A reaction at 300 K with ΔG° = −3486 J consists of 2 moles of A(g), 4 moles of B(g) and 2 moles of C(g). If A, B and C are in equilibrium in a one litre vessel, then the reaction should be (ln 2 = 0.7

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A reaction at 300 K with ΔG° = −3486 J consists of 2 moles of A(g), 4 moles of B(g) and 2 moles of C(g). If A, B and C are in equilibrium in a one litre vessel, then the reaction should be (ln 2 = 0.7, R = 8.3 J/K-mol)

TestHub · Accepted Answer

At equilibrium ΔG = 0, so K = e^(−ΔG°/RT) = e^(3486/(8.3 × 300)) = e 1.4 = 4. With [A] = 2, [B] = 4, [C] = 2 mol/L: (a) 2/(2×4) = 0.25; (b) 4×2/2 = 4 ✓; (c) 4/2² = 1; (d) 4×2²/2 = 8. Only A ⇌ B + C gives K = 4. Matches (b).

Chemistry - Thermodynamics - II Question with Solution | TestHub

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