Assertion:- The reaction quotient Q, has the same presentation form as the equilibrium constant K and Q is evaluated using any given concentrations of the species involved in the reaction, and not necesssarily equilibrium concenetrations.
Reason:- If the numerical value of Q is not the same as the value of equilibrium constant, that time reaction will never proceed.

Options

A. If both Assertion `&` Reason are True `&` the Reason is a correct explanation of the Assertion.
B. If both Assertion `&` Reason are True but Reason is not a correct explanation of the Assertion.
C. If Assertion is True but the Reason is False.
D. If both Assertion `&` Reason are False.

Answer

To solve the assertion-reason question, we need to analyze both the assertion and the reason separately.

### Step 1: Analyze the Assertion
The assertion states: "The reaction quotient Q has the same presentation form as the equilibrium constant K, and Q is evaluated using any given concentrations of the species involved in the reaction, and not necessarily equilibrium concentrations."

- **Explanation**:
- The reaction quotient \( Q \) is calculated using the concentrations of reactants and products at any point in time, not just at equilibrium.
- The expression for \( Q \) is similar to that of the equilibrium constant \( K \), which is defined at equilibrium.
- For a general reaction \( aA + bB \rightleftharpoons cC + dD \), the expressions are:
- \( K = \frac{[C]^c [D]^d}{[A]^a [B]^b} \) (at equilibrium)
- \( Q = \frac{[C]^c [D]^d}{[A]^a [B]^b} \) (at any time)

Thus, the assertion is **true**.

### Step 2: Analyze the Reason
The reason states: "If the numerical value of Q is not the same as the value of the equilibrium constant, that time reaction will never proceed."

- **Explanation**:
- This statement is **false**.
- If \( Q \) is not equal to \( K \), it does not mean the reaction will not proceed. Instead:
- If \( Q < K \), the reaction will shift to the right (towards products) to reach equilibrium.
- If \( Q > K \), the reaction will shift to the left (towards reactants) to reach equilibrium.
- Therefore, the reaction can proceed in either direction depending on the relationship between \( Q \) and \( K \).

Thus, the reason is **false**.

### Conclusion
- The assertion is true, and the reason is false. Therefore, the correct answer is that the assertion is true, but the reason is false.

### Final Answer
Assertion: True
Reason: False
Correct Option: C

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