Question

Ammonia and oxygen reacts at higher temperatures as $4N{H}_3\left(g\right)+5O_2\left(g\right)\to 4NO\left(g\right)+6H_{2}O\left(g\right)$
In an experiment, the concentration of $NO$ increase by $1.08\times {10}^{-2}mollitr{e}^{-1}$ in $3$ seconds. calculate.
(i) rate of reaction.
(ii) rate of disappearance of ammonia
(iii) rate of formation of water

Answer 1

$4N{H}_3+5O_2\to 4NO+6H_{2}O$,

(i) rate of reaction = $\frac{1}{4}\times \frac{dN{H}_3}{dt}$

= $\frac{1}{4}\times \frac{1.08\times {10}^{-2}}{3}$

= $9\times {10}^{-4}$

(ii)rate of dissappearance of ammonia$\times (-\frac{1}{4})$ =rate ofreaction

=$9\times {10}^{-4}\times 4$

=$36\times {10}^{-4}$

(iii)rate of formation of water =$5\times$ rate of reaction

=$5\times 9\times {10}^{-4}$

=$45\times {10}^{-4}$