ΔG° for the reaction: X + Y ⇌ C is -4.606 kcal at 1000 K. The equilibrium constant for the reverse m — Chemical Equilibrium Chemistry Question

💡 Solution & Explanation

For the forward reaction, ΔG° = -4.606 kcal. For the reverse reaction C ⇌ X + Y, ΔG° = +4.606 kcal = 4606 cal. Using ΔG° = -2.303 RT log K_rev: 4606 = -2.303(2)(1000) log K_rev = -4606 log K_rev. This yields log K_rev = -1, so K_rev = 10⁻¹ = 0.1. Therefore, correct answer is D.