Question

In the following reaction $2H_2{O}_2\left(aq\right)\to 2H_{2}O\left(l\right)+O_2\left(g\right)$ rate of formation of $O_2$ is $36g.mi{n}^{-1}$,

(a) What is rate of formation of $H_{2}O$?
(b) What is rate of disappearance of $H_2{O}_2$?

Answer 1

$2H_2{O}_2(a.q)\to 2H_{2}O\left(l\right)+O_2\left(g\right)$

$-\frac{1}{2}\frac{d\left[H_2{O}_2\right]}{dt}=+\frac{1}{2}\frac{d\left[H_{2}O\right]}{dt}=\frac{d\left[O_2\right]}{dt}$

Given $\frac{d\left[O_2\right]}{dt}=36gmi{n}^{-1}$

$\frac{d\left[O_2\right]}{dt}=\frac{36}{32}molmi{n}^{-1}$

$\frac{d\left[H_{2}O\right]}{dt}=2\frac{d\left[O_2\right]}{dt}=2\times \frac{36}{32}\times 18gmi{n}^{-1}$

$\frac{d\left[H_2{O}_2\right]}{dt}=-2\frac{d\left[O_2\right]}{dt}=-2\times \frac{36}{32}\times 34gmi{n}^{-1}$