What is the relationship between the Gibbs free energy change (ΔG) and the equil

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

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

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) indicates the ratio of products to reactants at equilibrium.
Step 3: Recognize that at standard conditions, ΔG and K are related by the equation ΔG = -RT ln K.
Step 4: In this equation, R is the universal gas constant and T is the temperature in Kelvin.
Step 5: 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.
Step 7: If K equals 1, ΔG is zero, indicating the system is at equilibrium.

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