3. CO(g) + O2(g) CO2(g) The combustion of carbon monoxide is represented by the equation above. (a) Determine the value of the standard enthalpy change, for the combustion of CO(g) at 298 K using the following information. ∆H˚rxn C(s) + O2(g) CO(g) = kJ mol-1 ∆H˚298 –110.5 C(s) + O2(g) CO2(g) = kJ mol-1 ∆H˚298 –393.5 (b) Determine the value of the standard entropy change, for the combustion of CO(g) at 298 K using the information in the following table. ∆S˚rxn, S˚298 Substance (J mol-1 K-1) CO(g) 197.7 CO2(g) 213.7 O2(g) 205.1 (c) Determine the standard free energy change, for the reaction at 298 K. Include with your answer. ∆G˚rxn, (d) Is the reaction spontaneous under standard conditions at 298 K? Justify your answer. (e) Calculate the value of the equilibrium constant, for the reaction at 298 K. Keq, The initial temperature of your water, the final temperature of your reaction are measured, and is calculated ΔT of reactants are calculated. The specific heat of water is used (4.18 J/mol K) q absorbed by is calculated qsurroundings = negative qsystem is assumed Getting from q to ΔH Convert q Joules into KJ divide by moles of reactant (from molarity(MxL) if solution and grams--> moles if solid )to get reaction!!! ΔH
3. CO(g) + O2(g) CO2(g) The combustion of carbon monoxide is represented by the equation above. (a) Determine the value of the standard enthalpy change, ∆H˚rxn for the combustion of CO(g) at 298 K using the following information. C(s) + O2(g) CO(g) ∆H˚298 = –110.5 kJ mol-1 C(s) + O2(g) CO2(g) ∆H˚298 = –393.5 kJ mol-1 (b) Determine the value of the standard entropy change, ∆S˚rxn, for the combustion of CO(g) at 298 K using the information in the following table. Substance S˚298 (J mol-1 K-1) CO(g) 197.7 CO2(g) 213.7 O2(g) 205.1 (c) Determine the standard free energy change, ∆G˚rxn, for the reaction at 298 K. Include with your answer. (d) Is the reaction spontaneous under standard conditions at 298 K? Justify your answer. (e) Calculate the value of the equilibrium constant, Keq, for the reaction at 298 K. The initial temperature of your water, the final temperature of your reaction are measured, and ΔT is calculated of reactants are calculated. The specific heat of water is used (4.18 J/mol K) q absorbed by is calculated qsurroundings = negative qsystem is assumed Getting from q to ΔH Convert q Joules into KJ divide by moles of reactant (from molarity(MxL) if solution and grams--> moles if solid )to get ΔH reaction!!!
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