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The rate equation for a reaction $\mathrm{A} \rightarrow \mathrm{B}$ is $\mathrm{r}=\mathrm{k}[\mathrm{A}]^{0}$. If the initial concentration of the reactant is $a \mathrm{~mol} \mathrm{dm}{ }^{-3}$, the half-life period of the reaction is
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$\frac{\mathrm{a}}{2 \mathrm{k}}$
$\begin{array}{lc}\mathrm{A} \longrightarrow \mathrm{B} & \\ \because \quad \mathrm{r}=\mathrm{k}[\mathrm{A}]^{0} \\ \text { or } \quad \mathrm{r}=\mathrm{k} \\ \text { This is a zero order reaction. } \\ \therefore \quad \mathrm{t}_{1 / 2}=\frac{\mathrm{a}}{2 \mathrm{k}}\end{array}$
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