1. 11 Entropy and Free Energy How to predict if a reaction can occur, given enough time? THERMODYNAMICS How to predict if a reaction can occur at a reasonable rate? KINETICS

2. 22 Thermodynamics and Kinetics Diamond is thermodynamically favored to convert to graphite, but not kinetically favored. Paper burns — a product-favored reaction. Also kinetically favored once reaction is begun.

3. 33 Spontaneous Reactions In general, spontaneous reactions are exothermic. Fe 2 O 3 (s) + 2 Al(s) ---> 2 Fe(s) + Al 2 O 3 (s) ∆H = - 848 kJ

4. 44 Directionality of Reactions Energy Dispersal Exothermic reactions involve a release of stored chemical potential energy to the surroundings. The stored potential energy starts out in a few molecules but is finally dispersed over a great many molecules. The final state—with energy dispersed—is more probable and makes a reaction spontaneous.

5. 55 Spontaneous Reactions But many spontaneous reactions or processes are endothermic or even have ∆H = 0. NH 4 NO 3 (s) + heat ---> NH 4 NO 3 (aq)

6. 66 How probable is it that reactant molecules will react? PROBABILITY suggests that a spontaneous reaction will result in the dispersal *of energy *or of matter * or of energy & matter. Directionality of Reactions

7. 77 Entropy, S One property common to spontaneous processes is that the final state is more DISORDERED or RANDOM than the original. Spontaneity is related to an increase in randomness. The thermodynamic property related to randomness is ENTROPY, S. Reaction of K with water

8. 88 The entropy of liquid water is greater than the entropy of solid water (ice) at 0˚ C.

9. 99 S (gases) > S (liquids) > S (solids) S o (J/Kmol) H 2 O(liq)69.95 H 2 O(gas)188.8 S o (J/Kmol) H 2 O(liq)69.95 H 2 O(gas)188.8 Entropy, S

10. 1010 Entropy Changes for Phase Changes For a phase change, ∆S = q/T where q = heat transferred in phase change For H 2 O (liq) ---> H 2 O(g) ∆H = q = +40,700 J/mol

11. 1111 Entropy and Temperature S increases slightly with T S increases a large amount with phase changes

12. 1212 Why does the entropy of a substance increases with temperature? Entropy, S

13. 1313 Entropies of ionic solids depend on coulombic attractions. S o (J/Kmol) MgO26.9 NaF51.5 S o (J/Kmol) MgO26.9 NaF51.5 Entropy, S Mg 2+ & O 2- Na + & F -

14. 1414 Increase in molecular complexity generally leads to increase in S. Entropy, S

15. 1515 Entropy usually increases when a pure liquid or solid dissolves in a solvent. Entropy, S

16. 1616 Standard Molar Entropies

17. 1717 Consider 2 H 2 (g) + O 2 (g) ---> 2 H 2 O(liq) ∆S o = 2 S o (H 2 O) - [2 S o (H 2 ) + S o (O 2 )] ∆S o = 2 mol (69.9 J/Kmol) - [2 mol (130.7 J/Kmol) + 1 mol (205.3 J/Kmol)] ∆S o = -326.9 J/K Note that there is a decrease in S because 3 mol of gas give 2 mol of liquid. Calculating ∆S for a Reaction ∆S o =  S o (products) -  S o (reactants)

18. 1818 2nd Law of Thermodynamics A reaction is spontaneous if ∆S for the universe is positive. ∆S universe > 0 for spontaneous process

19. 1919 Dissolving NH 4 NO 3 in water—an entropy driven process. 2nd Law of Thermodynamics

20. 2020

21. 2121 Sublimation Solid gas

22. 2222 Solid liquid gas liquid evaporationmelting