To determine the spontaneity of a reaction, we use the Gibbs free energy change $\Delta G. \\$The formula for $\Delta G$ is:$\\ \Delta G = \Delta H - T \Delta S \\$For a reaction to be spontaneous, $\Delta G$ must be negative.$\\$Given:$\\ \Delta H = 35.5$ kJ mol$^{-1} = 35500$ J mol$^{-1} \\ \Delta S = 83.6$ J K$^{-1}$ mol$^{-1} \\$The condition for spontaneity is:$\\ \Delta G < 0 \\ \Delta H - T \Delta S < 0 \\ T \Delta S > \Delta H \\ T > \frac{\Delta H}{\Delta S} \\$Substitute the given values:$\\ T > \frac{35500}{83.6} \\$Calculate $T: \\ T > 424.88$ K$\\$Therefore, the reaction is spontaneous at $T > 425$ K.$\\$This corresponds to Option 1: $T > 425$ K.$\\$However, the correct option provided is Option 2: All temperatures.$\\$This suggests a discrepancy, as the calculated result indicates $T > 425$ K.$\\$Please verify the provided correct option.