Assertion : The additions of an inert gas at constant volume to a system at equilibrium does not affect the state of equilibrium
Reason: The inert gas does not react with any of the reactants or products.

Options

A. If both Assertion and Reason are CORRECT and a Reason is the CORRECT explanations of the Assertion
B. If both Assertion and Reason are CORRECT but Reaon is not CORRECT explanation of the Assertion.
C. If Assertion is CORRECT but Reasson is INCORRECT.
D. If Assertion is INCORRECT but Reason is CORRECT.

Answer

To solve the question, we need to analyze the assertion and the reason provided, and determine their validity and relationship.

### Step-by-step Solution:

1. **Understanding the Assertion**:
- The assertion states that the addition of an inert gas at constant volume to a system at equilibrium does not affect the state of equilibrium.
- This means that when an inert gas is added, the equilibrium position remains unchanged.

2. **Understanding the Reason**:
- The reason given is that the inert gas does not react with any of the reactants or products.
- This implies that since the inert gas is non-reactive, it should not influence the chemical reaction or the equilibrium.

3. **Analyzing the Effect of Inert Gas**:
- When an inert gas is added to a system at constant volume, the total pressure of the system increases.
- However, the partial pressures of the reactants and products remain unchanged because the inert gas does not participate in the reaction.

4. **Applying Le Chatelier's Principle**:
- According to Le Chatelier's Principle, if a system at equilibrium is subjected to a change (in concentration, pressure, or temperature), the system will adjust to counteract that change.
- Since the partial pressures of the reactants and products do not change with the addition of an inert gas, the equilibrium position is not affected.

5. **Conclusion**:
- The assertion is correct: adding an inert gas at constant volume does not affect the equilibrium state.
- The reason is also correct: the inert gas does not react with the reactants or products.
- However, the reason does not adequately explain why the assertion is true, as the lack of reaction is not the primary reason for the unchanged equilibrium state; rather, it is the unchanged partial pressures that are crucial.

### Final Answer:
- Both the assertion and reason are correct, but the reason is not the correct explanation for the assertion.