A reaction with a low enthalpy of reaction value is not spontaneous at low temperature but becomes spontaneous at high temperature. What are the signs for $\Delta$H° and $\Delta$S°, respectively?

Question

Quizplus · Accepted Answer

For a reaction to be non-spontaneous at low temperatures and spontaneous at high temperatures, $\Delta$H° must be positive and $\Delta$S° must be positive. This is because the T$\Delta$S° term becomes more significant at higher temperatures, allowing the reaction to become spontaneous ($\Delta$G° = $\Delta$H° - T$\Delta$S° < 0).

A Reaction with a Low Enthalpy of Reaction Value Is Δ\DeltaΔ

A Reaction with a Low Enthalpy of Reaction Value Is $\Delta$