At constant T and P, in which situation will the reaction be product-favored at high temperature but not at low temperature?

Question

Quizplus · Accepted Answer

For a reaction to be product-favored at high temperature but not at low temperature, the reaction should be endothermic ($ \Delta H > 0 $) and have an increase in entropy ($ \Delta S > 0 $). According to the Gibbs free energy equation $ \Delta G = \Delta H - T\Delta S $, at high temperatures, the $ T\Delta S $ term becomes significant, leading to a negative $ \Delta G $ if $ \Delta S > 0 $, favoring the products.

At Constant T and P, in Which Situation Will the Reaction