Question

The oxidation of ammonia takes place as, $4N{H}_3\left(g\right)+3O_2\left(g\right)⟶2N_2\left(g\right)+6H_{2}O\left(g\right)$, if the rate of formation of $N_2$ is $0.7M/s$, determine the rate at which $N{H}_3$ is consumed:

• A. $1.4$ $mol$ $L^{-1}{s}^{-1}$
• B. $0.7$ $mol$ $L^{-1}{s}^{-1}$
• C. $1.5$ $mol$ $L^{-1}{s}^{-1}$
• D. none of the above

Answer 1

The correct option is A $1.4$ $mol$ $L^{-1}{s}^{-1}$

For given reaction,

$-\frac{1}{4}\frac{d\left[N{H}_3\right]}{dt}=+\frac{1}{2}\frac{d\left[N_2\right]}{dt}$

$-\frac{d\left[N{H}_3\right]}{dt}=2\frac{d\left[N_2\right]}{dt}=2\times 0.7=1.4M/s$