The rate equation for a reaction, $\mathrm{N}_{2} \mathrm{O} \longrightarrow \mathrm{N}_{2}+1 / 2…
$\mathrm{N}_{2} \mathrm{O} \longrightarrow \mathrm{N}_{2}+1 / 2 \mathrm{O}_{2}$
is Rate $=\mathrm{k}\left[\mathrm{N}_{2} \mathrm{O}ight]^{0}=\mathrm{k}$. If the initial concentration of the reactant is $a$ mol $\mathrm{Lit}^{-1}$, the half-life period of the reaction is
- $t_{\frac{1}{2}}=\frac{a}{2 k}$
- $-t_{\frac{1}{2}}=k a$
- $t_{\frac{1}{2}}=\frac{a}{k}$
- $t_{\frac{1}{2}}=\frac{k}{a}$
Solution
$t_{1 / 2}=\frac{a}{2 k}$ .
Asked in: JEE-TOPICTESTS-CHEMISTRY