Question

Calculate the average rate of decomposition of $N_2{O}_5$ by the reaction, $2N_2{O}_5\left(g\right)⟶4N{O}_2\left(g\right)+O_2\left(g\right)$.
During the time interval from $t=600s$ to $t=1200s$ using the following data:
$\begin{array}{cc}Time& \left[N_2{O}_5\right]\\ 600s& 1.24\times {10}^{-2}M\\ 1200s& 0.93\times {10}^{-2}M\end{array}$

Answer 1

Average rate of decomposition of $N_2{O}_5$

$=\frac{-1△\left[N_2{O}_5\right]}{2△t}=\frac{-1}{2}\frac{[0.93\times {10}^{-2}-1.24\times {10}^{-2}]M}{1200-600s}$

$=-\frac{(-0.31)}{600}\times {10}^{-2}M{s}^{-1}$

$=\frac{0.051}{2}\times {10}^{-4}M{s}^{-1}$

$=0.026\times {10}^{-4}M{s}^{-1}$