1. Ch. 20: Entropy and Free Energy
Thermodynamics: the science of energy transfer
Objective: To learn how chemists predict when reactions will be product-favored vs. when they will be reactant-favored

2. Section 20.1
Ø Thermodynamics tells us NOTHING about the rate of reaction.
The study of rates and why some reactions are fast and others are slow is called kinetics (Ch. 15.)

3. Section 20.2 Entropy Entropy, S: Measure of dispersal or disorder.
Ø      Can be measured with a calorimeter. Assumes in a perfect crystal at absolute zero, no disorder and S = 0.
Ø      If temperature change is very small, can calculate entropy change, DS = q/T (heat absorbed / T at which change occurs)
Ø      Sum of DS can give total entropy at any desired temperature. See Table 20.1

4. Section Entropy
In general, the final state is more probable than the initial one if:
(1)    energy can be dispersed over a greater number of atoms and molecules (hot  cold)
(2)    the atoms and molecules can be more disordered (dissolving, diffusion of gas)

5. Section 20.2 Entropy More specifically,
(1)   if energy and matter are both more dispersed, it is definitely product-favored
(2)   if only energy or matter is dispersed, then quantitative information is necessary to decide which effects are greater
(3)   if neither matter nor energy is more dispersed, then the process will be reactant-favored

6. Entropy Examples (positive DS)
Boiling water
Melting ice
Preparing solutions
CaCO3 (s)  CaO (s) + CO2 (g)

7. Entropy Examples (negative DS)
Molecules of gas collecting
Liquid converting to solid at room temp
2 CO (g) + O2 (g)  2 CO2 (g)
Ag+ (aq) Cl-(aq)  AgCl (s)

8. Entropy Generalizations
Sgas > S liquid > Ssolid
Entropies of more complex molecules are larger than those of simpler molecules (Spropane > Sethane>Smethane)
Entropies of ionic solids are higher when attraction between ions are weaker.
Ø      Entropy usually increases when a pure liquid or solid dissolves in a solvent.
   Entropy increases when a dissolved gas escapes from a solution

9. Laws of Thermodynamics
First law: Total energy of the universe is a constant.
Second law: Total entropy of the universe is always increasing.
Third law: Entropy of a pure, perfectly formed crystalline substance at absolute zero = 0.

10. Calculating DSo system
DSo system =  So (products) -  So (reactants)
Can also relate surroundings to the system!
DSo surroundings = q surroundings / T
= - DHsystem / T

11. Calculating DSo universe
DSo universe = DSo surroundings + DSo system
DSo universe = DHsystem / T + DSo system
Can use 2nd law to predict whether a reaction is product-favored or reactant-favored!
The higher the temperature, the less important the enthalpy term is!

12. Roald Hoffmann (1981 Nobel prize): “One amusing way to describe synthetic chemistry, the making of molecules that is at the intellectual and economic center of chemistry, is that it is the local defeat of entropy.”

13. 20.3 Gibbs Free Energy
DG is a measure of the maximum magnitude of the net useful work that can be obtained from a reaction!

14. 20.3 Gibbs Free Energy DGsystem = - T DSuniverse
= DHsystem - TDSsystem
DGosystem = DHosystem - T DSosystem
DGorxn = DHorxn - T DSorxn

15. 20.3 Gibbs Free Energy
DGosystem or DGorxn If negative, then product-favored. If positive, then reactant-favored.
DGo reaction =  Gfo (products) -  Gfo (reactants)

16. 20.3 Gibbs Free Energy
DG is a measure of the maximum magnitude of the net useful work that can be obtained from a reaction!
Know the meaning of enthalpy-driven vs. entropy-driven reactions.
DGs are additive!

17. 20.4 Thermodynamics and K If not at standard conditions,
DG = DGo + RT ln Q
 (Equilibrium is characterized by the inability to do work.)
At equilibrium, Q = K and DG = O
 Therefore, substituting into previous equation gives 0 = DGo + RT ln K and
DGo = - RT ln K (can use Kp or Kc)

18. 2020.5 Thermodynamics and Time
2020.5      Thermodynamics and Time
First law: Total energy of the universe is a constant.
Second law: Total entropy of the universe is always increasing.
Third law: Entropy of a pure, perfectly formed crystalline substance at absolute zero = 0.
Entropy : time’s arrow
Absolutely MUST learn table in Chapter highlights!

19. 20.4 Thermodynamics and K
Ø      Understand relationship between DGo, K, and product-favored reactions!
DGo< K>1 product-favored
DGo= K=1
DGo> K<1 reactant-favored