Nitric oxide reacts with $H_2$ according to the reaction,$2 NO_{(g)} + 2 H_{2(g)} \rightarrow N_{2(g)} + 2 H_2O_{(g)}$. Identify the correct relationship among the following.

For a given chemical reaction $\gamma_{1} A + \gamma_{2} B \rightarrow \gamma_{3} C + \gamma_{4} D$,the rate of appearance of $D$ is $1.5$ times the rate of disappearance of $B$,which is twice the rate of disappearance of $A$. The rate of appearance of $D$ has been experimentally determined to be $9 \, mmol \, dm^{-3} s^{-1}$. Therefore,the rate of reaction is $...... \, mmol \, dm^{-3} s^{-1}$. (Nearest Integer)

Explain why the average rate of reaction decreases with the concentration of the reactant using an example.

For the decomposition reaction $N_2O_{4(g)} \rightarrow 2NO_{2(g)}$,the initial pressure of $N_2O_4$ decreases from $0.46 \ atm$ to $0.28 \ atm$ in $30 \ minutes$. What is the rate of formation of $NO_2$?

For the reaction,$5Br^-{_{\text{(aq)}}} + BrO_3^-{_{\text{(aq)}}} + 6H^+{_{\text{(aq)}}} \rightarrow 3Br_{2\text{(aq)}} + 3H_2O_{\text{(l)}}$,if $-\frac{\Delta[Br^{-}]}{\Delta t} = 0.05 \ mol \ L^{-1} \ min^{-1}$,then the value of $-\frac{\Delta[BrO_3^{-}]}{\Delta t}$ in $mol \ L^{-1} \ min^{-1}$ is:

In the following reaction; $x A \longrightarrow y B$
$\log_{10} \left[ -\frac{d[A]}{dt} \right] = \log_{10} \left[ \frac{d[B]}{dt} \right] + 0.3010$
$'A'$ and $'B'$ respectively can be