51) Calculate the ΔG°rxn using the following information. 4 HNO3(g) + 5 N2H4(l) → 7 N2(g) + 12 H2O(l)ΔG°rxn = ? ΔH°f (kJ/mol)-133.950.6-285.8 S°(J/mol?K)  266.9121.2191.670.0 A) +4.90 × 103 kJ B) +3.90 × 103 kJ C) -2.04 × 103 kJ D) -3.15 × 103 kJ E) -3.30 × 103 kJ 52) Calculate the ΔG°rxn using the following information. 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g)ΔG°rxn = ? ΔH°f (kJ/mol)-20.6-296.8-241.8 S°(J/mol?K)205.8205.2248.2188.8 A) -990.3 kJ B) +108.2 kJ C) -466.1 kJ D) +676.2 kJ E) -147.1 kJ 53) Use Hess’s law to calculate ΔG°rxn using the following information. NO(g) + O(g) → NO2(g)ΔG°rxn = ? 2 O3(g) → 3 O2(g)ΔG°rxn = +489.6 kJ O2(g) → 2 O(g)ΔG°rxn = +463.4 kJ NO(g) + O3(g) → NO2(g) + O2(g)ΔG°rxn = – 199.5 kJ A) +753.5 kJ B) +277.0 kJ C) -676.0 kJ D) -1152.5 kJ E) -225.7 kJ 54) Use Hess’s law to calculate ΔG°rxn using the following information. CO(g) → C(s) + 1/2 O2(g) ΔG°rxn = ? CO2(g) → C(s) + O2(g)ΔG°rxn = +394.4 kJ CO(g) + 1/2 O2(g) → CO2(g)ΔG°rxn = -257.2 kJ A) -60.0 kJ B) +651.6 kJ C) -265.8 kJ D) +137.2 kJ E) +523.0 kJ 55) Use Hess’s law to calculate ΔG°rxn using the following information. ClO(g) + O3(g) → Cl(g) + 2 O2(g)ΔG°rxn = ? 2 O3(g)→ 3 O2(g)ΔG°rxn = +489.6 kJ Cl(g) + O3(g) → ClO(g) + O2(g)ΔG°rxn = -34.5 kJ A) -472.4 kJ B) -210.3 kJ C) +455.1 kJ D) +262.1 kJ E) +524.1 kJ 56) Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. 3 O2(g) → 2 O3(g)ΔG° = +326 kJ P(O2) = 0.41 atm, P(O3) = 5.2 atm A) +341 kJ B) +17.8 kJ C) +332 kJ D) -47.4 kJ E) -109 kJ 57) Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. 2 Hg(g) + O2(g) → 2 HgO(s) ΔG° = -180.8 kJ P(Hg) = 0.025 atm, P(O2) = 0.037 atm A) +207 kJ B) -154.4 kJ C) -26.5 kJ D) -164 kJ E) +60.7 kJ 58) Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. CaCO3(s) → CaO(s) + CO2(g)ΔG° =+131.1 kJ P(CO2) = 0.033 atm A) -49.3 kJ B) -8.32 kJ C) +122.6 kJ D) +39.7 kJ E) +43.3 kJ 59) Which of the following is not true for ΔGrxn? A) If ΔG°rxn > 0, the reaction is spontaneous in the forward direction. B) If Q = 1, then ΔGrxn = ΔG°rxn. C) ΔG°rxn = K D) If ΔG°rxn > 0, the reaction is spontaneous in the reverse direction. E) Under equilibrium conditions, ΔGrxn = 0. 60) Choose the statement below that is true. A) K > 1, ΔG°rxn is positive. B) K < 1, ΔG°rxn is negative. C) ΔG°rxn = 0 at equilibrium. D) ΔGrxn = 0 at equilibrium. E) None of the above statements are true.