Relationship between Equilibrium Constant Kc and Gibbs Free Energy (? G)
The equilibrium constant Kc and Gibbs free energy (? G) of a reaction are related through the following equation:

G = -RT ln(Kc)
Where:
- G is the Gibbs free energy
- R is the gas constant
- T is the temperature in Kelvin
- Kc is the equilibrium constant

Interpretation
1. Gibbs Free Energy (G): Gibbs free energy is a measure of the amount of work that can be extracted from a system at constant temperature and pressure. A negative ? G value indicates a spontaneous reaction, while a positive value indicates a non-spontaneous reaction.
2. Equilibrium Constant (Kc): The equilibrium constant Kc is a measure of the extent to which a reaction proceeds to form products at equilibrium. A higher Kc value indicates a greater concentration of products at equilibrium.
3. Relationship: The equation relating G and Kc shows that there is an inverse relationship between the equilibrium constant and Gibbs free energy. As the equilibrium constant increases, the Gibbs free energy decreases, and vice versa. This means that a reaction with a high equilibrium constant will have a lower Gibbs free energy, making it more favorable.
In conclusion, the equilibrium constant Kc and Gibbs free energy are inversely related, where a higher Kc value corresponds to a lower ? G value, indicating a more favorable reaction.