Assertion: Many endothermic reactions that ar | vedclass

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(C) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G$ must be negative,where $\Delta G = \Delta H - T\Delta S$.For endothermic

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If the Assertion is correct but Reason is incorrect.

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(C) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G$ must be negative,where $\Delta G = \Delta H - T\Delta S$.For endothermic reactions,$\Delta H > 0$. If the reaction involves an increase in entropy $(\Delta S > 0)$,then at high temperatures,the term $T\Delta S$ becomes larger than $\Delta H$.Consequently,$\Delta G = \Delta H - T\Delta S$ becomes negative,making the reaction spontaneous at high temperatures.The reason provided is incorrect because the entropy of a system is generally considered a state function that does not necessarily increase with temperature in the context of the spontaneity condition; rather,the term $T\Delta S$ increases with temperature.

Assertion: Many endothermic reactions that are not spontaneous at room temperature become spontaneous at high temperature.
Reason: Entropy of the system increases with increase in temperature.

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Which of the following is correct?

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Assertion: Many endothermic reactions that are not spontaneous at room temperature become spontaneous at high temperature.Reason: Entropy of the system increases with increase in temperature.