Homework # 9 Ksp and Thermodynamics Spring 2023

3. Answer each of the following questions (a – c) for the reactions given in parts i. – iii. below. a. Predict the entropy change for the reaction to be less than zero, near zero or greater than zero and explain your prediction conceptually. b. Use the data given in the tables to calculate Δ H° , Δ S° , and Δ G° at 298 K for each of the following reactions. c. Discuss whether each reaction will be spontaneous at all temperatures, high temperatures, low temperatures, or nonspontaneous at all temperatures (i.e. never spontaneous). (a) Ni( s ) + Cl 2 ( g ) ⇌ NiCl 2 ( s ) ΔH° (kJ/mol) ΔG° (kJ/mol) S° (J/mol K) NiCl 2 (s) -305.3 -259.1 97.7 Ni(s) 0 0 30.1 Cl 2 (g) 0 0 223.0 (b) CaCO 3 ( s , calcite) ⇌ CaO( s ) + CO 2 ( g ) ΔH° (kJ/mol) ΔG° (kJ/mol) S° (J/mol K) CaO(s) -635.6 -604.2 39.8 CO 2 (g) -393.5 -394.4 213.6 CaCO 3 (s) -1206.9 -1128.8 92.9 (c) 2 CH 3 OH( l ) + 3 O 2 ( g ) ⇌ 2 CO 2 ( g ) + 4 H 2 O( l ) ΔH° (kJ/mol) ΔG° (kJ/mol) S° (J/mol K) H 2 O(l) -285.8 -237.2 69.9 CO 2 (g) -393.5 -394.4 213.6 O 2 (g) 0 0 205 CH 3 OH(l) -238.7 -166.3 126.8 4. At 298 K, ΔG° f [CO(g)] = ‒137.15 kJ/mol and K p = 6.5 × 10 11 for the reaction below: CO(g) + Cl 2 (g) ⇌ COCl 2 (g) Determine the ΔG° f [COCl 2 (g)] using only these data.