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(C) For a reaction to be spontaneous,the Gibbs free energy change must be negative,i.e.,$\Delta G < 0$.According to the Gibbs-Helmholtz equation,$\Del

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$\Delta S > 0, \Delta H < 0, \Delta G < 0$ at all temperatures

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(C) For a reaction to be spontaneous,the Gibbs free energy change must be negative,i.e.,$\Delta G According to the Gibbs-Helmholtz equation,$\Delta G = \Delta H - T\Delta S$.If $\Delta H  0$ (increase in entropy),then $\Delta G$ will always be negative at all temperatures because $\Delta H$ is negative and $-T\Delta S$ is also negative.Therefore,the condition $\Delta S > 0, \Delta H < 0, \Delta G < 0$ represents a spontaneous reaction at all temperatures.

Which of the following conditions indicates the reaction is spontaneous?

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