Question

The decomposition of $N_2{O}_5$ at 318 K according to the following equation follows first order reaction:
$N_2{O}_5\left(g\right)\to 2N{O}_2\left(g\right)+1/2O_2\left(g\right)$
The initial concentration of $N_2{O}_5$ was $1.24\times {10}^{-2}$ mol $L^{-1}$ and after 60 minutes was $0.20\times {10}^{-2}$ mo $L^{-1}$, Calculate the rate constant of the reaction at 318 K.

Answer 1

$N_2{O}_5\to 2N{O}_2+\frac{1}{2}{O}_2$

$t=0$ $1.24\times {10}^{-2}$

$t=60$ $0.2\times {10}^{-2}$

For first order reaction ,

$\lambda =\frac{1}{T}ln\left(\frac{Co}{Cl}\right)$

$=\frac{1}{60}\times ln\left(\frac{1.24}{0.20}\right)$

$\Rightarrow$ $\lambda$ = $0.0304$ mol $L^{-1}$ $mi{n}^{-1}$