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Question

Calculate ΔG\Delta G^{\circ} at 45 degree C for reactions for which

(a) ΔH=293 kJ;ΔS=695 J/K\Delta H^{\circ}=293 \mathrm{~kJ} ; \Delta S^{\circ}=-695 \mathrm{~J} / \mathrm{K}

(b) ΔH=1137 kJ;ΔS=0.496 kJ/K\Delta H^{\circ}=-1137 \mathrm{~kJ} ; \Delta S^{\circ}=0.496 \mathrm{~kJ} / \mathrm{K}

(c) ΔH=86.6 kJ;ΔS=382 J/K\Delta H^{\circ}=-86.6 \mathrm{~kJ} ; \Delta S^{\circ}=-382 \mathrm{~J} / \mathrm{K}

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At constant temperature and pressure, the change in Gibbs free energy is defined as ΔG=ΔHTΔS\Delta \text G = \Delta \text H - \text{T}\Delta \text S

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