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(C) For an endothermic process,the enthalpy change is positive,so $\Delta H > 0$.For a spontaneous process,the Gibbs free energy change must be negati

Vedclass · Accepted Answer

$\Delta S > 0$

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(C) For an endothermic process,the enthalpy change is positive,so $\Delta H > 0$.For a spontaneous process,the Gibbs free energy change must be negative,so $\Delta G Using the Gibbs-Helmholtz equation: $\Delta G = \Delta H - T \Delta S$.Since $\Delta G  0$,the term $T \Delta S$ must be positive and larger than $\Delta H$ to make $\Delta G$ negative.Therefore,$\Delta S$ must be positive,i.e.,$\Delta S > 0$.

For a spontaneous endothermic process at constant pressure,which of the following is true?

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