SOLVED

41) Below what temperature does the following reaction become nonspontaneous? 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l)ΔH = +136.5 kJ; ΔS = +287.5 J/K A) 39.2 K B) 151 K C) 475 K D) This reaction is nonspontaneous at all temperatures. E) This reaction is spontaneous at all temperatures. 42) What can change the direction of a reversible reaction? A) change in temperature B) change in pressure C) change in volume D) A, B, and C E) none of the above 43) Give the name of the reaction that achieves the theoretical limits with respect to free energy in thermodynamics. A) reversible reaction B) forward reaction C) reverse reaction D) nonspontaneous reaction E) irreversible reaction 44) Give the name of the reaction that does not achieve the theoretical limits with respect to free energy in thermodynamics. A) reversible reaction B) forward reaction C) reverse reaction D) equilibrium reaction E) irreversible reaction 45) Determine ΔG°rxn using the following information. H2(g) + CO(g) → CH2O(g)ΔH°= +1.9 kJ; ΔS°= -109.6 J/K A) +57.7 kJ B) -30.8 kJ C) +34.6 kJ D) -41.5 kJ E) +17.3 kJ 46) Determine ΔG°rxn using the following information. 2 H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g)ΔH°= +1.12 kJ; ΔS°= -390.7 J/K A) -118 kJ B) -348 kJ C) +28.4 kJ D) -58.3 kJ E) +440 kJ 47) Given the following equation, N2O(g) + NO2(g) → 3 NO(g)ΔG°rxn = -23.0 kJ Calculate ΔG°rxn for the following reaction. 3 NO(g) → N2O(g) + NO2(g) A) -23.0 kJ B) 69.0 kJ C) -69.0 kJ D) -7.67 kJ E) 23.0 kJ 48) Calculate the ΔG°rxn using the following information. 4 HNO3(g) + 5 N2H4(l) → 7 N2(g) + 12 H2O(l)ΔG°rxn = ? ΔG°f (kJ/mol)-73.5149.3-237.1 A) -3.298 × 103 kJ B) -312.9 kJ C) +2.845 × 103 kJ D) +110.7 kJ E) -954.7 kJ 49) Calculate the ΔG°rxn using the following information. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l)ΔG°rxn = ? ΔG°f (kJ/mol)-110.987.651.3-237.1 A) -162.5 kJ B) +51.0 kJ C) -54.5 kJ D) +171.1 kJ E) -87.6 kJ 50) Calculate the ΔG°rxn using the following information. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l)ΔG°rxn = ? ΔH°f (kJ/mol)-207.091.333.2-285.8 S°(J/mol?K146.0210.8240.170.0 A) -151 kJ B) -85.5 kJ C) +50.8 kJ D) +222 kJ E) -186 kJ