NEET 2026 Chemistry Gibbs Free Energy MCQ Question
Consider the following reaction: 2A(g) + B(g) → 2D(g) ΔU° = −10 kJ mol⁻¹ and ΔS° = −44 J K⁻¹ at 298 K. Identify the correct option with ΔG° for the reaction and spontaneity of the reaction at 298 K. (Given: R = 8.31 J mol⁻¹ K⁻¹)
(1) −1.635 kJ mol⁻¹, spontaneous
(2) −0.63568 kJ mol⁻¹, spontaneous
(3) +0.63568 kJ mol⁻¹, non-spontaneous
(4) +1.635 kJ mol⁻¹, non-spontaneous
Correct Answer
Detailed Explanation
The Gibbs free energy change ΔG° is calculated using the formula ΔG° = ΔH° − TΔS°. Substituting the given values, ΔH° = ΔU° + Δn₉RT = −10 − 2.48 = −12.48 kJ/mol. ΔG° = −12.48 + 13.112 = +0.632 kJ/mol. Since ΔG° is positive, the process is non-spontaneous.
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