1. Find the change in entropy when 87.3 g of water vapor condense, given that water’s heat of vaporization is 5.99 kJ/mol. 373.15 K = –0.0779 = –77.9 For a system in which heat is transferred at constant temperature… -- T in K -- common unit for entropy  i.e., heat (energy) temperature

2. Third Law of Thermodynamics: The entropy of a pure, crystalline substance at absolute zero is… -- that would be a state of perfect order ZERO. (impossible)

3. Entropy increases when: 1. the number of gas particles increases 2. liquids or solutions are formed from solids 3. gases are formed from liquids or solids 2 NH 3 N 2 + 3 H 2 fewer bonds; fewer restrictions on motion of atoms; more degrees of freedom; more possible microstates +S+S

4. Which has the greater entropy? 1 mol KCl(s) @ 300 K or 1 mol HCl(g) @ 300 K 1 mol O 2 (g) @ 300 K or 1 mol O 2 (g) @ 500 K 2 mol HCl(g) @ 300 K or 4 mol HCl(g) @ 300 K (same volume) 1 mol HCl(g) @ 300 K or 1 mol Ar(g) @ 300 K (same volume) 2 mol HCl(g) @ 300 K or 2 mol HCl(g) @ 300 K (in a 5-L vessel)(in a 10-L vessel) (same volume)

5. Calculating Entropy Changes standard molar entropies, S o : molar entropy values of substances in their standard states (i.e., pure substances at ~1 atm) S o values typically… -- actually, at 1 bar = 10 5 Pa = 0.987 atm In a chemical reaction… are NOT zero w /increasing molar mass w /increasing # of atoms in formula  S o =  nS o P –  mS o R (n and m are the coeff. for each substance)

6. Calculate the standard entropy change for… P 4 (s,white) + 10 Cl 2 (g)  4 PCl 5 (g) 177223353 tabulated values of S o in J/mol-K  S o =  nS o P –  mS o R  S o = 4(353) – [177 + 10(223)] = –995J/K White phosphorus (or “WP”) is used in bombs, artillery shells, and mortar shells that burst into burning flakes of phosphorus upon impact. Smokescreen or flesh-fryer?