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In a reaction, at 300k, KC is given as 2 x 10^13, then what is the value of ΔG?(a) – 7.64 × 10^4 J(b) – 7.64 × 10^4 J mol^–1(c) – 7.64 × 10 J mol^–1(d) – 7.64 × 10^4 mol^–1This question was addressed to me in semester exam.I'm obligated to ask this question of Relationship between Equilibrium Constant K, Reaction Quotient Q and Gibbs Energy G in portion Equilibrium of Chemistry – Class 11

Answer»

The correct choice is (b) – 7.64 × 10^4 J mol^–1

For explanation I WOULD say: We know that ΔG0 = – RT lnKc, where ΔG0 is the standard Gibbs free energy, R is universal gas CONSTANT, T is the temperature and KC is equilibrium constant; substituting KC as 2 x 10^13, ΔG0 = (– 8.314J mol^–1K^–1 × 300K) × ln(2×10^13); ΔG0 = – 7.64 × 10^4 J mol^–1.


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