Chapter 16, Problem 8RQ

Consider the equation ∆G = ∆G° + RT ln(Q). What is the value of ∆G for a reaction at equilibrium? What does Q equal at equilibrium? At equilibrium, the previous equation reduces to ∆G° = −RT ln(K). When ∆G° > 0, what does it indicate about K? When ∆G° < 0, what does it indicate about K? When t ∆G° = 0, what does it indicate about K? ∆G predicts spontaneity for a reaction, whereas ∆G° predicts the equilibrium position. Explain what this statement means. Under what conditions can you use ∆G° to determine the spontaneity of a reaction?