For the following reaction in aqueous solution,what happens to the rate of reaction if $HCl$ is added?
$NH_2NO_{2(aq)} + OH^-_{(aq)} \to NHNO^-_{2(aq)} + H_2O_{(l)}$
$NHNO^-_{2(aq)} \to N_2O_{(aq)} + OH^-_{(aq)}$

For the reaction,$A + 3 B \rightarrow 2 C$,the rate of consumption of $A$ is $1.4 \ mol \ dm^{-3} \ minute^{-1}$. Calculate the rate of consumption of $B$.

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:

$5 Br^{-}_{(aq)} + BrO^{-}_{3(aq)} + 6 H^{+}_{(aq)} \rightarrow 3 Br_{2(aq)} + 3 H_{2}O_{(l)}$
The rate of consumption of $H^{+}$ is $x \ mol \ L^{-1} \ s^{-1}$.
$(a)$ What is the rate of consumption of $Br^{-}$?
$(b)$ What is the rate of formation of $Br_{2}$?

For the reaction ${N_2}_{(g)} + 3{H_2}_{(g)} \to 2N{H_3}_{(g)}$,what is the relationship between $\frac{d[N{H_3}]}{dt}$ and $-\frac{d[{H_2}]}{dt}$?

At $298 \ K$ the value of $-\frac{\Delta[Br^{-}]}{\Delta t}$ for the reaction$5Br^-{_{\text{(aq)}}} + BrO_3^-{_{\text{(aq)}}} + 6H^+{_{\text{(aq)}}} \rightarrow 3Br_{2\text{(aq)}} + 3H_2O_{\text{(l)}}$ is $x \ mol \ L^{-1} \ min^{-1}$. What is the rate (in $mol \ L^{-1} \ min^{-1}$) of this reaction?