01ΔG° ↔ K
ΔG° = −RT ln K. Negative ΔG° → K > 1 (products favored). Positive ΔG° → K < 1.
ΔG° = 0 → K = 1. R = 8.314 J/(mol·K).
02Notebook box
ΔG = ΔG° + RT ln Q (moves toward zero at equilibrium).
Worked example: ΔG° = −5.7 kJ at 298 K → K = e^(5700/(8.314×298)) ≈ 10.