In the reaction,$N_{2} + 3H_{2} \longrightarrow 2NH_{3}$,the rate of disappearance of $H_{2}$ is $0.02 \ M/s$. The rate of appearance of $NH_{3}$ is (in $M/s$)

Ammonia and oxygen react at high temperature as $4 NH_{3(g)} + 5 O_{2(g)} \longrightarrow 4 NO_{(g)} + 6 H_2 O_{(g)}$. If the rate of formation of $NO_{(g)}$ is $3.6 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$,then the rate of disappearance of ammonia is:

For a given reaction $3A + B \to C + D$,the rate of reaction can be represented by:

Explain how the rate of reaction depends on concentration and time using graphs.

For the reaction $5Br_{(aq)}^{-} + BrO_{3_{(aq)}}^{-} + 6H_{(aq)}^{+} \rightarrow 3Br_{2_{(aq)}} + 3H_{2}O_{(l)}$,if $\frac{-\Delta[Br^{-}]}{\Delta t} = 4.2 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$,calculate the rate of formation of $Br_{2}$,i.e.,$\frac{\Delta[Br_{2}]}{\Delta t}$.

The rate of reaction is expressed as
$+\frac{1}{2}\frac{d[C]}{dt} = -\frac{1}{3}\frac{d[D]}{dt} = +\frac{1}{4}\frac{d[A]}{dt} = -\frac{d[B]}{dt}$
The reaction is: