For an endothermic reaction A rightarrow B to | vedclass

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(C) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G$ must be negative,i.e.,$\Delta G < 0$.The relationship between Gibbs free

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$\Delta S > 0$

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(C) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G$ must be negative,i.e.,$\Delta G The relationship between Gibbs free energy,enthalpy,and entropy is given by $\Delta G = \Delta H - T\Delta S$.For an endothermic reaction,the enthalpy change $\Delta H > 0$.For $\Delta G$ to be negative $(\Delta G  \frac{\Delta H}{T}$.Since $\Delta H > 0$ and $T > 0$,it follows that $\Delta S$ must be positive,i.e.,$\Delta S > 0$.

For an endothermic reaction $A \rightarrow B$ to occur spontaneously at a constant temperature $T$,the entropy change $\Delta S$ must be:

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