The rate law for the reaction : $2\mathrm{C}+\mathrm{D}\to \mathrm{A}+\mathrm{E}$ is $-\frac{\mathrm{d}\left[\mathrm{D}\right]}{\mathrm{dt}}=\mathrm{k}{\left[\mathrm{C}\right]}^2\left[\mathrm{D}\right]$

If $\mathrm{C}$ is present in large excess, the order of the reaction will be -

The half life period of a chemical reaction is given by : ${\mathrm{t}}_1\propto \frac{1}{{\mathrm{a}}^{\mathrm{n}-1}}$

The order of the reaction is :

$99\%$ of a first order reaction was completed in $32$ minutes when $99.9\%$ of the reaction will complete: