Question Detail
Question
When a reaction is non-spontaneous under standard conditions, what could make it spontaneous?
Correct Answer
Option B is the correct answer.
Detailed Explanation
From ΔG = ΔH - TΔS, if ΔS is positive, increasing the temperature T increases the magnitude of the -TΔS term. If this term becomes sufficiently large to make the overall ΔG negative, the reaction can become spontaneous.
Hint
Manipulate the Gibbs free energy equation. Which term is temperature-dependent, and how does its sign affect spontaneity?