To solve this problem, we need to understand the relationship between the initial concentration of the reactant and the half-life period for a zero-order reaction.$\newline$For a zero-order reaction, the rate of reaction is independent of the concentration of the reactant.$\newline$The rate law for a zero-order reaction is given by:$\newline$Rate$= k \newline$where $k$ is the rate constant.$\newline$The integrated rate equation for a zero-order reaction is:$\newline [A] = [A]_0 - kt \newline$where $[A]$ is the concentration of the reactant at time $t,$ and $[A]_0$ is the initial concentration.$\newline$The half-life $(t_{1/2})$ for a zero-order reaction is given by:$\newline t_{1/2} = \frac{[A]_0}{2k} \newline$From this equation, we can see that the half-life is directly proportional to the initial concentration $[A]_0. \newline$Therefore, if the initial concentration of the reactant is doubled, the half-life period will also be doubled.$\newline$This corresponds to Option 2.