Without doing a numerical calculation, determine which of the following will reduce the free energy change for the reaction, that is, make it less positive or more negative, when the temperature is increased. Explain.(a) N2(g) + 3H2(g) ⟶ 2NH3(g)(b) HCl(g) + NH3(g) ⟶ NH4 Cl(s)(c) (NH4)2 Cr2 O7(s) ⟶ Cr2 O3(s) + 4H2 O(g) + N2(g)(d) 2Fe(s) + 3O2(g) ⟶ Fe2 O3(s)

Predict whether entropy increases or decreases in each of the following reactions. (a) 2H2S (g)+SO2 (g)→3S (s)+2H2O (g)(b) 2Cl-(aq) +2H2O (l) →2OH- (aq)+H2 (g) +Cl2 (g)

A reaction has a standard free-energy change of -13.10 kJ mol-¹(-3.131 kcal mol-¹). Calculate the equilibrium constant for the reaction at 25 °C. Keq =

10. Use data from your textbook’s appendix to determine ΔG° for the following reaction at 549 K and standard conditions:CH2O(g) + 2 H2(g) ⇌ CH4(g) + H2O(g).(a) 193.7 kJ (b) ‒193.7 kJ (c) 5.749×104 kJ (d) ‒150.1 kJ 11. Determine the equilibrium constant (K) for the reaction in the problem above. CH2O(g) + 2 H2(g) ⇌ CH4(g) + H2O(g).(a) 481 (b) 1.07×109 (c) 2.08×10‒3 (d) 1.87×1014                        CH2O(g) + 2 H2(g) ⇌ CH4(g) + H2O(g). H(kJ/mol)       -108.6        0             -74.6         -241.8 S (J.mol k)       218.8         130.7       186.3          188.8