At constant T and P, in which of the following situations will the reaction always be product-favored?

Question

Quizplus · Accepted Answer

According to Gibbs free energy equation, for a reaction to be product-favored (i.e. spontaneous), ΔG must be negative. ΔG is dependent on ΔH and ΔS, as follows:

ΔG = ΔH - TΔS

If we assume that T and P are constant, then as ΔH becomes more negative (exothermic reaction), ΔG becomes more negative making the reaction spontaneous. Additionally, if ΔS becomes more positive (more entropy) then ΔG becomes more negative as well. Thus, the only option where both ΔH and ΔS promote a spontaneous reaction is D (DH < 0 and DS > 0).

At Constant T and P, in Which of the Following