What is the relationship between the equilibrium constant (K) and the Gibbs free

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Question: What is the relationship between the equilibrium constant (K) and the Gibbs free energy change (ΔG) at standard conditions? (2022)

Options:

Correct Answer: ΔG = -RT ln(K)

Exam Year: 2022

Solution:

The relationship is given by ΔG = -RT ln(K), where R is the gas constant and T is the temperature in Kelvin.

What is the relationship between the equilibrium constant (K) and the Gibbs free energy change (ΔG) at standard conditions? (2022)

What is the relationship between the equilibrium constant (K) and the Gibbs free energy change (ΔG) at standard conditions? (2022)

Step 1: Understand that ΔG represents the change in Gibbs free energy for a reaction.
Step 2: Know that K is the equilibrium constant, which tells us the ratio of products to reactants at equilibrium.
Step 3: Recognize that the equation ΔG = -RT ln(K) connects ΔG and K.
Step 4: Identify R as the gas constant, which is approximately 8.314 J/(mol·K).
Step 5: Remember that T is the temperature in Kelvin, which is important for the calculation.
Step 6: Realize that if K is greater than 1, ΔG will be negative, indicating that the reaction is spontaneous.
Step 7: Conversely, if K is less than 1, ΔG will be positive, indicating that the reaction is non-spontaneous.

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