According to Le-Chatelier's principle, the equilibrium constant of a reversible reaction will not shift by

Options

A. Increasing the temperature of an exothermic reaction
B. Increasing the temperature of an endothermic reaction
C. Changing the concentrations of the reactants
D. The effect of a catalyst

Explanation

To solve the question regarding Le-Chatelier's principle and the equilibrium constant of a reversible reaction, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding Le-Chatelier's Principle**:
- Le-Chatelier's principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust itself to counteract that change and restore a new equilibrium.

2. **Identifying Factors Affecting Equilibrium**:
- The factors that can affect the equilibrium position include:
- Change in concentration of reactants or products
- Change in temperature
- Change in pressure (for gaseous reactions)
- Change in volume (which indirectly affects pressure)

3. **Effect of Temperature on Equilibrium Constant**:
- The equilibrium constant (K) is dependent on temperature. For an exothermic reaction, increasing the temperature will shift the equilibrium to the left (toward the reactants), while for an endothermic reaction, increasing the temperature shifts the equilibrium to the right (toward the products).

4. **Conclusion about the Equilibrium Constant**:
- The equilibrium constant itself does not shift due to changes in concentration or pressure. It only changes with temperature. Therefore, the equilibrium constant remains constant unless there is a change in temperature.

5. **Final Answer**:
- According to Le-Chatelier's principle, the equilibrium constant of a reversible reaction will not shift by changes in concentration, pressure, or volume. The correct answer is that it does not shift due to these factors.