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(D) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G$ must be negative,i.e.,$\Delta G < 0$.Given $\Delta G = \Delta H - T\Delta

Vedclass · Accepted Answer

$1118$

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(D) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G$ must be negative,i.e.,$\Delta G Given $\Delta G = \Delta H - T\Delta S$.At equilibrium,$\Delta G = 0$,so $T = \frac{\Delta H}{\Delta S}$.Substituting the values: $\Delta H = 179.1 	imes 10^3 \, J \, mol^{-1}$ and $\Delta S = 160.2 \, J \, K^{-1} \, mol^{-1}$.$T = \frac{179.1 	imes 10^3}{160.2} \approx 1118 \, K$.Since the reaction is endothermic $(\Delta H > 0)$ and entropy increases $(\Delta S > 0)$,the reaction becomes spontaneous at temperatures higher than the equilibrium temperature.Therefore,the reaction becomes spontaneous above $1118 \, K$.

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