$\mathrm{r}=\mathrm{k}[\mathrm{A}]$ for a reaction, $50 \%$ of A is decomposed in 120 minutes. The time taken for $90 \%$ decomposition of $A$ is $\_\_\_\_$ minutes.

$\mathrm{NO}_2$ required for a reaction is produced by decomposition of $\mathrm{N}_2 \mathrm{O}_5$ in $\mathrm{CCl}_4$ as by equation $2 \mathrm{~N}_2 \mathrm{O}_{5(\mathrm{~g})} \rightarrow 4 \mathrm{NO}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}$
The initial...

The half-life of radioisotopic bromine - 82 is 36 hours. The fraction which remains after one day is $\times 10^{-2}$. (Given antilog $0.2006=1.587$ )

Time required for completion of $99.9 \%$ of a First order reaction is times of half life $\left(t_{1 / 2}\right)$ of the reaction.

Half life of zero order reaction $\mathrm{A} \rightarrow$ product is 1 hour, when initial concentration of reactant is $2.0 \mathrm{molL}^{-1}$. The time required to decrease...

Consider the following plots of log of rate constant $k(\log k)$ vs $\frac{1}{T}$ for three different reactions. The correct order of activation energies of these...