Question

Given below are two statements
Assertion (A): A catalyst generally increases the rate of a reaction
Reason (R): It lowers the activation energy of a reaction by providing a new path

• A. Both (A) and (R) are correct and (R) is the correct explanation of (A)
• B. Both (A) and (R) are correct and (R) is not the correct explanation of (A)
• C. (A) is correct but (R) is not correct
• D. (A) is not correct but (R) is correct

Hint:

A catalyst speeds up a reaction by lowering the activation energy, which is the key reason for the increased rate. Check if the reason directly explains the assertion in such questions.

Answer 1

The Correct Option is A

Let's evaluate the given statements:
- Assertion (A): A catalyst generally increases the rate of a reaction. This is correct. A catalyst increases the rate of a reaction by providing an alternative reaction pathway, allowing the reaction to proceed faster.
- Reason (R): It lowers the activation energy of a reaction by providing a new path. This is also correct. The primary mechanism by which a catalyst increases the reaction rate is by lowering the activation energy, which is the energy barrier that reactants must overcome to form products.
Now, we need to determine if (R) is the correct explanation of (A). Since a catalyst increases the reaction rate precisely because it lowers the activation energy (as stated in R), the reason directly explains the assertion. Therefore, both (A) and (R) are correct, and (R) is the correct explanation of (A).
So, the correct answer is Both (A) and (R) are correct and (R) is the correct explanation of (A).

Answer 2

Given below are two statements

Assertion (A): A catalyst generally increases the rate of a reaction
Reason (R): It lowers the activation energy of a reaction by providing a new path

Step 1: Understand the role of a catalyst:
A catalyst is a substance that increases the rate of a chemical reaction without itself undergoing permanent chemical change. It does not alter the final equilibrium position but helps the system reach equilibrium faster.

Step 2: Mechanism of action:
A catalyst works by providing an alternative reaction pathway with a lower activation energy. Activation energy is the minimum energy required for a chemical reaction to occur. By lowering this barrier, more reactant molecules can successfully collide and form products, increasing the reaction rate.

Step 3: Analyze the given statements:
- Assertion (A) is correct because a catalyst does indeed increase the rate of a reaction.
- Reason (R) is also correct because the primary function of a catalyst is to lower the activation energy.
- Additionally, the reason given clearly explains why the assertion is true.

Final Answer:
\[ \boxed{\text{Both (A) and (R) are correct and (R) is the correct explanation of (A)}} \]