Question

A reaction that does not tend to go at room temperature may become feasible as the temperature rises because ________ decreases in magnitude as T increases.

1) the enthalpy change (ΔH) of the reaction
2) the entropy change (ΔS) of the reaction
3) the activation energy (Ea) of the reaction
4) the equilibrium constant (K) of the reaction

Answer 1

A reaction becomes more feasible at higher temperatures due to the increased significance of the entropy change (ΔS), which decreases the Gibbs free energy (ΔG) and makes the reaction more spontaneous.

Step-by-step explanation:

A reaction that does not tend to go at room temperature may become feasible as the temperature rises because the Gibbs free energy (ΔG) decreases in magnitude as T (temperature) increases.

This is due to the entropy change (ΔS) of the reaction becoming more significant in the equation ΔG = ΔH - TΔS, where ΔH is the enthalpy change. If ΔS is positive, increasing the temperature amplifies the TΔS term, which can lead to a decrease in ΔG, making the reaction more spontaneous.

Therefore, the correct answer is that the entropy change (ΔS) of the reaction decreases in magnitude as T increases.