Given ΔG = -35 kJ/mol for a reaction at 298 K, calculate the equilibrium constant K.
Correct: D
We use the equation ΔG = -RTlnK. Rearranging for K, we get K = exp(-ΔG/RT). R = 8.314 J/(mol*K). Therefore, K = exp(-(-35000 J/mol) / (8.314 J/(mol*K) * 298 K)) = exp(14.12) ≈ 1.4 x 10⁶.