The combustion of carbon monoxide is represented by the equation above.(a) Determine the value of the standard enthalpy change, ÄHºrxn, for the combustion of CO(g) at 298 K using the following information. (2 points)(b) Determine the value of the standard entropy change, ÄSºrxn, for the combustion of CO(g) at 298 K using the information in the following table.(2 points)(c) Determine the standard free energy change, ÄGºrxn,for the reaction at 298 K. Include units with your answer.(2 points)(d) Is the reaction spontaneous under standard conditions at 298 K? Justify your answer.(1 point)(e) Calculate the value of the equilibrium constant, Keq , for the reaction at 298 K.(2 points).

Above what temperature does the following reaction become nonspontaneous? 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) ÄH = -1036 kJ; ÄS = -153.2 J/K

Use Hess’s law to calculate ÄG°rxn using the following information. NO(g) + O(g) → NO2(g) ÄG°rxn = ? 2 O3(g) → 3 O2(g) ÄG°rxn = +489.6 kJ O2(g) → 2 O(g) ÄG°rxn = +463.4 kJ NO(g) + O3(g) → NO2(g) + O2(g) ÄG°rxn = – 199.5 kJ

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