topic: thermodynamics do now: packet p.1. every physical or chemical change is accompanied by energy...
TRANSCRIPT
Topic: Thermodynamics
Do Now: packet p.1
Every physical or chemical change is accompanied by
energy change
Energy released = _________________
Energy absorbed = _______________
exothermic
endothermic
G
L
S
• Thermodynamics is the study of entropy and enthalpy changes that accompany chemical reactions
Thermodynamics Tells us if a reaction will occur
The total amount of energy a substance contains depends on many factors, some of which are not totally understood…it’s impossible to know the total heat content of a substance.
So scientists measure ΔH
H = enthalpy = the heat content of a system at constant pressure. It describes chemical PE stored in matter
ΔH = enthalpy (heat) of reactionΔH = Hproducts – Hreactants
--the difference between the enthalpy(heat) of the substances that exist at the end of the reaction and the enthalpy(heat) of the substances that exist at the beginning of the reaction
Thermochemical Equations
• balanced chemical equation• shows physical state of all reactants &
products
• gives energy change – It can be written 2 ways
• energy term can be written as reactant or product
OR• H is given right after equation
4Fe(s) + 3O2(g) 2Fe2O3(s) + 1625 kJ
OR
4Fe(s) + 3O2(g) 2Fe2O3(s)
H = -1625 kJ
NH4NO3(s) + 27 kJ NH4+(aq) + NO3
-(aq)
OR
NH4NO3(s) NH4+(aq) + NO3
-(aq)
H = 27 kJ
If ΔH is negative…- ΔH = exothermic
- Hproducts < Hreactants
- PE of Products < PE of Reactant- Example: 4Fe(s) + 3O2(g) 2Fe2O3(s) + 1625 kJ
- ΔH = -1625kJ
If ΔH is positive…+ ΔH = endothermic
- Hproducts > Hreactants
- PE of Products > PE of Reactant
Example: NH4NO3(s) + 27 kJ NH4+(aq) + NO3
-(aq)- ΔH = +27kJ
Universe
Environment
System A
B
Since energy is conversed…the system changes in one direction and the surrounding have to change in the opposite direction
A. Reaction is Exothermic, environment gets _________________
B. Reaction is Endothermic, environment gets _________________
warmer
colder
For any reaction occurring at constant pressure ΔH = Q
• Q = mCT– Q = Energy change
– m = mass of water
– C = specific heat of water
– T = temperature change = Tf – Ti
Since there are different types of reactions, you have various ΔH’s
• ΔHcomb = enthalpy (heat) of combustion – the enthalpy change for the complete bunring of one mole of the substance
• ΔHformation = enthalpy (heat) of formation – the enthalpy change for the formation of a compound from its constituent elements
• ΔHsolution = enthalpy (heat) of solution – the enthalpy change when 1 mole of an ionic substance is dissolved in water.
Look at Table I: Heats of ReactionLets label the various types from above
• Rxns 1-6: combustion rxns
-H = heat of combustion
• Rxns 7-18: formation (synthesis) rxns
– Substance is formed from its elements
– H = heat of formation
• Rxns 19-24: dissolving equations
– H = heat of solution
Table I
Many other processes other than chemical reactions absorb or release energy
like, Changes of state
Hvaporization = molar heat of vaporization
= amount of heat required to vaporize one mole of a liquid
Hfusion = molar heat of fusion
= amount of heat required to melt one moles of a solid
Energy depends on amount
• Remember – it takes more energy to heat up water in the ocean than to make a cup of tea
CH4(g) + 2O2(g) CO2(g) + 2H2O (l) H = -890.4 kJ
1 mole of methane + 2 mole of oxygen →
1 mole of carbon dioxide gas & 2 moles of liquid water
reaction is ____________ (negative sign for ΔH)
890.4 kJ energy released per mole of CH4(g) burned
exothermic
What would happen if we had 2 moles of methane?
Twice as much energy would be released
2 x 890.4 kJ = 1780.8 kJ will be released
Reactions: Energy depends on direction too!
• N2(g) + 3H2(g) 2NH3(g) H = -91.8 kJ
• 2NH3(g) N2(g) + 3H2(g) H = _______
If reverse equation, reverse sign of H
91.8 kJ
If we can’t calc. H for one individual substance how are we
able to calc. ΔH???!
FYI: Hess’s Law(not on regents)
Can add 2 or more equations by adding the H’s
Enables you to calculate H for # of rxns
Say you’re interested in
2S(s) + 3O2(g) 2SO3(g)
2S(s) + 3O2(g) 2SO3(g)Have H’s for the following:
a) S(s) + O2(g) SO2(g) H = -297 kJ
b) 2SO3(g) 2SO2(g) + O2(g) H = 198 kJ
2 2 2
2SO2(g) + O2(g) 2SO3(g) H = -198 kJ
H = -594KJ + (- 198kJ) H = -792 kJ
x (2)