Chapt. 10 Spontaneity, Entropy & Free Energy

1. Spontaneous Processes

2. Entropy Changes in Chemical Reactions

2.1. dSsurr: determined primarily by heat flow dSsys: determined by differences in # of positional randomness of products & reactants

3. Free Energy and Chemical Reactions

3.1. Three Ways to Compute DGrxn

3.1.1. From dHo & dSo

3.1.2. Hess' Law

3.1.3. From dGform

4. Reversible and Irreversible Processes: A Summary

5. Free Energy and Work

6. Free Energy and Equilibrium

6.1. dGo=-RTlnK

7. The Dependence of Free Energy on Pressure

7.1. dG=dGo+RTln(Q)

8. 3rd Law: S of all substances is 0 at 0K

9. T-dependence of K: van't Hoff Equation: Rln(K)=-dH/T+dS

10. Max useful work="free" energy

11. The Isothermal Expansion and Compression of an Ideal Gas

12. Entropy and Physical Changes

13. The Definition of Entropy

14. Entropy and the Second Law of Thermodynamics

15. The Effect of Temperature on Spontaneity

15.1. Exothermicity most important at low T

16. Free Energy

16.1. dSuniv=-dG/T

16.2. dG=dH-TdS

17. The change in the entropy of the universe for a given process is a measure of the driving force behind that process

18. Isothermal expansion of an ideal gas against a vacuum involves no change in energy, work or heatflow

19. Reversible processes yield maximum work & heat

19.1. Reversible Work

19.2. Reversible heat

20. Only when a cyclic process is done in infinite number of steps is the universe the same at the beginning & end of the process.

21. All real processes are thermodynamically irreversible

22. S changes in surroundings usually due to heat flow

22.1. dSsurr=-dH/T

23. ENTROPY BUDGET: dSuniv=dSsys+dSsurr=-dG/T