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(C) The Gibbs free energy equation is given by $\Delta G = \Delta H - T\Delta S$.For a spontaneous process,the condition is $\Delta G < 0$.For an endo

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$\Delta S > 0$

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(C) The Gibbs free energy equation is given by $\Delta G = \Delta H - T\Delta S$.For a spontaneous process,the condition is $\Delta G For an endothermic reaction,the enthalpy change is positive,i.e.,$\Delta H > 0$.Substituting these into the equation: $\Delta G = (+\Delta H) - T\Delta S This implies that $T\Delta S > \Delta H$. Since $\Delta H$ is positive and $T$ is positive,$\Delta S$ must be positive $(\Delta S > 0)$ for the reaction to be spontaneous.

For an endothermic reaction at constant temperature $T$ and pressure $P$,if the process is spontaneous,which of the following is true?

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