What is the relationship between the Gibbs free energy change (ΔG) and the equilibrium constant (K)?
Practice Questions
1 question
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
The relationship is given by the equation ΔG = -RT ln(K), where R is the gas constant and T is the temperature in Kelvin.
Questions & Step-by-step Solutions
1 item
Q
Q: What is the relationship between the Gibbs free energy change (ΔG) and the equilibrium constant (K)?
Solution: The relationship is given by the equation ΔG = -RT ln(K), where R is the gas constant and T is the temperature in Kelvin.
Steps: 6
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.
