Answer
$\Delta G=\Delta H-T \Delta S$
$\Delta G=-7000 \mathrm{\ J} \cdot \mathrm{mol}^{-1}-(298 \mathrm{\ K})\left(-25 \mathrm{\ J} \cdot \mathrm{\ K}^{-1} \cdot \mathrm{mol}^{-1}\right)$
$\Delta G=-7000+7450 \mathrm{\ J} \cdot \mathrm{mol}^{-1}=450 \mathrm{\ J} \cdot \mathrm{mol}^{-1}$
$\text{The reaction is not spontaneous because $\Delta G>0 .$ The temperature}$
$\text{must be decreased in order to decrease the value of the $T \Delta S$ term.}$
Work Step by Step
$\Delta G=\Delta H-T \Delta S$
$\Delta G=-7000 \mathrm{\ J} \cdot \mathrm{mol}^{-1}-(298 \mathrm{\ K})\left(-25 \mathrm{\ J} \cdot \mathrm{\ K}^{-1} \cdot \mathrm{mol}^{-1}\right)$
$\Delta G=-7000+7450 \mathrm{\ J} \cdot \mathrm{mol}^{-1}=450 \mathrm{\ J} \cdot \mathrm{mol}^{-1}$
$\text{The reaction is not spontaneous because $\Delta G>0 .$ The temperature}$
$\text{must be decreased in order to decrease the value of the $T \Delta S$ term.}$
