A zero order reaction $\mathrm{A}⟶\mathrm{B}$ is half completed in time equal to

In a zero order reaction, the amount of time needed to finish half the reactant is equal to $\mathrm{a}/\left(2\mathrm{k}\right)$.
The amount of time needed for the concentration of the radioactive chemical to drop to half of its initial value is known as the half life $\left({\mathrm{t}}_{1/2}\right)$) of a reaction. A zero-order reaction's half-life can be calculated as follows:

According to the definition of a half-life, the time it takes for half of the initial concentration of reactant a to react in a reaction involving reactant an is known as ${\mathrm{t}}_{1/2}$. The following results can be obtained by substituting these new criteria into the integrated rate law form:

$1/2\left[\mathrm{a}\right]=-{\mathrm{kt}}_{1/2}+\mathrm{a}$
The result of solving for$t_{1/2}$ is as follows:

${\mathrm{t}}_{1/2}=\mathrm{a}/\left(2\mathrm{k}\right)$