A reaction at 300 K with ΔG° = −1743 J consist 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 one liter vessel, then the reaction should be (ln 2 = 0.7, R

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A reaction at 300 K with ΔG° = −1743 J consist 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 one liter 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^(1743/(8.3 × 300)) = e 0.7 = 2. With [A] = 3, [B] = 6, [C] = 3 mol/L, test each stoichiometry: (a) 3/(3×6) = 1/6; (b) 6×3²/3 = 18; (c) 6×3/3² = 2 ✓; (d) 3²/(3×6) = 1/2. Only 2A ⇌ B + C gives K = 2. Matches (c).

Chemistry - Thermodynamics - II Question with Solution | TestHub

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