5{ following have positive values for S° of the system?

a. H₂O(s) ---> H₂O(l) at 25°C
b. Ag⁺(aq, 1 M) + Cl^-(aq, 1 M) ---> AgCl(s)
c. H⁺(aq) + OH^-(aq) ---> H₂O(l)
d. CaCO₃(s) ---> CaO(s) + CO₂(g)

How, if at all, can this reaction be made spontaneous by changing the temperature?

TiCl₄(g) + O₂(g) ---> TiO₂(s) + 2 Cl₂(g)

For this process H° < 0 and S° < 0.

The process below has H° = -112 kJ/mol and S° = -8.07 J/mol•K. What is G° for this process at 25°C?

Si(s) + C(graphite) ---> SiC(s)

Use the reactions and G° values below to determine G° for:

3 CH₄(g) + 4 O₂(g) ---> C₃O₂(g) + 6 H₂O(g)

For CH₄(g) + 2 O₂(g) ---> CO₂(g) + 2 H₂O(g), G° = -800.8 kJ/mol
For 3 CO₂(g) ---> C₃O₂(g) + 2 O₂(g), G° = +1073.4 kJ/mol

Calculate G for the process below and determine whether it is spontaneous when the partial pressure of NO is 0.10 atm and the partial pressure of NOBr is 1.7 atm at 298 K.

2 NO(g) + Br₂(l) ---> 2 NOBr(g)

Under standard conditions, the reaction below is nonspontaneous at 25°C. For this process, G° = 1.72 kJ/mol. Which of the following changes will lead to this process being spontaneous?

H₂(g) + I₂(g) <==> 2 HI(g)

Use thermodynamic and other data in the appendix to determine the standard free energy of formation of the acetate, CH₃COO^-(aq), ion at 25°C. An ionization reaction in which this forms is below.

CH₃COOH(aq) <==> H⁺(aq) + CH₃COO^-(aq)

What is the H of a reaction if K doubles when the temperature is increased from 273 K to 373 K?

NH₃(g, S° =192.51 J/mol.deg) + HCl (g, S° = 186.69 J/mol.deg) => NH₄Cl (s, S° = 94.56 J/mol.deg). The standard entropy change for this reaction in J/mol.deg is

Consider the reaction:

3 N₂(g) + 2 O₃(g) => 6 NO(g)

(DELTA) H°_f in kJ/mol = 0.00, 142.26, and 90.37

S° in J/mol.K = 191.5, 237.7, and 210.6

(a) What is the (DELTA) H°_rxn for this reaction in kJ/mol?

(b) What is (DELTA) S°_rxn for this reaction in J/mol.K?

(c) What is (DELTA) G°_rxn for this reaction in kJ/mol at 500 K?