What is the relationship between Gibbs Free Energy and the equilibrium constant

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Question: What is the relationship between Gibbs Free Energy and the equilibrium constant (K)?

Options:

Correct Answer: ΔG = -RT ln(K)

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 Gibbs Free Energy and the equilibrium constant (K)?

What is the relationship between Gibbs Free Energy and the equilibrium constant (K)?

Correct Answer: ΔG = -RT ln(K)

Step 1: Understand that Gibbs Free Energy (ΔG) is a measure of the energy available to do work in a system.
Step 2: Know that the equilibrium constant (K) tells us the ratio of products to reactants at equilibrium in a chemical reaction.
Step 3: Learn the formula that connects ΔG and K: ΔG = -RT ln(K).
Step 4: Identify the variables in the formula: R is the gas constant (approximately 8.314 J/(mol·K)), T is the temperature in Kelvin, and ln(K) is the natural logarithm of the equilibrium constant K.
Step 5: Realize that if ΔG is negative, the reaction is spontaneous and K is greater than 1, meaning products are favored.
Step 6: If ΔG is positive, the reaction is non-spontaneous and K is less than 1, meaning reactants are favored.

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