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(C) The spontaneity of a reaction is determined by the Gibbs free energy equation: $\Delta G = \Delta H - T \Delta S$. For a reaction to be spontaneou

Vedclass · Accepted Answer

$\Delta G = -ve, \Delta H = +ve, \Delta S = +ve$

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(C) The spontaneity of a reaction is determined by the Gibbs free energy equation: $\Delta G = \Delta H - T \Delta S$. For a reaction to be spontaneous,$\Delta G For a reaction to be non-spontaneous,$\Delta G > 0$. Given that the reaction is non-spontaneous at $298 \ K$ $(\Delta G > 0)$ and spontaneous at $350 \ K$ $(\Delta G  0)$ and have a positive entropy change $(\Delta S > 0)$. At lower temperatures,the $T \Delta S$ term is smaller than $\Delta H$,making $\Delta G$ positive. At higher temperatures,the $T \Delta S$ term exceeds $\Delta H$,making $\Delta G$ negative. Thus,the conditions are $\Delta H > 0$ and $\Delta S > 0$.

If a chemical reaction is known to be non-spontaneous at $298 \ K$ but spontaneous at $350 \ K$,then which among the following conditions is true for the reaction?

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