Thermodynamics

$\left(\Delta_{\text {sys }} \mathrm{S}^{\circ}\right)+\Delta_{\text {surr }} \mathrm{S}^{\circ}=-7692 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$, the reaction is spontaneous.

$\left(\Delta_{\text {sys }} \mathrm{S}^{\circ}\right)+\Delta_{\text {surr }} \mathrm{S}^{\circ}=-5692 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$, the reaction is non-spontaneous.

$\left(\Delta_{\text {sys }} \mathrm{S}^{\circ}\right)+\Delta_{\text {surr }} \mathrm{S}^{\circ}=+5692 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$, the reaction is spontaneous.

$\left(\Delta_{\text {sys }} \mathrm{S}^{\circ}\right)+\Delta_{\text {surr }} \mathrm{S}^{\circ}=+7692 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$, the reaction is non-spontaneous.