A reaction at 300 K with ΔG° = -1743 J consists of 3 moles of A(g), 6 moles of B(g) and 3 moles of C(g). If A, B and C are in equilibrium in 1L container, then the reaction may be (ln 2 = 0.7, R = 8.3

Question

A reaction at 300 K with ΔG° = -1743 J consists of 3 moles of A(g), 6 moles of B(g) and 3 moles of C(g). If A, B and C are in equilibrium in 1L container, then the reaction may be (ln 2 = 0.7, R = 8.3 J/K-mol)

Prashant Kotian · Accepted Answer

Correct answer: C. Using ΔG° = -RT ln K, -1743 = -8.3 × 300 × ln K => ln K = 1743 / 2490 = 0.7. Since ln 2 = 0.7, K = 2. The concentrations are [A] = 3 M, [B] = 6 M, [C] = 3 M. Checking option (c): 2A ⇌ B + C gives K = ([B][C]) / [A]² = (6 × 3) / 3² = 18 / 9 = 2. This matches the calculated K value. Therefore, correct answer is C.

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