Assertion : If reaction quotient, `Q_(c)` for a particular reaction is greater than `K_(c)` the reaction will proceed in the direction of reactants.
Reason : Reaction quotient is defined in the same way as the equilibrium constant `K_(c)` except that the concentrations in `Q_(c)` are not necessarily equilibrium values. (a)If both assertion and reason are true and reason is the correct explanation of assertion. (b)If both assertion and reason are true but reason is not the correct explanation of assertion. (c)If assertion is true but reason is false. (d)If both assertion and reason are false

Options

A. If both assertion and reason are true and reason is the correct explanation of assertion.
B. If both assertion and reason are true but reason is not the correct explanation of assertion.
C. If assertion is true but reason is false.
D. If both assertion and reason are false.

Explanation

To solve the question, we need to analyze the assertion and the reason given.

### Step-by-Step Solution:

1. **Understanding the Assertion**:
- The assertion states: "If the reaction quotient, \( Q_c \), for a particular reaction is greater than \( K_c \), the reaction will proceed in the direction of reactants."
- This means that when the concentration of products (as represented in \( Q_c \)) is higher than what it would be at equilibrium (represented by \( K_c \)), the reaction will shift to the left (toward the reactants) to reach equilibrium.

2. **Understanding the Reason**:
- The reason states: "Reaction quotient is defined in the same way as the equilibrium constant \( K_c \) except that the concentrations in \( Q_c \) are not necessarily equilibrium values."
- This is true because both \( Q_c \) and \( K_c \) are calculated using the same formula, but \( Q_c \) can be calculated at any point in time during the reaction, while \( K_c \) is calculated only at equilibrium.

3. **Evaluating the Truth of the Statements**:
- The assertion is true because if \( Q_c > K_c \), the reaction will indeed shift toward the reactants to decrease \( Q_c \) until it equals \( K_c \).
- The reason is also true as it correctly describes the relationship between \( Q_c \) and \( K_c \).

4. **Determining the Relationship**:
- While both statements are true, the reason does not directly explain why the assertion is true. The reason merely states how \( Q_c \) is defined, but it does not clarify why a higher \( Q_c \) leads to a shift toward the reactants.

5. **Conclusion**:
- Since both the assertion and reason are true, but the reason is not the correct explanation for the assertion, the correct answer is (b): "If both assertion and reason are true but reason is not the correct explanation of assertion."