Assertion (A) : The rate of reaction can also increase w.r.t its product if one of the products act as catalyst
Reason (R) : A catalyst lowers the activation energy of reactions.

Options

A. Both (A) and (R) are true (R) is the correct explanation to (A)
B. Both (A) and (R) are true but (R) is not the correct explanation to (A)
C. (A) is true but (R) is false
D. Both (A) and (R) are false

Explanation

**Step-by-Step Solution:**

1. **Understanding the Assertion (A)**: The assertion states that the rate of reaction can increase with respect to its product if one of the products acts as a catalyst. This implies that a product can influence the rate of the reaction positively by acting as a catalyst.

2. **Understanding the Reason (R)**: The reason provided states that a catalyst lowers the activation energy of reactions. This is a fundamental property of catalysts; they provide an alternative pathway for the reaction with a lower activation energy, thereby increasing the rate of the reaction.

3. **Analyzing the Relationship**: Both the assertion and the reason are true. The assertion is valid because if a product acts as a catalyst, it can indeed increase the rate of the reaction. The reason is also true as it explains the mechanism by which catalysts work.

4. **Conclusion**: Since both the assertion and the reason are true, and the reason correctly explains the assertion, we conclude that both statements are correct, and the reason is a valid explanation for the assertion.

**Final Answer**: Both Assertion (A) and Reason (R) are true, and R is the correct explanation of A.

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