SOLVED

61) What is true if ln K is negative? A) ΔG°rxn is positive and the reaction is spontaneous in the forward direction. B) ΔG°rxn is negative and the reaction is spontaneous in the forward direction. C) ΔG°rxn is negative and the reaction is spontaneous in the reverse direction. D) ΔG°rxn is positive and the reaction is spontaneous in the reverse direction. E) ΔG°rxn is zero and the reaction is at equilibrium. 62) What is true if ln K is positive? A) ΔG°rxn is positive and the reaction is spontaneous in the forward direction. B) ΔG°rxn is negative and the reaction is spontaneous in the forward direction. C) ΔG°rxn is negative and the reaction is spontaneous in the reverse direction. D) ΔG°rxn is positive and the reaction is spontaneous in the reverse direction. E) ΔG°rxn is zero and the reaction is at equilibrium. 63) What is true if ln K is 1? A) ΔG°rxn is positive and the reaction is spontaneous in the forward direction. B) ΔG°rxn is negative and the reaction is spontaneous in the forward direction. C) ΔG°rxn is negative and the reaction is spontaneous in the reverse direction. D) ΔG°rxn is positive and the reaction is spontaneous in the reverse direction. E) ΔG°rxn is zero and the reaction is at equilibrium. 64) Which of the following reactions will have the largest equilibrium constant (K) at 298 K? A) CaCO3(s) → CaO(s) + CO2(g)ΔG° =+131.1 kJ B) 2 Hg(g) + O2(g) → 2 HgO(s) ΔG° = -180.8 kJ C) 3 O2(g) → 2 O3(g)ΔG° = +326 kJ D) Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g)ΔG° = -28.0 kJ E) It is not possible to determine without more information. 65) Use the free energies of formation given below to calculate the equilibrium constant (K) for the following reaction at 298 K. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l)K = ? ΔG°f (kJ/mol)-110.987.651.3-237.1 A) 8.71 × 108 B) 0.980 C) 1.15 × 10-9 D) 1.02 E) 5.11 × 10-4 66) Determine the equilibrium constant for the following reaction at 298 K. SO3(g) + H2O(g) → H2SO4(l)ΔG° = -90.5 kJ A) 1.37 × 10-16 B) 4.78 × 1011 C) 9.11 × 10-8 D) 7.31 × 1015 E) 0.964 67) Determine the equilibrium constant for the following reaction at 298 K. Cl(g) + O3(g) → ClO(g) + O2(g)ΔG° = – 34.5 kJ A) 5.66 × 105 B) 0.986 C) 8.96 × 10-7 D) 4.98 × 10-4 E) 1.12 × 106 68) Determine the equilibrium constant for the following reaction at 498 K. 2 Hg(g) + O2(g) → 2 HgO(s) ΔH° = -304.2 kJ; ΔS° = -414.2 J/K A) 1.87 × 1010 B) 8.10 × 1031 C) 2.31 × 10-22 D) 5.34 × 10-11 E) 4.33 × 1021 69) Determine the equilibrium constant for the following reaction at 655 K. HCN(g) + 2 H2(g) → CH3NH2(g)ΔH° = -158 kJ; ΔS°= -219.9 J/K A) 3.99 × 1012 B) 13.0 C) 2.51 × 10-13 D) 3.26 × 10-12 E) 3.07 × 1011 70) Determine the equilibrium constant for the following reaction at 549 K. CH2O(g) + 2 H2(g) → CH4(g) + H2O(g) ΔH° = -94.9 kJ; ΔS°= -224.2 J/K A) 481 B) 1.07 × 109 C) 2.08 × 10-3 D) 9.35 × 10-10 E) 1.94 × 10-12