gtgt
Calorimetry is the measurement of the heat flow into or out of a system for chemical and physical processesbull In a calorimetry experiment involving an
endothermic process the heat absorbed by the system is equal to the heat released by its surroundings
bull In an exothermic process the heat released by the system is equal to the heat absorbed by its surroundings
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
6
gtgt
Calorimetry is the measurement of the heat flow into or out of a system for chemical and physical processesbull The insulated device used to measure the
absorption or release of heat in chemical or physical processes is called a calorimeter
CalorimetryCalorimetry
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7
gtgt
Constant-Pressure Calorimeters
Foam cups can be used as simple calorimeters because they do not let much heat in or out
bull Most chemical reactions and physical changes carried out in the laboratory are open to the atmosphere and thus occur at constant pressure
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
8
gtgt
Constant-Pressure Calorimeters
The enthalpy (H) of a system accounts for the heat flow of the system at constant pressure
bull The heat absorbed or released by a reaction at constant pressure is the same as the change in enthalpy symbolized as ΔH
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
9
gtgt
Constant-Pressure Calorimeters
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at constant pressure
bull In this textbook the terms heat and enthalpy change are used interchangeably
bull In other words q = ΔH
CalorimetryCalorimetry
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10
gtgt
Constant-Pressure Calorimeters
bull To measure the enthalpy change for a reaction in aqueous solution in a foam cup calorimeter dissolve the reacting chemicals (the system) in known volumes of water (the surroundings)
CalorimetryCalorimetry
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11
gtgt
Constant-Pressure Calorimeters
bull Measure the initial temperature of each solution and mix the solutions in the foam cup
bull After the reaction is complete measure the final temperature of the mixed solutions
CalorimetryCalorimetry
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12
gtgt
Constant-Pressure Calorimeters
You can calculate the heat absorbed or released by the surroundings (qsurr) using the formula for the specific heat the initial and final temperatures and the heat capacity of water
qsurr = m C ΔT
CalorimetryCalorimetry
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13
gtgt
Constant-Pressure Calorimeters
qsurr = m C ΔT
bull m is the mass of the water
bull C is the specific heat of water
bull ΔT = Tf ndash Ti
CalorimetryCalorimetry
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14
gtgt
Constant-Pressure Calorimeters
The heat absorbed by the surroundings is equal to but has the opposite sign of the heat released by the system
qsurr = ndashqsys
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
15
gtgt
Constant-Pressure Calorimeters
The enthalpy change for the reaction (ΔH) can be written as follows
qsys = ΔH = ndashqsurr = ndashm C ΔT
bull The sign of ΔH is positive for an endothermic reaction and negative for an exothermic reaction
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
16
gtgt
Constant-Volume Calorimeters
Calorimetry experiments can also be performed at a constant volume using a device called a bomb calorimeter
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
17
gtgt
Constant-Volume CalorimetersIn a bomb calorimeter a sample of a compound is burned in a constant-volume chamber in the presence of oxygen at high pressure
CalorimetryCalorimetry
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18
gtgt CalorimetryCalorimetry
Constant-Volume Calorimetersbull The heat that is
released warms the water surrounding the chamber
bull By measuring the temperature increase of the water it is possible to calculate the quantity of heat released during the combustion reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
19
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
20
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
A constant-volume or bomb calorimeter would be used to measure the heat released when a match burns The match would be ignited in the chamber By measuring the temperature increase in the water and using the equation q = ndashm C ΔT the heat released q can be calculated
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
21
gtgt
When 250 mL of water containing 0025 mol HCl at 250degC is added to 250 mL of water containing 0025 mol NaOH at 250degC in a foam-cup calorimeter a reaction occurs Calculate the enthalpy change (in kJ) during this reaction if the highest temperature observed is 320degC Assume that the densities of the solutions are 100 gmL and the volume of the final solution is equal to the sum of the volumes of the reacting solutions
Sample Problem 173Sample Problem 173
Enthalpy Change in a Calorimetry Experiment
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
22
gtgt
Analyze List the knowns and the unknown1
bull Use dimensional analysis to determine the mass of the water
bull You must also calculate ΔT
bull Use ΔH = ndashqsurr = ndashm C ΔT to solve for ΔH
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
23
gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
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36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
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42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
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44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
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45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
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46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
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53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
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55
gtgt
END OF 172END OF 172
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4
gtgt CalorimetryCalorimetry
Calorimetry is the measurement of the heat flow into or out of a system for chemical and physical processes
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
5
gtgt
Calorimetry is the measurement of the heat flow into or out of a system for chemical and physical processesbull In a calorimetry experiment involving an
endothermic process the heat absorbed by the system is equal to the heat released by its surroundings
bull In an exothermic process the heat released by the system is equal to the heat absorbed by its surroundings
CalorimetryCalorimetry
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6
gtgt
Calorimetry is the measurement of the heat flow into or out of a system for chemical and physical processesbull The insulated device used to measure the
absorption or release of heat in chemical or physical processes is called a calorimeter
CalorimetryCalorimetry
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7
gtgt
Constant-Pressure Calorimeters
Foam cups can be used as simple calorimeters because they do not let much heat in or out
bull Most chemical reactions and physical changes carried out in the laboratory are open to the atmosphere and thus occur at constant pressure
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
8
gtgt
Constant-Pressure Calorimeters
The enthalpy (H) of a system accounts for the heat flow of the system at constant pressure
bull The heat absorbed or released by a reaction at constant pressure is the same as the change in enthalpy symbolized as ΔH
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
9
gtgt
Constant-Pressure Calorimeters
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at constant pressure
bull In this textbook the terms heat and enthalpy change are used interchangeably
bull In other words q = ΔH
CalorimetryCalorimetry
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10
gtgt
Constant-Pressure Calorimeters
bull To measure the enthalpy change for a reaction in aqueous solution in a foam cup calorimeter dissolve the reacting chemicals (the system) in known volumes of water (the surroundings)
CalorimetryCalorimetry
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11
gtgt
Constant-Pressure Calorimeters
bull Measure the initial temperature of each solution and mix the solutions in the foam cup
bull After the reaction is complete measure the final temperature of the mixed solutions
CalorimetryCalorimetry
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12
gtgt
Constant-Pressure Calorimeters
You can calculate the heat absorbed or released by the surroundings (qsurr) using the formula for the specific heat the initial and final temperatures and the heat capacity of water
qsurr = m C ΔT
CalorimetryCalorimetry
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13
gtgt
Constant-Pressure Calorimeters
qsurr = m C ΔT
bull m is the mass of the water
bull C is the specific heat of water
bull ΔT = Tf ndash Ti
CalorimetryCalorimetry
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14
gtgt
Constant-Pressure Calorimeters
The heat absorbed by the surroundings is equal to but has the opposite sign of the heat released by the system
qsurr = ndashqsys
CalorimetryCalorimetry
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15
gtgt
Constant-Pressure Calorimeters
The enthalpy change for the reaction (ΔH) can be written as follows
qsys = ΔH = ndashqsurr = ndashm C ΔT
bull The sign of ΔH is positive for an endothermic reaction and negative for an exothermic reaction
CalorimetryCalorimetry
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16
gtgt
Constant-Volume Calorimeters
Calorimetry experiments can also be performed at a constant volume using a device called a bomb calorimeter
CalorimetryCalorimetry
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17
gtgt
Constant-Volume CalorimetersIn a bomb calorimeter a sample of a compound is burned in a constant-volume chamber in the presence of oxygen at high pressure
CalorimetryCalorimetry
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18
gtgt CalorimetryCalorimetry
Constant-Volume Calorimetersbull The heat that is
released warms the water surrounding the chamber
bull By measuring the temperature increase of the water it is possible to calculate the quantity of heat released during the combustion reaction
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19
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
20
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
A constant-volume or bomb calorimeter would be used to measure the heat released when a match burns The match would be ignited in the chamber By measuring the temperature increase in the water and using the equation q = ndashm C ΔT the heat released q can be calculated
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21
gtgt
When 250 mL of water containing 0025 mol HCl at 250degC is added to 250 mL of water containing 0025 mol NaOH at 250degC in a foam-cup calorimeter a reaction occurs Calculate the enthalpy change (in kJ) during this reaction if the highest temperature observed is 320degC Assume that the densities of the solutions are 100 gmL and the volume of the final solution is equal to the sum of the volumes of the reacting solutions
Sample Problem 173Sample Problem 173
Enthalpy Change in a Calorimetry Experiment
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22
gtgt
Analyze List the knowns and the unknown1
bull Use dimensional analysis to determine the mass of the water
bull You must also calculate ΔT
bull Use ΔH = ndashqsurr = ndashm C ΔT to solve for ΔH
Sample Problem 173Sample Problem 173
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23
gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
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24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
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25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
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26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
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27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
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28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
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31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
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35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
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36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
5
gtgt
Calorimetry is the measurement of the heat flow into or out of a system for chemical and physical processesbull In a calorimetry experiment involving an
endothermic process the heat absorbed by the system is equal to the heat released by its surroundings
bull In an exothermic process the heat released by the system is equal to the heat absorbed by its surroundings
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
6
gtgt
Calorimetry is the measurement of the heat flow into or out of a system for chemical and physical processesbull The insulated device used to measure the
absorption or release of heat in chemical or physical processes is called a calorimeter
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
7
gtgt
Constant-Pressure Calorimeters
Foam cups can be used as simple calorimeters because they do not let much heat in or out
bull Most chemical reactions and physical changes carried out in the laboratory are open to the atmosphere and thus occur at constant pressure
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
8
gtgt
Constant-Pressure Calorimeters
The enthalpy (H) of a system accounts for the heat flow of the system at constant pressure
bull The heat absorbed or released by a reaction at constant pressure is the same as the change in enthalpy symbolized as ΔH
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
9
gtgt
Constant-Pressure Calorimeters
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at constant pressure
bull In this textbook the terms heat and enthalpy change are used interchangeably
bull In other words q = ΔH
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
10
gtgt
Constant-Pressure Calorimeters
bull To measure the enthalpy change for a reaction in aqueous solution in a foam cup calorimeter dissolve the reacting chemicals (the system) in known volumes of water (the surroundings)
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
11
gtgt
Constant-Pressure Calorimeters
bull Measure the initial temperature of each solution and mix the solutions in the foam cup
bull After the reaction is complete measure the final temperature of the mixed solutions
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
12
gtgt
Constant-Pressure Calorimeters
You can calculate the heat absorbed or released by the surroundings (qsurr) using the formula for the specific heat the initial and final temperatures and the heat capacity of water
qsurr = m C ΔT
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
13
gtgt
Constant-Pressure Calorimeters
qsurr = m C ΔT
bull m is the mass of the water
bull C is the specific heat of water
bull ΔT = Tf ndash Ti
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
14
gtgt
Constant-Pressure Calorimeters
The heat absorbed by the surroundings is equal to but has the opposite sign of the heat released by the system
qsurr = ndashqsys
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
15
gtgt
Constant-Pressure Calorimeters
The enthalpy change for the reaction (ΔH) can be written as follows
qsys = ΔH = ndashqsurr = ndashm C ΔT
bull The sign of ΔH is positive for an endothermic reaction and negative for an exothermic reaction
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
16
gtgt
Constant-Volume Calorimeters
Calorimetry experiments can also be performed at a constant volume using a device called a bomb calorimeter
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
17
gtgt
Constant-Volume CalorimetersIn a bomb calorimeter a sample of a compound is burned in a constant-volume chamber in the presence of oxygen at high pressure
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
18
gtgt CalorimetryCalorimetry
Constant-Volume Calorimetersbull The heat that is
released warms the water surrounding the chamber
bull By measuring the temperature increase of the water it is possible to calculate the quantity of heat released during the combustion reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
19
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
20
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
A constant-volume or bomb calorimeter would be used to measure the heat released when a match burns The match would be ignited in the chamber By measuring the temperature increase in the water and using the equation q = ndashm C ΔT the heat released q can be calculated
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21
gtgt
When 250 mL of water containing 0025 mol HCl at 250degC is added to 250 mL of water containing 0025 mol NaOH at 250degC in a foam-cup calorimeter a reaction occurs Calculate the enthalpy change (in kJ) during this reaction if the highest temperature observed is 320degC Assume that the densities of the solutions are 100 gmL and the volume of the final solution is equal to the sum of the volumes of the reacting solutions
Sample Problem 173Sample Problem 173
Enthalpy Change in a Calorimetry Experiment
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22
gtgt
Analyze List the knowns and the unknown1
bull Use dimensional analysis to determine the mass of the water
bull You must also calculate ΔT
bull Use ΔH = ndashqsurr = ndashm C ΔT to solve for ΔH
Sample Problem 173Sample Problem 173
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23
gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
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24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
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25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
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26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
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27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
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28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
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31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
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32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
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33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
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35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
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36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
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37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
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39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
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42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
6
gtgt
Calorimetry is the measurement of the heat flow into or out of a system for chemical and physical processesbull The insulated device used to measure the
absorption or release of heat in chemical or physical processes is called a calorimeter
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
7
gtgt
Constant-Pressure Calorimeters
Foam cups can be used as simple calorimeters because they do not let much heat in or out
bull Most chemical reactions and physical changes carried out in the laboratory are open to the atmosphere and thus occur at constant pressure
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
8
gtgt
Constant-Pressure Calorimeters
The enthalpy (H) of a system accounts for the heat flow of the system at constant pressure
bull The heat absorbed or released by a reaction at constant pressure is the same as the change in enthalpy symbolized as ΔH
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
9
gtgt
Constant-Pressure Calorimeters
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at constant pressure
bull In this textbook the terms heat and enthalpy change are used interchangeably
bull In other words q = ΔH
CalorimetryCalorimetry
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
10
gtgt
Constant-Pressure Calorimeters
bull To measure the enthalpy change for a reaction in aqueous solution in a foam cup calorimeter dissolve the reacting chemicals (the system) in known volumes of water (the surroundings)
CalorimetryCalorimetry
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
11
gtgt
Constant-Pressure Calorimeters
bull Measure the initial temperature of each solution and mix the solutions in the foam cup
bull After the reaction is complete measure the final temperature of the mixed solutions
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
12
gtgt
Constant-Pressure Calorimeters
You can calculate the heat absorbed or released by the surroundings (qsurr) using the formula for the specific heat the initial and final temperatures and the heat capacity of water
qsurr = m C ΔT
CalorimetryCalorimetry
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
13
gtgt
Constant-Pressure Calorimeters
qsurr = m C ΔT
bull m is the mass of the water
bull C is the specific heat of water
bull ΔT = Tf ndash Ti
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
14
gtgt
Constant-Pressure Calorimeters
The heat absorbed by the surroundings is equal to but has the opposite sign of the heat released by the system
qsurr = ndashqsys
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
15
gtgt
Constant-Pressure Calorimeters
The enthalpy change for the reaction (ΔH) can be written as follows
qsys = ΔH = ndashqsurr = ndashm C ΔT
bull The sign of ΔH is positive for an endothermic reaction and negative for an exothermic reaction
CalorimetryCalorimetry
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
16
gtgt
Constant-Volume Calorimeters
Calorimetry experiments can also be performed at a constant volume using a device called a bomb calorimeter
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
17
gtgt
Constant-Volume CalorimetersIn a bomb calorimeter a sample of a compound is burned in a constant-volume chamber in the presence of oxygen at high pressure
CalorimetryCalorimetry
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
18
gtgt CalorimetryCalorimetry
Constant-Volume Calorimetersbull The heat that is
released warms the water surrounding the chamber
bull By measuring the temperature increase of the water it is possible to calculate the quantity of heat released during the combustion reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
19
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
20
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
A constant-volume or bomb calorimeter would be used to measure the heat released when a match burns The match would be ignited in the chamber By measuring the temperature increase in the water and using the equation q = ndashm C ΔT the heat released q can be calculated
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
21
gtgt
When 250 mL of water containing 0025 mol HCl at 250degC is added to 250 mL of water containing 0025 mol NaOH at 250degC in a foam-cup calorimeter a reaction occurs Calculate the enthalpy change (in kJ) during this reaction if the highest temperature observed is 320degC Assume that the densities of the solutions are 100 gmL and the volume of the final solution is equal to the sum of the volumes of the reacting solutions
Sample Problem 173Sample Problem 173
Enthalpy Change in a Calorimetry Experiment
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
22
gtgt
Analyze List the knowns and the unknown1
bull Use dimensional analysis to determine the mass of the water
bull You must also calculate ΔT
bull Use ΔH = ndashqsurr = ndashm C ΔT to solve for ΔH
Sample Problem 173Sample Problem 173
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23
gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
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25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
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27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
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53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
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54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
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55
gtgt
END OF 172END OF 172
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7
gtgt
Constant-Pressure Calorimeters
Foam cups can be used as simple calorimeters because they do not let much heat in or out
bull Most chemical reactions and physical changes carried out in the laboratory are open to the atmosphere and thus occur at constant pressure
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
8
gtgt
Constant-Pressure Calorimeters
The enthalpy (H) of a system accounts for the heat flow of the system at constant pressure
bull The heat absorbed or released by a reaction at constant pressure is the same as the change in enthalpy symbolized as ΔH
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
9
gtgt
Constant-Pressure Calorimeters
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at constant pressure
bull In this textbook the terms heat and enthalpy change are used interchangeably
bull In other words q = ΔH
CalorimetryCalorimetry
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10
gtgt
Constant-Pressure Calorimeters
bull To measure the enthalpy change for a reaction in aqueous solution in a foam cup calorimeter dissolve the reacting chemicals (the system) in known volumes of water (the surroundings)
CalorimetryCalorimetry
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11
gtgt
Constant-Pressure Calorimeters
bull Measure the initial temperature of each solution and mix the solutions in the foam cup
bull After the reaction is complete measure the final temperature of the mixed solutions
CalorimetryCalorimetry
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12
gtgt
Constant-Pressure Calorimeters
You can calculate the heat absorbed or released by the surroundings (qsurr) using the formula for the specific heat the initial and final temperatures and the heat capacity of water
qsurr = m C ΔT
CalorimetryCalorimetry
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13
gtgt
Constant-Pressure Calorimeters
qsurr = m C ΔT
bull m is the mass of the water
bull C is the specific heat of water
bull ΔT = Tf ndash Ti
CalorimetryCalorimetry
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14
gtgt
Constant-Pressure Calorimeters
The heat absorbed by the surroundings is equal to but has the opposite sign of the heat released by the system
qsurr = ndashqsys
CalorimetryCalorimetry
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15
gtgt
Constant-Pressure Calorimeters
The enthalpy change for the reaction (ΔH) can be written as follows
qsys = ΔH = ndashqsurr = ndashm C ΔT
bull The sign of ΔH is positive for an endothermic reaction and negative for an exothermic reaction
CalorimetryCalorimetry
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16
gtgt
Constant-Volume Calorimeters
Calorimetry experiments can also be performed at a constant volume using a device called a bomb calorimeter
CalorimetryCalorimetry
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17
gtgt
Constant-Volume CalorimetersIn a bomb calorimeter a sample of a compound is burned in a constant-volume chamber in the presence of oxygen at high pressure
CalorimetryCalorimetry
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18
gtgt CalorimetryCalorimetry
Constant-Volume Calorimetersbull The heat that is
released warms the water surrounding the chamber
bull By measuring the temperature increase of the water it is possible to calculate the quantity of heat released during the combustion reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
19
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
20
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
A constant-volume or bomb calorimeter would be used to measure the heat released when a match burns The match would be ignited in the chamber By measuring the temperature increase in the water and using the equation q = ndashm C ΔT the heat released q can be calculated
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
21
gtgt
When 250 mL of water containing 0025 mol HCl at 250degC is added to 250 mL of water containing 0025 mol NaOH at 250degC in a foam-cup calorimeter a reaction occurs Calculate the enthalpy change (in kJ) during this reaction if the highest temperature observed is 320degC Assume that the densities of the solutions are 100 gmL and the volume of the final solution is equal to the sum of the volumes of the reacting solutions
Sample Problem 173Sample Problem 173
Enthalpy Change in a Calorimetry Experiment
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
22
gtgt
Analyze List the knowns and the unknown1
bull Use dimensional analysis to determine the mass of the water
bull You must also calculate ΔT
bull Use ΔH = ndashqsurr = ndashm C ΔT to solve for ΔH
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
23
gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
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25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
8
gtgt
Constant-Pressure Calorimeters
The enthalpy (H) of a system accounts for the heat flow of the system at constant pressure
bull The heat absorbed or released by a reaction at constant pressure is the same as the change in enthalpy symbolized as ΔH
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
9
gtgt
Constant-Pressure Calorimeters
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at constant pressure
bull In this textbook the terms heat and enthalpy change are used interchangeably
bull In other words q = ΔH
CalorimetryCalorimetry
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
10
gtgt
Constant-Pressure Calorimeters
bull To measure the enthalpy change for a reaction in aqueous solution in a foam cup calorimeter dissolve the reacting chemicals (the system) in known volumes of water (the surroundings)
CalorimetryCalorimetry
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
11
gtgt
Constant-Pressure Calorimeters
bull Measure the initial temperature of each solution and mix the solutions in the foam cup
bull After the reaction is complete measure the final temperature of the mixed solutions
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
12
gtgt
Constant-Pressure Calorimeters
You can calculate the heat absorbed or released by the surroundings (qsurr) using the formula for the specific heat the initial and final temperatures and the heat capacity of water
qsurr = m C ΔT
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
13
gtgt
Constant-Pressure Calorimeters
qsurr = m C ΔT
bull m is the mass of the water
bull C is the specific heat of water
bull ΔT = Tf ndash Ti
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
14
gtgt
Constant-Pressure Calorimeters
The heat absorbed by the surroundings is equal to but has the opposite sign of the heat released by the system
qsurr = ndashqsys
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
15
gtgt
Constant-Pressure Calorimeters
The enthalpy change for the reaction (ΔH) can be written as follows
qsys = ΔH = ndashqsurr = ndashm C ΔT
bull The sign of ΔH is positive for an endothermic reaction and negative for an exothermic reaction
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
16
gtgt
Constant-Volume Calorimeters
Calorimetry experiments can also be performed at a constant volume using a device called a bomb calorimeter
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
17
gtgt
Constant-Volume CalorimetersIn a bomb calorimeter a sample of a compound is burned in a constant-volume chamber in the presence of oxygen at high pressure
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
18
gtgt CalorimetryCalorimetry
Constant-Volume Calorimetersbull The heat that is
released warms the water surrounding the chamber
bull By measuring the temperature increase of the water it is possible to calculate the quantity of heat released during the combustion reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
19
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
20
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
A constant-volume or bomb calorimeter would be used to measure the heat released when a match burns The match would be ignited in the chamber By measuring the temperature increase in the water and using the equation q = ndashm C ΔT the heat released q can be calculated
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
21
gtgt
When 250 mL of water containing 0025 mol HCl at 250degC is added to 250 mL of water containing 0025 mol NaOH at 250degC in a foam-cup calorimeter a reaction occurs Calculate the enthalpy change (in kJ) during this reaction if the highest temperature observed is 320degC Assume that the densities of the solutions are 100 gmL and the volume of the final solution is equal to the sum of the volumes of the reacting solutions
Sample Problem 173Sample Problem 173
Enthalpy Change in a Calorimetry Experiment
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22
gtgt
Analyze List the knowns and the unknown1
bull Use dimensional analysis to determine the mass of the water
bull You must also calculate ΔT
bull Use ΔH = ndashqsurr = ndashm C ΔT to solve for ΔH
Sample Problem 173Sample Problem 173
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23
gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
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25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
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26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
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27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
9
gtgt
Constant-Pressure Calorimeters
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at constant pressure
bull In this textbook the terms heat and enthalpy change are used interchangeably
bull In other words q = ΔH
CalorimetryCalorimetry
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
10
gtgt
Constant-Pressure Calorimeters
bull To measure the enthalpy change for a reaction in aqueous solution in a foam cup calorimeter dissolve the reacting chemicals (the system) in known volumes of water (the surroundings)
CalorimetryCalorimetry
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
11
gtgt
Constant-Pressure Calorimeters
bull Measure the initial temperature of each solution and mix the solutions in the foam cup
bull After the reaction is complete measure the final temperature of the mixed solutions
CalorimetryCalorimetry
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
12
gtgt
Constant-Pressure Calorimeters
You can calculate the heat absorbed or released by the surroundings (qsurr) using the formula for the specific heat the initial and final temperatures and the heat capacity of water
qsurr = m C ΔT
CalorimetryCalorimetry
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
13
gtgt
Constant-Pressure Calorimeters
qsurr = m C ΔT
bull m is the mass of the water
bull C is the specific heat of water
bull ΔT = Tf ndash Ti
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
14
gtgt
Constant-Pressure Calorimeters
The heat absorbed by the surroundings is equal to but has the opposite sign of the heat released by the system
qsurr = ndashqsys
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
15
gtgt
Constant-Pressure Calorimeters
The enthalpy change for the reaction (ΔH) can be written as follows
qsys = ΔH = ndashqsurr = ndashm C ΔT
bull The sign of ΔH is positive for an endothermic reaction and negative for an exothermic reaction
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
16
gtgt
Constant-Volume Calorimeters
Calorimetry experiments can also be performed at a constant volume using a device called a bomb calorimeter
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
17
gtgt
Constant-Volume CalorimetersIn a bomb calorimeter a sample of a compound is burned in a constant-volume chamber in the presence of oxygen at high pressure
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
18
gtgt CalorimetryCalorimetry
Constant-Volume Calorimetersbull The heat that is
released warms the water surrounding the chamber
bull By measuring the temperature increase of the water it is possible to calculate the quantity of heat released during the combustion reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
19
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
20
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
A constant-volume or bomb calorimeter would be used to measure the heat released when a match burns The match would be ignited in the chamber By measuring the temperature increase in the water and using the equation q = ndashm C ΔT the heat released q can be calculated
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
21
gtgt
When 250 mL of water containing 0025 mol HCl at 250degC is added to 250 mL of water containing 0025 mol NaOH at 250degC in a foam-cup calorimeter a reaction occurs Calculate the enthalpy change (in kJ) during this reaction if the highest temperature observed is 320degC Assume that the densities of the solutions are 100 gmL and the volume of the final solution is equal to the sum of the volumes of the reacting solutions
Sample Problem 173Sample Problem 173
Enthalpy Change in a Calorimetry Experiment
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
22
gtgt
Analyze List the knowns and the unknown1
bull Use dimensional analysis to determine the mass of the water
bull You must also calculate ΔT
bull Use ΔH = ndashqsurr = ndashm C ΔT to solve for ΔH
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
23
gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
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55
gtgt
END OF 172END OF 172
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10
gtgt
Constant-Pressure Calorimeters
bull To measure the enthalpy change for a reaction in aqueous solution in a foam cup calorimeter dissolve the reacting chemicals (the system) in known volumes of water (the surroundings)
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
11
gtgt
Constant-Pressure Calorimeters
bull Measure the initial temperature of each solution and mix the solutions in the foam cup
bull After the reaction is complete measure the final temperature of the mixed solutions
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
12
gtgt
Constant-Pressure Calorimeters
You can calculate the heat absorbed or released by the surroundings (qsurr) using the formula for the specific heat the initial and final temperatures and the heat capacity of water
qsurr = m C ΔT
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
13
gtgt
Constant-Pressure Calorimeters
qsurr = m C ΔT
bull m is the mass of the water
bull C is the specific heat of water
bull ΔT = Tf ndash Ti
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
14
gtgt
Constant-Pressure Calorimeters
The heat absorbed by the surroundings is equal to but has the opposite sign of the heat released by the system
qsurr = ndashqsys
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
15
gtgt
Constant-Pressure Calorimeters
The enthalpy change for the reaction (ΔH) can be written as follows
qsys = ΔH = ndashqsurr = ndashm C ΔT
bull The sign of ΔH is positive for an endothermic reaction and negative for an exothermic reaction
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
16
gtgt
Constant-Volume Calorimeters
Calorimetry experiments can also be performed at a constant volume using a device called a bomb calorimeter
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
17
gtgt
Constant-Volume CalorimetersIn a bomb calorimeter a sample of a compound is burned in a constant-volume chamber in the presence of oxygen at high pressure
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
18
gtgt CalorimetryCalorimetry
Constant-Volume Calorimetersbull The heat that is
released warms the water surrounding the chamber
bull By measuring the temperature increase of the water it is possible to calculate the quantity of heat released during the combustion reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
19
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
20
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
A constant-volume or bomb calorimeter would be used to measure the heat released when a match burns The match would be ignited in the chamber By measuring the temperature increase in the water and using the equation q = ndashm C ΔT the heat released q can be calculated
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
21
gtgt
When 250 mL of water containing 0025 mol HCl at 250degC is added to 250 mL of water containing 0025 mol NaOH at 250degC in a foam-cup calorimeter a reaction occurs Calculate the enthalpy change (in kJ) during this reaction if the highest temperature observed is 320degC Assume that the densities of the solutions are 100 gmL and the volume of the final solution is equal to the sum of the volumes of the reacting solutions
Sample Problem 173Sample Problem 173
Enthalpy Change in a Calorimetry Experiment
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
22
gtgt
Analyze List the knowns and the unknown1
bull Use dimensional analysis to determine the mass of the water
bull You must also calculate ΔT
bull Use ΔH = ndashqsurr = ndashm C ΔT to solve for ΔH
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
23
gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
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11
gtgt
Constant-Pressure Calorimeters
bull Measure the initial temperature of each solution and mix the solutions in the foam cup
bull After the reaction is complete measure the final temperature of the mixed solutions
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
12
gtgt
Constant-Pressure Calorimeters
You can calculate the heat absorbed or released by the surroundings (qsurr) using the formula for the specific heat the initial and final temperatures and the heat capacity of water
qsurr = m C ΔT
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
13
gtgt
Constant-Pressure Calorimeters
qsurr = m C ΔT
bull m is the mass of the water
bull C is the specific heat of water
bull ΔT = Tf ndash Ti
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
14
gtgt
Constant-Pressure Calorimeters
The heat absorbed by the surroundings is equal to but has the opposite sign of the heat released by the system
qsurr = ndashqsys
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
15
gtgt
Constant-Pressure Calorimeters
The enthalpy change for the reaction (ΔH) can be written as follows
qsys = ΔH = ndashqsurr = ndashm C ΔT
bull The sign of ΔH is positive for an endothermic reaction and negative for an exothermic reaction
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
16
gtgt
Constant-Volume Calorimeters
Calorimetry experiments can also be performed at a constant volume using a device called a bomb calorimeter
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
17
gtgt
Constant-Volume CalorimetersIn a bomb calorimeter a sample of a compound is burned in a constant-volume chamber in the presence of oxygen at high pressure
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
18
gtgt CalorimetryCalorimetry
Constant-Volume Calorimetersbull The heat that is
released warms the water surrounding the chamber
bull By measuring the temperature increase of the water it is possible to calculate the quantity of heat released during the combustion reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
19
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
20
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
A constant-volume or bomb calorimeter would be used to measure the heat released when a match burns The match would be ignited in the chamber By measuring the temperature increase in the water and using the equation q = ndashm C ΔT the heat released q can be calculated
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
21
gtgt
When 250 mL of water containing 0025 mol HCl at 250degC is added to 250 mL of water containing 0025 mol NaOH at 250degC in a foam-cup calorimeter a reaction occurs Calculate the enthalpy change (in kJ) during this reaction if the highest temperature observed is 320degC Assume that the densities of the solutions are 100 gmL and the volume of the final solution is equal to the sum of the volumes of the reacting solutions
Sample Problem 173Sample Problem 173
Enthalpy Change in a Calorimetry Experiment
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22
gtgt
Analyze List the knowns and the unknown1
bull Use dimensional analysis to determine the mass of the water
bull You must also calculate ΔT
bull Use ΔH = ndashqsurr = ndashm C ΔT to solve for ΔH
Sample Problem 173Sample Problem 173
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23
gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
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25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
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27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
12
gtgt
Constant-Pressure Calorimeters
You can calculate the heat absorbed or released by the surroundings (qsurr) using the formula for the specific heat the initial and final temperatures and the heat capacity of water
qsurr = m C ΔT
CalorimetryCalorimetry
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
13
gtgt
Constant-Pressure Calorimeters
qsurr = m C ΔT
bull m is the mass of the water
bull C is the specific heat of water
bull ΔT = Tf ndash Ti
CalorimetryCalorimetry
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
14
gtgt
Constant-Pressure Calorimeters
The heat absorbed by the surroundings is equal to but has the opposite sign of the heat released by the system
qsurr = ndashqsys
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
15
gtgt
Constant-Pressure Calorimeters
The enthalpy change for the reaction (ΔH) can be written as follows
qsys = ΔH = ndashqsurr = ndashm C ΔT
bull The sign of ΔH is positive for an endothermic reaction and negative for an exothermic reaction
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
16
gtgt
Constant-Volume Calorimeters
Calorimetry experiments can also be performed at a constant volume using a device called a bomb calorimeter
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
17
gtgt
Constant-Volume CalorimetersIn a bomb calorimeter a sample of a compound is burned in a constant-volume chamber in the presence of oxygen at high pressure
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
18
gtgt CalorimetryCalorimetry
Constant-Volume Calorimetersbull The heat that is
released warms the water surrounding the chamber
bull By measuring the temperature increase of the water it is possible to calculate the quantity of heat released during the combustion reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
19
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
20
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
A constant-volume or bomb calorimeter would be used to measure the heat released when a match burns The match would be ignited in the chamber By measuring the temperature increase in the water and using the equation q = ndashm C ΔT the heat released q can be calculated
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
21
gtgt
When 250 mL of water containing 0025 mol HCl at 250degC is added to 250 mL of water containing 0025 mol NaOH at 250degC in a foam-cup calorimeter a reaction occurs Calculate the enthalpy change (in kJ) during this reaction if the highest temperature observed is 320degC Assume that the densities of the solutions are 100 gmL and the volume of the final solution is equal to the sum of the volumes of the reacting solutions
Sample Problem 173Sample Problem 173
Enthalpy Change in a Calorimetry Experiment
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
22
gtgt
Analyze List the knowns and the unknown1
bull Use dimensional analysis to determine the mass of the water
bull You must also calculate ΔT
bull Use ΔH = ndashqsurr = ndashm C ΔT to solve for ΔH
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
23
gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
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55
gtgt
END OF 172END OF 172
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
13
gtgt
Constant-Pressure Calorimeters
qsurr = m C ΔT
bull m is the mass of the water
bull C is the specific heat of water
bull ΔT = Tf ndash Ti
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
14
gtgt
Constant-Pressure Calorimeters
The heat absorbed by the surroundings is equal to but has the opposite sign of the heat released by the system
qsurr = ndashqsys
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
15
gtgt
Constant-Pressure Calorimeters
The enthalpy change for the reaction (ΔH) can be written as follows
qsys = ΔH = ndashqsurr = ndashm C ΔT
bull The sign of ΔH is positive for an endothermic reaction and negative for an exothermic reaction
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
16
gtgt
Constant-Volume Calorimeters
Calorimetry experiments can also be performed at a constant volume using a device called a bomb calorimeter
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
17
gtgt
Constant-Volume CalorimetersIn a bomb calorimeter a sample of a compound is burned in a constant-volume chamber in the presence of oxygen at high pressure
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
18
gtgt CalorimetryCalorimetry
Constant-Volume Calorimetersbull The heat that is
released warms the water surrounding the chamber
bull By measuring the temperature increase of the water it is possible to calculate the quantity of heat released during the combustion reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
19
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
20
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
A constant-volume or bomb calorimeter would be used to measure the heat released when a match burns The match would be ignited in the chamber By measuring the temperature increase in the water and using the equation q = ndashm C ΔT the heat released q can be calculated
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
21
gtgt
When 250 mL of water containing 0025 mol HCl at 250degC is added to 250 mL of water containing 0025 mol NaOH at 250degC in a foam-cup calorimeter a reaction occurs Calculate the enthalpy change (in kJ) during this reaction if the highest temperature observed is 320degC Assume that the densities of the solutions are 100 gmL and the volume of the final solution is equal to the sum of the volumes of the reacting solutions
Sample Problem 173Sample Problem 173
Enthalpy Change in a Calorimetry Experiment
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
22
gtgt
Analyze List the knowns and the unknown1
bull Use dimensional analysis to determine the mass of the water
bull You must also calculate ΔT
bull Use ΔH = ndashqsurr = ndashm C ΔT to solve for ΔH
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
23
gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
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55
gtgt
END OF 172END OF 172
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14
gtgt
Constant-Pressure Calorimeters
The heat absorbed by the surroundings is equal to but has the opposite sign of the heat released by the system
qsurr = ndashqsys
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
15
gtgt
Constant-Pressure Calorimeters
The enthalpy change for the reaction (ΔH) can be written as follows
qsys = ΔH = ndashqsurr = ndashm C ΔT
bull The sign of ΔH is positive for an endothermic reaction and negative for an exothermic reaction
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
16
gtgt
Constant-Volume Calorimeters
Calorimetry experiments can also be performed at a constant volume using a device called a bomb calorimeter
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
17
gtgt
Constant-Volume CalorimetersIn a bomb calorimeter a sample of a compound is burned in a constant-volume chamber in the presence of oxygen at high pressure
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
18
gtgt CalorimetryCalorimetry
Constant-Volume Calorimetersbull The heat that is
released warms the water surrounding the chamber
bull By measuring the temperature increase of the water it is possible to calculate the quantity of heat released during the combustion reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
19
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
20
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
A constant-volume or bomb calorimeter would be used to measure the heat released when a match burns The match would be ignited in the chamber By measuring the temperature increase in the water and using the equation q = ndashm C ΔT the heat released q can be calculated
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
21
gtgt
When 250 mL of water containing 0025 mol HCl at 250degC is added to 250 mL of water containing 0025 mol NaOH at 250degC in a foam-cup calorimeter a reaction occurs Calculate the enthalpy change (in kJ) during this reaction if the highest temperature observed is 320degC Assume that the densities of the solutions are 100 gmL and the volume of the final solution is equal to the sum of the volumes of the reacting solutions
Sample Problem 173Sample Problem 173
Enthalpy Change in a Calorimetry Experiment
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22
gtgt
Analyze List the knowns and the unknown1
bull Use dimensional analysis to determine the mass of the water
bull You must also calculate ΔT
bull Use ΔH = ndashqsurr = ndashm C ΔT to solve for ΔH
Sample Problem 173Sample Problem 173
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23
gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
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25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
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26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
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27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
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32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
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35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
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36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
15
gtgt
Constant-Pressure Calorimeters
The enthalpy change for the reaction (ΔH) can be written as follows
qsys = ΔH = ndashqsurr = ndashm C ΔT
bull The sign of ΔH is positive for an endothermic reaction and negative for an exothermic reaction
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
16
gtgt
Constant-Volume Calorimeters
Calorimetry experiments can also be performed at a constant volume using a device called a bomb calorimeter
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
17
gtgt
Constant-Volume CalorimetersIn a bomb calorimeter a sample of a compound is burned in a constant-volume chamber in the presence of oxygen at high pressure
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
18
gtgt CalorimetryCalorimetry
Constant-Volume Calorimetersbull The heat that is
released warms the water surrounding the chamber
bull By measuring the temperature increase of the water it is possible to calculate the quantity of heat released during the combustion reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
19
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
20
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
A constant-volume or bomb calorimeter would be used to measure the heat released when a match burns The match would be ignited in the chamber By measuring the temperature increase in the water and using the equation q = ndashm C ΔT the heat released q can be calculated
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
21
gtgt
When 250 mL of water containing 0025 mol HCl at 250degC is added to 250 mL of water containing 0025 mol NaOH at 250degC in a foam-cup calorimeter a reaction occurs Calculate the enthalpy change (in kJ) during this reaction if the highest temperature observed is 320degC Assume that the densities of the solutions are 100 gmL and the volume of the final solution is equal to the sum of the volumes of the reacting solutions
Sample Problem 173Sample Problem 173
Enthalpy Change in a Calorimetry Experiment
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
22
gtgt
Analyze List the knowns and the unknown1
bull Use dimensional analysis to determine the mass of the water
bull You must also calculate ΔT
bull Use ΔH = ndashqsurr = ndashm C ΔT to solve for ΔH
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
23
gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
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54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
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55
gtgt
END OF 172END OF 172
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16
gtgt
Constant-Volume Calorimeters
Calorimetry experiments can also be performed at a constant volume using a device called a bomb calorimeter
CalorimetryCalorimetry
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17
gtgt
Constant-Volume CalorimetersIn a bomb calorimeter a sample of a compound is burned in a constant-volume chamber in the presence of oxygen at high pressure
CalorimetryCalorimetry
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18
gtgt CalorimetryCalorimetry
Constant-Volume Calorimetersbull The heat that is
released warms the water surrounding the chamber
bull By measuring the temperature increase of the water it is possible to calculate the quantity of heat released during the combustion reaction
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19
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
20
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
A constant-volume or bomb calorimeter would be used to measure the heat released when a match burns The match would be ignited in the chamber By measuring the temperature increase in the water and using the equation q = ndashm C ΔT the heat released q can be calculated
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
21
gtgt
When 250 mL of water containing 0025 mol HCl at 250degC is added to 250 mL of water containing 0025 mol NaOH at 250degC in a foam-cup calorimeter a reaction occurs Calculate the enthalpy change (in kJ) during this reaction if the highest temperature observed is 320degC Assume that the densities of the solutions are 100 gmL and the volume of the final solution is equal to the sum of the volumes of the reacting solutions
Sample Problem 173Sample Problem 173
Enthalpy Change in a Calorimetry Experiment
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22
gtgt
Analyze List the knowns and the unknown1
bull Use dimensional analysis to determine the mass of the water
bull You must also calculate ΔT
bull Use ΔH = ndashqsurr = ndashm C ΔT to solve for ΔH
Sample Problem 173Sample Problem 173
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23
gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
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25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
17
gtgt
Constant-Volume CalorimetersIn a bomb calorimeter a sample of a compound is burned in a constant-volume chamber in the presence of oxygen at high pressure
CalorimetryCalorimetry
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
18
gtgt CalorimetryCalorimetry
Constant-Volume Calorimetersbull The heat that is
released warms the water surrounding the chamber
bull By measuring the temperature increase of the water it is possible to calculate the quantity of heat released during the combustion reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
19
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
20
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
A constant-volume or bomb calorimeter would be used to measure the heat released when a match burns The match would be ignited in the chamber By measuring the temperature increase in the water and using the equation q = ndashm C ΔT the heat released q can be calculated
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
21
gtgt
When 250 mL of water containing 0025 mol HCl at 250degC is added to 250 mL of water containing 0025 mol NaOH at 250degC in a foam-cup calorimeter a reaction occurs Calculate the enthalpy change (in kJ) during this reaction if the highest temperature observed is 320degC Assume that the densities of the solutions are 100 gmL and the volume of the final solution is equal to the sum of the volumes of the reacting solutions
Sample Problem 173Sample Problem 173
Enthalpy Change in a Calorimetry Experiment
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
22
gtgt
Analyze List the knowns and the unknown1
bull Use dimensional analysis to determine the mass of the water
bull You must also calculate ΔT
bull Use ΔH = ndashqsurr = ndashm C ΔT to solve for ΔH
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
23
gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
18
gtgt CalorimetryCalorimetry
Constant-Volume Calorimetersbull The heat that is
released warms the water surrounding the chamber
bull By measuring the temperature increase of the water it is possible to calculate the quantity of heat released during the combustion reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
19
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
20
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
A constant-volume or bomb calorimeter would be used to measure the heat released when a match burns The match would be ignited in the chamber By measuring the temperature increase in the water and using the equation q = ndashm C ΔT the heat released q can be calculated
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
21
gtgt
When 250 mL of water containing 0025 mol HCl at 250degC is added to 250 mL of water containing 0025 mol NaOH at 250degC in a foam-cup calorimeter a reaction occurs Calculate the enthalpy change (in kJ) during this reaction if the highest temperature observed is 320degC Assume that the densities of the solutions are 100 gmL and the volume of the final solution is equal to the sum of the volumes of the reacting solutions
Sample Problem 173Sample Problem 173
Enthalpy Change in a Calorimetry Experiment
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
22
gtgt
Analyze List the knowns and the unknown1
bull Use dimensional analysis to determine the mass of the water
bull You must also calculate ΔT
bull Use ΔH = ndashqsurr = ndashm C ΔT to solve for ΔH
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
23
gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
19
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
20
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
A constant-volume or bomb calorimeter would be used to measure the heat released when a match burns The match would be ignited in the chamber By measuring the temperature increase in the water and using the equation q = ndashm C ΔT the heat released q can be calculated
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
21
gtgt
When 250 mL of water containing 0025 mol HCl at 250degC is added to 250 mL of water containing 0025 mol NaOH at 250degC in a foam-cup calorimeter a reaction occurs Calculate the enthalpy change (in kJ) during this reaction if the highest temperature observed is 320degC Assume that the densities of the solutions are 100 gmL and the volume of the final solution is equal to the sum of the volumes of the reacting solutions
Sample Problem 173Sample Problem 173
Enthalpy Change in a Calorimetry Experiment
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
22
gtgt
Analyze List the knowns and the unknown1
bull Use dimensional analysis to determine the mass of the water
bull You must also calculate ΔT
bull Use ΔH = ndashqsurr = ndashm C ΔT to solve for ΔH
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
23
gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
20
gtgt
What type of calorimeter would you use to measure the heat released when a match burns Describe the experiment and how you would calculate the heat released
CHEMISTRY amp YOUCHEMISTRY amp YOU
A constant-volume or bomb calorimeter would be used to measure the heat released when a match burns The match would be ignited in the chamber By measuring the temperature increase in the water and using the equation q = ndashm C ΔT the heat released q can be calculated
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
21
gtgt
When 250 mL of water containing 0025 mol HCl at 250degC is added to 250 mL of water containing 0025 mol NaOH at 250degC in a foam-cup calorimeter a reaction occurs Calculate the enthalpy change (in kJ) during this reaction if the highest temperature observed is 320degC Assume that the densities of the solutions are 100 gmL and the volume of the final solution is equal to the sum of the volumes of the reacting solutions
Sample Problem 173Sample Problem 173
Enthalpy Change in a Calorimetry Experiment
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
22
gtgt
Analyze List the knowns and the unknown1
bull Use dimensional analysis to determine the mass of the water
bull You must also calculate ΔT
bull Use ΔH = ndashqsurr = ndashm C ΔT to solve for ΔH
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
23
gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
21
gtgt
When 250 mL of water containing 0025 mol HCl at 250degC is added to 250 mL of water containing 0025 mol NaOH at 250degC in a foam-cup calorimeter a reaction occurs Calculate the enthalpy change (in kJ) during this reaction if the highest temperature observed is 320degC Assume that the densities of the solutions are 100 gmL and the volume of the final solution is equal to the sum of the volumes of the reacting solutions
Sample Problem 173Sample Problem 173
Enthalpy Change in a Calorimetry Experiment
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
22
gtgt
Analyze List the knowns and the unknown1
bull Use dimensional analysis to determine the mass of the water
bull You must also calculate ΔT
bull Use ΔH = ndashqsurr = ndashm C ΔT to solve for ΔH
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
23
gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
22
gtgt
Analyze List the knowns and the unknown1
bull Use dimensional analysis to determine the mass of the water
bull You must also calculate ΔT
bull Use ΔH = ndashqsurr = ndashm C ΔT to solve for ΔH
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
23
gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
23
gtgt
Analyze List the knowns and the unknown1
KNOWNS UNKNOWN
Cwater = 418 J(gdegC)
Vfinal = VHCl + VNaOH
= 250 mL + 250 mL = 500 mL
Ti = 250degC
Tf = 320degC
densitysolution = 100 gmL
ΔH = kJ
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
24
gtgt
First calculate the total mass of the water
Calculate Solve for the unknown2
mwater = 500 mL = 500 g1 mL
100 g
Assume that the densities of the solutions are 100 gmL to find the total mass of the water
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
25
gtgt
Now calculate ΔT
Calculate Solve for the unknown2
ΔT = Tf ndash Ti = 320degC ndash 250degC = 70degC
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
26
gtgt
Use the values for mwater Cwater and ΔT to calculate ΔH
Calculate Solve for the unknown2
Use the relationship 1 kJ = 1000 J to convert your answer from J to kJ
Sample Problem 173Sample Problem 173
ΔH = ndashqsurr = ndashmwater Cwater ΔT
= ndash(500 g)(418 J(goC))(70degC)
= ndash1500 J = ndash15 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
27
gtgt
bull The temperature of the solution increases which means that the reaction is exothermic and thus the sign of ΔH should be negative
bull About 4 J of heat raises the temperature of 1 g of water 1degC so 200 J of heat is required to raise 50 g of water 1degC Raising the temperature of 50 g of water 7degC requires about 1400 J or 14 kJ
bull This estimated answer is very close to the calculated value of ΔH
Evaluate Does the result make sense3
Sample Problem 173Sample Problem 173
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
28
gtgt
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
29
gtgt
ΔH = ndashm C ΔT
= ndash367 g 418 J(gdegC) (87degC ndash 24degC)
= ndash97000 J = ndash97 kJ
The initial temperature of the water in a constant-pressure calorimeter is 24degC A reaction takes place in the calorimeter and the temperature rises to 87degC The calorimeter contains 367 g of water which has a specific heat of 418 J(gdegC) Calculate the enthalpy change during this reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
30
gtgtThermochemical Thermochemical EquationsEquations
Thermochemical Equations
How can you express the enthalpy change for a reaction in a chemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
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172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
31
gtgtThermochemical Thermochemical EquationsEquations
In a chemical equation the enthalpy change for the reaction can be written as either a reactant or a product
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
32
gtgtThermochemical Thermochemical EquationsEquations
In the equation describing the exothermic reaction of calcium oxide and water the enthalpy change can be considered a product
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
Calcium oxide is one of the components of cement
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
33
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s) + 652 kJ
A chemical equation that includes the enthalpy change is called a thermochemical equation
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
34
gtgtThermochemical Thermochemical EquationsEquations
The heat of reaction is the enthalpy change for the chemical equation exactly as it is writtenbull Heats of reaction are reported as ΔH
bull The physical state of the reactants and products must also be given
bull The standard conditions are that the reaction is carried out at 1013 kPa (1 atm) and 25degC
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
35
gtgtThermochemical Thermochemical EquationsEquations
CaO(s) + H2O(l) rarr Ca(OH)2(s)
Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 652 kJ of heat
ΔH = ndash652 kJ
bull In exothermic processes the chemical potential energy of the reactants is higher than the chemical potential energy of the products
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
36
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Baking soda (sodium bicarbonate) decomposes when it is heated This process is endothermic
Heats of Reaction
The carbon dioxide released in the reaction causes muffins to rise while baking
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
37
gtgtThermochemical Thermochemical EquationsEquations
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) + CO2(g)
Heats of Reaction
Remember that ΔH is positive for endothermic reactions Therefore you can write the reaction as follows
2NaHCO3(s) rarr Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
38
gtgtThermochemical Thermochemical EquationsEquations
The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved
bull The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat
bull Therefore the decomposition of 4 mol of the same substance would require twice as much heat or 170 kJ
Heats of Reaction
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
39
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
40
gtgtThermochemical Thermochemical EquationsEquations
Heats of ReactionTo see why the physical state of the reactants and products must be stated compare the following two equations
bull The vaporization of 1 mol of liquid water to water vapor at 25degC requires 440 kJ of heat
H2O(l) rarr H2O(g) ΔH = 440 kJ
difference = 440 kJ
H2O(l) rarr H2(g) + O2(g) ΔH = 2858 kJ 1 2
H2O(g) rarr H2(g) + O2(g) ΔH = 2418 kJ 1 2
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
41
gtgt
Calculate the amount of heat (in kJ) required to decompose 224 mol NaHCO3(s)
Using the Heat of Reaction to Calculate Enthalpy Change
2NaHCO3(s) + 85 kJ rarr Na2CO3(s) + H2O(l) CO2(g)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
42
gtgt
Analyze List the knowns and the unknown1
KNOWNS
UNKNOWN
amount of NaHCO3(s) that decomposes = 224 mol
ΔH = 85 kJ for 2 mol NaHCO3
ΔH = kJ for 224 mol NaHCO3
Use the thermochemical equation to write a conversion factor relating kJ of heat and moles of NaHCO3 Then use the conversion factor to determine ΔH for 224 mol NaHCO3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
43
gtgt
Write the conversion factor relating kJ of heat and moles of NaHCO3
Calculate Solve for the unknown2
The thermochemical equation indicates that 85 kJ are needed to decompose 2 mol NaHCO3(s)
85 kJ2 mol NaHCO3(s)
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
44
gtgt
Using dimensional analysis solve for ΔH
Calculate Solve for the unknown2
Sample Problem 174Sample Problem 174
85 kJ2 mol NaHCO3(s)ΔH = 224 mol NaHCO3(s)
= 95 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
45
gtgt
bull The 85 kJ in the thermochemical equation refers to the decomposition of 2 mol NaHCO3(s)
bull Therefore the decomposition of 224 mol should absorb more heat than 85 kJ
bull The answer of 95 kJ is consistent with this estimate
Evaluate Does the result make sense3
Sample Problem 174Sample Problem 174
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
46
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionThe heat of combustion is the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
47
gtgtThermochemical Thermochemical EquationsEquations
Heats of CombustionSmall amounts of natural gas within crude oil are burned off at oil refineries
bull This is an exothermic reaction
bull Burning 1 mol of methane releases 890 kJ of heat
bull The heat of combustion (ΔH) for this reaction is ndash890 kJ per mole of methane burned
CH4(g) + 2O2(g) rarr CO2(g) + 2H2O(l) + 890 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
48
gtgt
Like other heats of reaction heats of combustion are reported as the enthalpy changes when the reactions are carried out at 1013 kPa and 25degC
Interpret DataInterpret Data
Heats of Combustion at 25degC
Substance Formula ΔH (kJmol)
Hydrogen H2(g) ndash286
CarbonC(s graphite)
ndash394
Methane CH4(g) ndash890
Acetylene C2H2(g) ndash1300
Ethanol C2H6O(l) ndash1368
Propane C3H8(g) ndash2220
Glucose C6H12O6(s) ndash2808
Octane C8H18(l) ndash5471
Sucrose C12H22O11(s) ndash5645
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
49
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
50
gtgt
Which of the following thermochemical equations represents an endothermic reaction
A Cgraphite(s) + 2 kJ Cdiamond(s)
B 2H2(g) + O2(g) 2H2O + 4836 kJ
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
51
gtgtKey Concepts amp Key Key Concepts amp Key EquationEquation
The value of ΔH of a reaction can be determined by measuring the heat flow of the reaction at a constant pressure
In a chemical equation the enthalpy change for the reaction can be written as either a reaction or a product
qsys = ΔH = ndashqsurr = ndashm C ΔT
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
52
gtgt Glossary TermsGlossary Terms
bull calorimetry the precise measurement of heat flow out of a system for chemical and physical processes
bull calorimeter an insulated device used to measure the absorption or release of heat in chemical or physical processes
bull enthalpy (H) the heat content of a system at constant pressure
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
53
gtgt Glossary TermsGlossary Terms
bull thermochemical equation a chemical equation that includes the enthalpy change
bull heat of reaction the enthalpy change for a chemical equation exactly as it is written
bull heat of combustion the heat of reaction for the complete burning of one mole of a substance
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
54
gtgt
The heat of reaction or process can be determined experimentally through calorimetry
BIG IDEABIG IDEA
Matter and Energy
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172
Copyright copy Pearson Education Inc or its affiliates All Rights Reserved
172 Measuring and Expressing 172 Measuring and Expressing Enthalpy Changes Enthalpy Changes
55
gtgt
END OF 172END OF 172