Question

For the reaction

$2N_2{O}_5\left(g\right)⟶4N{O}_2\left(g\right)+O_2\left(g\right),$
the rate of formation of $N{O}_2\left(g\right)$ is $2.8\times {10}^{-3}mol{s}^{-1}.$ Calculate the rate of disapperance of $N_2{O}_5\left(g\right).$

Answer 1

$2N_2{O}_5\left(g\right)⟶4N{O}_2\left(g\right)+O_2\left(g\right)$

$-\frac{1}{2}\frac{d\left[N_2{O}_5\right]}{dt}=\frac{1}{4}\frac{d\left[N{O}_2\right]}{dt}$

$\frac{d\left[N_2{O}_5\right]}{dt}=\frac{2}{4}\times 2.8\times {10}^{-3}$

= $1.4\times {10}^{-3}$

So, rate of disappearance of $N_2{O}_5\left(g\right)$

= $1.4\times {10}^{-3}mol{s}^{-1}$