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# Calculate $\Delta G^{\circ}$ at 45 degree C for reactions for which(a) $\Delta H^{\circ}=293 \mathrm{~kJ} ; \Delta S^{\circ}=-695 \mathrm{~J} / \mathrm{K}$(b) $\Delta H^{\circ}=-1137 \mathrm{~kJ} ; \Delta S^{\circ}=0.496 \mathrm{~kJ} / \mathrm{K}$(c) $\Delta H^{\circ}=-86.6 \mathrm{~kJ} ; \Delta S^{\circ}=-382 \mathrm{~J} / \mathrm{K}$

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

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