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(B) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G$ must be negative.$\Delta G = \Delta H - T\Delta S$.Given that both $\Delt

Vedclass · Accepted Answer

$T\Delta S > \Delta H$ and both $\Delta H$ and $\Delta S$ are $+ve$

Vedclass · Answer

(B) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G$ must be negative.$\Delta G = \Delta H - T\Delta S$.Given that both $\Delta H$ and $\Delta S$ are positive $(+ve)$,$\Delta G = (+ve) - T(+ve)$.If $T\Delta S > \Delta H$,then the term $T\Delta S$ is larger than $\Delta H$,making $\Delta G$ negative.Therefore,the reaction is spontaneous when $T\Delta S > \Delta H$.

$A$ reaction occurs spontaneously if

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