What is the relationship between the Gibbs free energy change (ΔG) and the equil
Practice Questions
Q1
What is the relationship between the Gibbs free energy change (ΔG) and the equilibrium constant (K)?
ΔG = -RT ln(K)
ΔG = RT ln(K)
ΔG = K - RT
ΔG = 0 at equilibrium
Questions & Step-by-Step Solutions
What is the relationship between the Gibbs free energy change (ΔG) and the equilibrium constant (K)?
Correct Answer: ΔG = -RT ln(K)
Step 1: Understand that Gibbs free energy change (ΔG) tells us if a reaction is spontaneous or not.
Step 2: Know that the equilibrium constant (K) tells us the ratio of products to reactants at equilibrium.
Step 3: Learn the equation that connects ΔG and K: ΔG = -RT ln(K).
Step 4: Identify the variables in the equation: R is the gas constant (8.314 J/(mol·K)), T is the temperature in Kelvin, and K is the equilibrium constant.
Step 5: Realize that if K is greater than 1, ΔG is negative, meaning the reaction is spontaneous in the forward direction.
Step 6: If K is less than 1, ΔG is positive, meaning the reaction is not spontaneous in the forward direction.
