Statement 1: In a zero order reaction, if the concentration of the reactant is doubled, the half-life period is also doubled.

Statement 2: For a zero-order reaction, the rate of the reaction is independent of initial concentration.

Statement I and statement II are correct but statement II is not the correct explanation of statement I

The correct answer is option 2. Statement I and statement II are correct but statement II is not the correct explanation of statement I.

Let us delve deeper into why each statement is correct or incorrect and how they relate to each other:

Statement 1: In a zero-order reaction, if the concentration of the reactant is doubled, the half-life period is also doubled.

For a zero-order reaction, the rate of the reaction is constant and does not depend on the concentration of the reactants. The integrated rate law for a zero-order reaction is:

\([A] = [A_0] - kt\)

where \([A]\) is the concentration at time \(t\), \([A_0]\) is the initial concentration, and \(k\) is the rate constant.

The half-life (\(t_{1/2}\)) is given by:

\(t_{1/2} = \frac{[A_0]}{2k}\)

This shows that the half-life is directly proportional to the initial concentration \([A_0]\). Therefore, if the initial concentration is doubled, the half-life is also doubled. This is because the half-life formula includes \([A_0]\) in the numerator.

Statement 2: For a zero-order reaction, the rate of the reaction is independent of initial concentration.

In a zero-order reaction, the rate of reaction is given by:

\(\text{Rate} = k\)

where \(k\) is the rate constant and is not affected by the concentration of reactants.

This means the rate of the reaction remains constant regardless of the concentration of reactants. The reaction proceeds at a constant rate until the reactant is consumed.

Relationship Between Statements:

Statement 1 is correct as it accurately describes the behavior of the half-life in a zero-order reaction. The half-life depends directly on the initial concentration because of how the half-life is calculated.

Statement 2 is also correct because it correctly states that in zero-order kinetics, the reaction rate does not depend on the concentration of reactants.

However, Statement 2 does not explain Statement 1. Statement 2 describes a characteristic of zero-order reactions, while Statement 1 describes how the half-life of a zero-order reaction changes with concentration. The change in half-life with concentration is a result of the proportionality in the half-life formula, not directly explained by the rate’s independence from concentration.

Conclusion:

The correct answer is: Statement I and Statement II are correct but Statement II is not the correct explanation of Statement I.