Each question contains STATEMENT-1 (Assertion) and STATEMENT-2( Reason).
Examine the statements carefully and mark the correct answer according to the instruction given below:
STATEMENT-1: Equilibrium constant for the reverse reaction is the inverse of the equilibrium constant for the reaction in the forward direction.
STATEMENT-2: Equilibrium constant depends upon the way in which the reaction is written.

Options

A. (a) If both the statements are TRUE and STATEMENT-2 is the correct explanation of STATEMENT-1
B. (b) both the statement are TRUE but STATEMENT-2 is NOT the correct explanation of STATEMENT-1
C. (c) If STATEMENT-1 is TRUE and STATEMENT-2 is FALSE
D. (d) If STATEMENT-1 is FALSE and STATEMENT-2 is TRUE

Answer

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

**STATEMENT-1**: Equilibrium constant for the reverse reaction is the inverse of the equilibrium constant for the reaction in the forward direction.

**STATEMENT-2**: Equilibrium constant depends upon the way in which the reaction is written.

### Step-by-Step Solution:

1. **Understanding Equilibrium Constant**:
- The equilibrium constant (K) for a reaction at equilibrium is defined as the ratio of the concentrations of products to reactants, each raised to the power of their respective stoichiometric coefficients.

2. **Writing the Forward Reaction**:
- Consider a general reaction:
\[ aA + bB \rightleftharpoons cC + dD \]
- The equilibrium constant for this forward reaction (K) can be expressed as:
\[ K = \frac{[C]^c [D]^d}{[A]^a [B]^b} \]

3. **Writing the Reverse Reaction**:
- The reverse reaction would be:
\[ cC + dD \rightleftharpoons aA + bB \]
- The equilibrium constant for this reverse reaction (K') can be expressed as:
\[ K' = \frac{[A]^a [B]^b}{[C]^c [D]^d} \]

4. **Relating K and K'**:
- If we compare K and K', we can see that:
\[ K' = \frac{1}{K} \]
- This shows that the equilibrium constant for the reverse reaction is indeed the inverse of the equilibrium constant for the forward reaction.

5. **Analyzing STATEMENT-1**:
- Since we have established that the equilibrium constant for the reverse reaction is the inverse of that for the forward reaction, **STATEMENT-1 is true**.

6. **Analyzing STATEMENT-2**:
- The equilibrium constant does depend on how the reaction is written. For instance, if we reverse a reaction or multiply the coefficients by a factor, the equilibrium constant will change accordingly.
- Thus, **STATEMENT-2 is also true**.

7. **Conclusion**:
- Both statements are true, and STATEMENT-2 provides the correct explanation for STATEMENT-1. Therefore, the correct answer is that both statements are true, and the reason is the correct explanation of the assertion.

### Final Answer:
Both statements are true, and statement 2 is the correct explanation of statement 1.

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