Equilibrium Constant and Temperature

The equilibrium constant is a fundamental concept in thermodynamics that describes the extent of a chemical reaction at equilibrium. It is represented by the symbol K and is defined as the ratio of the concentrations (or partial pressures) of the products to the concentrations (or partial pressures) of the reactants, with each concentration raised to the power of its stoichiometric coefficient. The equilibrium constant is a dimensionless quantity and provides valuable information about the equilibrium position of a reaction.

Factors Affecting Equilibrium Constant
The equilibrium constant is influenced by various factors, including temperature, pressure, and concentrations of reactants and products. However, it is important to note that the equilibrium constant only depends on temperature, while the concentrations and pressures of reactants and products affect the position of the equilibrium.

Explanation of Temperature Dependence
The dependence of the equilibrium constant on temperature can be explained by considering the principles of thermodynamics and the concept of Gibbs free energy. The Gibbs free energy change (∆G) for a chemical reaction is related to the equilibrium constant by the equation:

∆G = -RT ln(K)

Where:
∆G is the Gibbs free energy change
R is the gas constant
T is the temperature in Kelvin
ln(K) is the natural logarithm of the equilibrium constant

From the above equation, it is evident that the equilibrium constant is directly related to the Gibbs free energy change and the temperature. The Gibbs free energy change (∆G) determines the spontaneity of a reaction. If ∆G is negative, the reaction is spontaneous in the forward direction; if ∆G is positive, the reaction is non-spontaneous in the forward direction; and if ∆G is zero, the reaction is at equilibrium.

Effect of Temperature on Equilibrium Constant
The temperature dependence of the equilibrium constant can be understood by considering the effect of temperature on the value of ∆G. As the temperature increases, the value of ∆G becomes more negative or less positive, resulting in changes in the equilibrium constant.

- Increase in Temperature:
When the temperature is increased, the value of ∆G becomes more negative. This is because the term -RT ln(K) becomes more negative as T increases, causing ∆G to decrease. As a result, the equilibrium constant K increases.

- Decrease in Temperature:
Conversely, when the temperature is decreased, the value of ∆G becomes less negative or more positive. The term -RT ln(K) becomes less negative as T decreases, causing ∆G to increase. Consequently, the equilibrium constant K decreases.

Conclusion
In conclusion, the equilibrium constant depends only on temperature because it is directly related to the Gibbs free energy change (∆G) of a reaction. As the temperature is increased, the equilibrium constant increases, indicating a shift towards the products. Conversely, as the temperature is decreased, the equilibrium constant decreases, indicating a shift towards the reactants. The temperature dependence of the equilibrium constant can be explained by considering the effect of temperature on the value of ∆G and the principles of thermodynamics.

No.
it depends on another also like pressure and concentration of reactants and products also.
if reaction is exothermic and we increase the temperature then equilibrium will shift towards reactants and if reaction is endothermic and we increase the temperature then reaction will shift towards products.
I hope it is correct. actually I am not sure about it.