The standard enthalpy and entropy changes for the reaction in equilibrium for the…

CHEMISTRY · Subjective · A Level · Chemistry · Thermodynamics · Thermodynamics

Problem

The standard enthalpy and entropy changes for the reaction in equilibrium for the forward direction are given below : CO(g)+H2O(g)⇌CO2(g)+H2(g)\text{CO}(\text{g}) + \text{H}_2\text{O}(\text{g}) \rightleftharpoons \text{CO}_2(\text{g}) + \text{H}_2(\text{g}) ΔH300K∘=−41.16 kJ mol−1;\Delta H_{300\text{K}}^\circ = -41.16 \text{ kJ mol}^{-1}; ΔS300K∘=−4.24×10−2 kJ mol−1\Delta S_{300\text{K}}^\circ = -4.24 \times 10^{-2} \text{ kJ mol}^{-1} ΔH1200K∘=−32.93 kJ mol−1;\Delta H_{1200\text{K}}^\circ = -32.93 \text{ kJ mol}^{-1}; ΔS1200K∘=−2.96×10−2 kJ mol−1\Delta S_{1200\text{K}}^\circ = -2.96 \times 10^{-2} \text{ kJ mol}^{-1} Calculate KpK_p at each temperature and predict the direction of reaction at 300 K and 1200 K, when PCO=PCO2=PH2=PH2O=1 atmP_{\text{CO}} = P_{\text{CO}_2} = P_{\text{H}_2} = P_{\text{H}_2\text{O}} = 1 \text{ atm} at initial state.

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