For a reaction $A + B \longrightarrow P$,the following data are provided. The rate constant for this reaction in standard units is:

Entry	$[A]$ in $M$	$[B]$ in $M$	Initial rate $(M/s)$
$1$	$0.02$	$0.02$	$2 \times 10^{-2}$
$2$	$0.02$	$0.04$	$4 \times 10^{-2}$
$3$	$0.04$	$0.04$	$8 \times 10^{-2}$

$A$ reaction $2NO + 2H_2 \longrightarrow N_2 + 2H_2O$ has the following mechanism:
Step-$I$: $2NO \longrightarrow N_2O_2$
Step-$II$: $N_2O_2 + H_2 \longrightarrow N_2O + H_2O$
Step-$III$: $N_2O + H_2 \longrightarrow N_2 + H_2O$
Which of the following substances is a reaction intermediate?

Consider the following reactions:
$A$ $\rightarrow P_1; B$ $\rightarrow P_2; C$ $\rightarrow P_3; D$ $\rightarrow P_4$
The orders of the above reactions are $a, b, c,$ and $d,$ respectively. The following graph is obtained when $\log[\text{rate}]$ vs. $\log[\text{conc.}]$ are plotted:
Among the following,the correct sequence for the order of the reactions is:

Consider the plots for the types of reaction $nA \to B + C$. These plots respectively correspond to the reaction orders:

From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant.
$H_2 O_2+3 I^{-}+2 H^{+} \rightarrow 2 H_2 O+I_3^{-} \text { Rate }=k\left[H_2 O_2\right]\left[I^{-}\right]$

For a gaseous reaction,the rate is given by $Rate = k [A] [B]$. If the volume of the container is reduced to $1/4$ of its initial volume,the rate of the reaction will become how many times the initial rate?