Question

What is the ratio between the rate of decomposition of $N_2{O}_5$ to rate of formation of $N{O}_2$?
$2N_2{O}_{5\left(g\right)}⟶4N{O}_{2\left(g\right)}+O_{2\left(g\right)}$

• A. 1:4
• B. 4:1
• C. 2:1
• D. 1:2

Answer 1

The correct option is D 1:2

The rate of the reaction, $r=-\frac{1}{2}\frac{d}{dt}\left[N_2{O}_5\right]=\frac{1}{4}\frac{d}{dt}\left[N{O}_2\right]=\frac{d}{dt}\left[O_2\right]$

The ratio between the rate of decomposition of $N_2{O}_5$ to rate of formation of $N{O}_2$ is $1:2$.

$2N_2{O}_{5\left(g\right)}⟶4N{O}_{2\left(g\right)}+O_{2\left(g\right)}$

The rate of decomposition of $N_2{O}_5$ is twice the rate of the reaction.
The rate of formation of $N{O}_2$ is four times the rate of the reaction.
The ratio between the rate of decomposition of $N_2{O}_5$ to rate of formation of $N{O}_2$ is $2:4$ or $1:2$.