STANDARD Chemistry Gibbs Free Energy MCQ Question
For a reaction, 2K(g) + L(g) → 2M(g); ΔU° = −10.5 kJ and ΔS° = −44.1 J K⁻¹. Calculate ΔG° for the reaction and predict whether the reaction will be spontaneous or non-spontaneous?
G = +0.16 kJ, non-spontaneous
G = −0.16 kJ, spontaneous
G = +26.12 kJ, non-spontaneous
G = −26.12 kJ, non-spontaneous
Correct Answer
Detailed Explanation
ΔG° = ΔH° − TΔS° = −12.98 + 13.14 = 0.16 kJ. Since ΔG° is +ve, hence it is non-spontaneous.
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