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

Vedclass · Accepted Answer

$1118$

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(D) For a process to be spontaneous,the Gibbs free energy change must be negative,i.e.,$\Delta G Given $\Delta G = \Delta H - T \Delta S$,the condition for spontaneity is $\Delta H - T \Delta S This implies $T > \frac{\Delta H}{\Delta S}$.Given $\Delta H = +179.1 \ kJ \ mol^{-1} = 179100 \ J \ mol^{-1}$ and $\Delta S = +160.2 \ J \ K^{-1} \ mol^{-1}$.$T > \frac{179100}{160.2} \ K$.$T > 1117.97 \ K$.Therefore,the process becomes spontaneous at temperatures higher than $1118 \ K$.

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