Statement-1. In a zero order reaction, if concentration of the reactant is doubled, half-life period is also doubled.
Statement-2. The total time taken for a zero order reaction to complete is double of the half-life period.

Options

A. Statement-1 is True, Statement-2 is True , Statement-1 is a correct explanation of Statement-1.
B. Statement-1 is True, Statement-2 is True , Statement-2 is NOT the correct explanation of Statement-1.
C. Statement-1 is True, Statement-2 is False.
D. Statement-1 is False, Statement-2 is True.

Explanation

To solve the question regarding the statements about zero-order reactions, we will analyze each statement step by step.

### Step 1: Understanding Zero-Order Reactions
In a zero-order reaction, the rate of reaction is constant and does not depend on the concentration of the reactants. The rate law can be expressed as:
\[ \text{Rate} = k \]
where \( k \) is the rate constant.

### Step 2: Half-Life of a Zero-Order Reaction
The half-life (\( t_{1/2} \)) for a zero-order reaction is given by the formula:
\[ t_{1/2} = \frac{[A]_0}{2k} \]
where \( [A]_0 \) is the initial concentration of the reactant.

### Step 3: Analyzing Statement 1
**Statement 1:** "In a zero-order reaction, if the concentration of the reactant is doubled, the half-life period is also doubled."

If we double the initial concentration \( [A]_0 \):
\[ t_{1/2} = \frac{2[A]_0}{2k} = \frac{[A]_0}{k} \]
This shows that the half-life is directly proportional to the initial concentration. Therefore, if the concentration is doubled, the half-life will also double.

**Conclusion for Statement 1:** This statement is **True**.

### Step 4: Analyzing Statement 2
**Statement 2:** "The total time taken for a zero-order reaction to complete is double the half-life period."

For a zero-order reaction, the total time (\( t \)) taken to complete the reaction can be calculated using the formula:
\[ t = \frac{[A]_0}{k} \]
This total time is equal to the sum of the half-lives. Since the half-life is given as \( t_{1/2} = \frac{[A]_0}{2k} \), the total time for the reaction to go to completion is:
\[ t = 2 \times t_{1/2} \]
Thus, the total time taken is indeed double the half-life period.

**Conclusion for Statement 2:** This statement is **True**.

### Final Conclusion
Both statements are true, but Statement 2 is not a direct explanation for Statement 1. Therefore, the correct answer is that both statements are true, but Statement 2 is not the correct explanation of Statement 1.

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