Select the correct statement.

For the zero order reaction, the half-life of a reaction is directly proportional to the initial concentration of the reactant, whereas for the first order reaction, the half-life is independent of the initial concentration of the reacting species.

The correct answer is Option (1) → For the zero order reaction, the half-life of a reaction is directly proportional to the initial concentration of the reactant, whereas for the first order reaction, the half-life is independent of the initial concentration of the reacting species.

For zero-order reaction:

$t_{1/2} = \frac{[A]_0}{2k} \quad \text{(directly proportional to initial concentration)}$

For first-order reaction:

$t_{1/2} = \frac{0.693}{k} \quad \text{(independent of initial concentration)}$

Correct answer: OPTION 1 : For the zero order reaction, the half-life of a reaction is directly proportional to the initial concentration of the reactant, whereas for the first order reaction, the half-life is independent of the initial concentration of the reacting species.

 OTHER OPTIONS 

OPTION 2 : For the zero order reaction, the half-life of a reaction is inversely proportional to the initial concentration of the reactant, whereas for the first order reaction, the half-life is independent of the initial concentration of the reacting species. Incorrect.

In zero order reactions, half-life is directly proportional, not inversely proportional.

OPTION 3 : The half-life of a reaction is directly proportional to the initial concentration of the reacting species for both zero and first order reactions. Incorrect.

For first order reactions, half-life is independent of initial concentration. 

OPTION 4 : The half-life of a reaction is inversely proportional to the initial concentration of the reacting species for both zero and first order reactions. Incorrect.

Neither zero order nor first order reactions follow this relation.