ib dp1 chemistry energetics
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IB DP1 ChemistryEnergetics
Why do chemical reactions get hot or cold?
Topic 5: Energetics (8 hours)5.1 Exothermic and endothermic reactions5.1.1 Define the terms exothermic reaction, endothermic reaction and standard enthalpy change of reaction ( ∆HO ) .5.1.2 State that combustion and neutralization are exothermic processes.5.1.3 Apply the relationship between temperature change, enthalpy change and the classification of a reaction as endothermic or exothermic.5.1.4 Deduce, from an enthalpy level diagram, the relative stabilities of reactants and products, and the sign of the enthalpy change for the reaction.
5.2 Calculation of enthalpy changes5.2.1 Calculate the heat energy change when the temperature of a pure substance is changed.5.2.2 Design suitable experimental procedures for measuring the heat energy changes of reactions.
5.2.3 Calculate the enthalpy change for a reaction using experimental data on temperature changes, quantities of reactants and mass of water.5.2.4 Evaluate the results of experiments to determine enthalpy changes.
5.3 Hess’s law5.3.1 Determine the enthalpy change of a reaction that is the sum of two or three reactions with known enthalpy changes.5.4 Bond enthalpies5.4.1 Define the term average bond enthalpy.5.4.2 Explain, in terms of average bond enthalpies, why some reactions are exothermic and others are endothermic.
Thermochemistry Study of energy changes during chemical
reactions Heat, light, mechanical energy …..
mix ammonium nitrate and water
burn ethanol
See Think Wonder
Why do chemical reactions get hot (or cold)?
What is the difference between energy and enthalpy? What is the difference between temperature and heat? How much heat does it take to increase the
temperature of a substance? What is the difference between enthalpy change and
standard enthalpy change? How is calorimetry used to measure enthalpy changes? How is standard enthalpy change calculated from a
temperature change?
Exothermic and endothermic reactions
Ammonium nitrate and water Iron and oxygen
Cold packA. The temperature of the cold pack decreases
during the reactionB. The temperature of the cold pack increases
during the reactionC. The cold pack transfers cold to the person
touching itD. Heat is taken in from the person to the cold packE. The cold pack has less energy and lower
enthalpy after it is used
Exothermic reactions examples
NaOH(s) + H2O NaOH(aq) + heatExothermic
HCl + NaOH NaCl + H2O + heatNeutralisation
Wood + O2 CO2 + H2O + heat Combustion
Endothermic reaction example
Ba(OH)2(s) + 2 NH4SCN(s) + heat
Ba2+(aq) + 2 SCN-
(aq) + 2 H2O(l) + NH3(aq)
Endothermic
Endothermic or exothermic?
In chemical reactions bonds break and formdifferent amounts of energy are in the bonds before and after the reaction Exothermic reaction: less energy is in the bonds after
the reaction: heat is produced Endothermic reaction = energy is needed
Distribution of speeds of particles
number of particles
speed
Temperature- average KE per particle
higher average speed higher temperature
more particles at same average speed same temperature
Distribution of speeds
Enthalpy, H Energy stored in chemical bonds of reactants (in
Joules) PE and KE of particles + energy to make space for
substance
Image: https://en.wikipedia.org/wiki/File:Ammonium_Nitrate.jpg
Exothermic reactionCH4 + 2 O2 CO2 + 2H2O + heat
Energy rich Energy poor
DH = (Energy poor) – (Energy rich) negative value Exothermic reactions: DH < O more stable
productsEndothermic reactions DH > O more reactive
products.
Exothermic reactionsEnthalpy, J
reaction coordinate
reactants
products
∆H
Endothermic reactionsEnthalpy, J
reaction coordinate
reactants
products
∆H
Standard enthalpy change of a reaction
∆H° to compare reactions in kJ/molmeasured at 298K and 1atm
Calculating standard enthalpy changes
2 Mg + O2 2 MgO DH = -1202 kJ/mol Exothermic The amount of energy released when 0.6 g of Mg is burnt?
Mgm 0.6 gM 24.3 g/moln 0.025 mol
1202*0.025 = 30 kJ
Calculating standard enthalpy change
What is the enthalpy change in kJ per mole if 45kJ are given out when 0.8g of methane is burned?What is the enthalpy change in kJ per mole if 1.6g of methanol is used to heat 200mL water from 20C to 38C?
Using temperature to calculate ∆Hᶱ
Heat energy = mass x specific heat capacity x temperature changeQ = mc∆T
How much energy is in a cracker? 1408kJ per 100grams 7 grams per cracker How much will a cracker increase the
temperature of 100mL of water when we burn it?
Calculating uncertaintiesHow do you calculate uncertainties when: adding or subtracting variables? multiplying or dividing variables?
Calculate the standard enthalpy change for the reaction between hydrochloric acid and sodium hydroxide
To calculate the uncertainty in the standard enthalpy for the reaction between zinc and copper sulphate...
absolute uncertainty in temperature change = percentage uncertainty in temperature change = percentage uncertainty in mass of liquid = percentage uncertainty in specific heat capacity = pecentage uncertainty in enthalpy = percentage uncertainty in number of moles = total percentage uncertainty = total absolute uncertainty in standard enthalpy =
Neutralization- acid-base reactionWrite word and chemical equations for the following reactions: hydrochloric acid + sodium hydroxide sulphuric acid + sodium hydroxide nitric acid + potassium hydroxide
Standard enthalpy of neutralizationH+
(aq) + OH-(aq) H2O(l)
standard enthalpy change of neutralization for a strong acid and base is -55.90 kJ/mol
Bond enthalpyThe enthalpy change when one mole of bonds is formed in the gaseous state:
X (g) + Y(g) X-Y(g)
Forming bonds is exothermic (negative ∆H)Breaking bonds is endothermic (positive ∆H)
Calculate a theoretical standard enthalpy of combustion of methane
Enthalpy of combustionBond Average bond
enthalpy kJ/molC-C 347C=O 746C-H 413O=O 498O-H 464C-O 358
Image: https://en.wikipedia.org/wiki/Burning
How does the theoretical standard enthalpy of combustion depend on the number of carbon atoms for the alkanes?
Compare your answers with experimental values.
Standard enthalpy of combustion of alkanes
C no. n name alkane ΔH1 methane CH4 -8902 ethane C2H6 -15603 propane C3H8 -22194 butane C4H10 -28775 pentane C5H12 -35096 hexane C6H14 -41637 heptane C7H16 -48178 octane C8H18 -5470
name alcohol ΔHcomb
methanol CH3OH -726
ethanol CH3CH2OH -1367
propan-1-ol CH3(CH2)2OH -2021
butan-1-ol CH3(CH2)3OH -2676
pentan-1-ol CH3(CH2)4OH -3329
hexan-1-ol CH3(CH2)5OH -3984
heptan-1-ol CH3(CH2)6OH -4638
Ammonia, NH3 Draw a Lewis diagram of the molecule State the bond angles and shape State whether the N-H bonds are polar, and
whether the molecule is polar Calculate the standard enthalpy of formation from
data booklet data
Standard enthalpy change of formation ΔHfᶱ
the standard enthalpy change when a compound is formed from its elements CH4 -74.4kJmol-1 CO2 -393.5kJ/mol-1 H2O -285.8kJ/mol-1
Formation of ammoniaN2 + 3 H2 2 NH3
N N triple bond 944kJmol-1H-H 436 kJmol-1N-H 388 kJmol-1
DH = (cost of bond breaking) – (gained for bond forming) =( 944 + 3*436) – (2*3*388) = -76 kJmol-1
Exothermic
Hess’s Law conservation of energy applied to chemistry total enthalpy change is the same whatever the
route of a chemical reaction
Combustion of carbon to form Carbon dioxide
C + ½ O2 CO DH1 = -110kJmol-1
CO +½ O2 CO2 DH2 = -283kJmol-1
C + O2 CO2 DH3 = DH1+DH2 =
Plan investigation…
Links Ionic bonding
http://www.teachersdomain.org/asset/lsps07_int_ionicbonding/
Covalent bonding http://www.teachersdomain.org/asset/lsps07_int_covalentbond/
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