Each question given below contains STATEMENT -1 (Assertion) and STATEMENT -2 (Reason). It has four choice (a), (b), ( c ) and (d) out of which ONLY ONE is correct . Choose the correct option as under :
Statement -1. Reaction quotiet of a reaction at any time decides the direction in which the reaction will proceed.
Statement -2. The value of reaction quotient cannot be greater than the equilibrium constant .

Explanation

To solve the given question, we need to analyze both statements provided:

**Statement 1 (Assertion):** The reaction quotient of a reaction at any time decides the direction in which the reaction will proceed.

**Statement 2 (Reason):** The value of the reaction quotient cannot be greater than the equilibrium constant.

### Step-by-Step Solution:

1. **Understanding Reaction Quotient (Q):**
- The reaction quotient (Q) is a measure of the relative concentrations of reactants and products at any point in time during a chemical reaction. It is calculated using the same expression as the equilibrium constant (K), but with the current concentrations instead of equilibrium concentrations.
- For a general reaction \( aA + bB \rightleftharpoons cC + dD \), the reaction quotient \( Q \) is given by:
\[ Q = \frac{[C]^c [D]^d}{[A]^a [B]^b} \]

2. **Determining the Direction of the Reaction:**
- The direction in which the reaction will proceed can be determined by comparing Q to K:
- If \( Q < K \): The reaction will proceed in the forward direction (towards products).
- If \( Q > K \): The reaction will proceed in the backward direction (towards reactants).
- If \( Q = K \): The reaction is at equilibrium.
- Therefore, Statement 1 is **true**.

3. **Understanding the Equilibrium Constant (K):**
- The equilibrium constant (K) is a specific value at a given temperature that describes the ratio of products to reactants at equilibrium.
- There is no theoretical limit that prevents \( Q \) from being greater than \( K \). In fact, \( Q \) can be greater than, less than, or equal to \( K \) depending on the concentrations of the reactants and products.
- Therefore, Statement 2 is **false**.

### Conclusion:
- **Statement 1 is true** and **Statement 2 is false**.

### Correct Option:
The correct option is (a): Statement 1 is true, Statement 2 is false.

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