Table 1. Standard state free energy changes and equilibrium constants for several chemical reactions (25^oC).

Reaction	Delta Go, kJ/mol	K
NaCl(s) <---> Na+(aq) + Cl-(aq)	-9.00	38
NH4NO3(s) <--> NH4+(aq) + NO3-(aq)	-4.31	5.7
Zn(s) + Cu2+(aq) <--> Cu(s) + Zn2+(aq)	-212.4	1.6 x 1037
2Cl-(1M) + Br2(l) <--> 2Br-(aq) + Cl2(g)	59.45	3.9 x 10-11
CH3COOH(aq) <--> CH3COO-(aq) + H+(aq)	27.18	1.8 x 10-5

1. Calculate DGo for the reaction

Delta G = 18.1 KJ/mole

HF(aq) H⁺(aq) + F^-(aq)

Use this data to calculate K_a for hydrofluoric acid.

2. Consider the reaction CO₂(g) + H₂(g) CO(g) + H₂O(g). Calculate DH^o, DS^o, DG^o, and K for this reaction at 25^oC. Predict the effect on the equilibrium constant when the temperature of the system is increased.

3. Without referring to tables to calculate Delta H^o and delta S^o, predict the signs of delta H^o and DS^o for the reaction NH₃(aq) NH₃(g). Explain why the odor of NH3(g) that collects above an aqueous solution of ammonia becomes more intense as the temperature is increased.

4. Explain why the equilibrium constant for the reaction below decreases as the temperature increases.

N₂(g) + 3H₂(g) 2NH₃(g)