Each question contains STATEMENTS-1 (Assertion) and STATEMENT -2 (Reason).
Examine the statements carefully and mark the correct answer according to the instructions given below:
STATEMENT -1: If the activation energy of reaction is zero, temperature will have no effect on the rate constant.
STATEMENT-2: Lower the activation energy faster is the raction.

Options

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

Answer

To solve the question regarding the two statements about activation energy and reaction rates, we will analyze each statement step by step.

### Step 1: Analyze Statement 1
**Statement 1:** If the activation energy of the reaction is zero, temperature will have no effect on the rate constant.

- The activation energy (Ea) is the minimum energy required for a reaction to occur. According to the Arrhenius equation:
\[ k = A e^{-\frac{E_a}{RT}} \]
where:
- \( k \) = rate constant
- \( A \) = Arrhenius constant
- \( R \) = universal gas constant
- \( T \) = temperature in Kelvin

- If \( E_a = 0 \), the equation simplifies to:
\[ k = A e^{0} = A \]
This means that the rate constant \( k \) is equal to the Arrhenius constant \( A \) and does not depend on temperature \( T \).

### Conclusion for Statement 1:
- **Statement 1 is true.** When the activation energy is zero, the rate constant is independent of temperature.

### Step 2: Analyze Statement 2
**Statement 2:** Lower the activation energy, faster is the reaction.

- A lower activation energy means that the exponential factor in the Arrhenius equation becomes larger, which increases the rate constant \( k \).
- Since the rate of reaction is directly proportional to the rate constant, a higher \( k \) implies a faster reaction.

### Conclusion for Statement 2:
- **Statement 2 is true.** Lower activation energy results in a faster reaction due to an increase in the rate constant.

### Step 3: Determine the Relationship Between the Statements
- Both statements are true, but we need to evaluate if Statement 2 is a correct explanation for Statement 1.
- While both statements are true, Statement 2 does not explain why temperature has no effect on the rate constant when activation energy is zero. It merely states that lower activation energy leads to a faster reaction.

### Final Conclusion:
- **Both statements are true, but Statement 2 does not explain Statement 1.**

### Answer:
The correct option is that both statements are true, but Statement 2 is not the correct explanation of Statement 1.

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