Rate of the reaction $A + B \rightarrow \text{product}$ is $3.6 \times 10^{-2} \ mol \ dm^{-3} \ s^{-1}$ and rate law is $r = k[A][B]^2$. What is the rate constant of the reaction if $[A] = 0.2 \ M$ and $[B] = 0.1 \ M$?

For the decomposition reaction $2NH_3(g) \rightarrow N_2(g) + 3H_2(g)$,if the rate constant $k = 2.6 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$,calculate the rate of formation of $N_2$ and $H_2$.

For a reaction involving substances $x$,$y$,and $z$,if the overall order of the reaction is $0.5$,which of the following rate laws is applicable?

$A_2 + B_2 \to 2AB$; $R.O.R = k[A_2]^a[B_2]^b$

Initial $[A_2]$	Initial $[B_2]$	$R.O.R. (r) \ M s^{-1}$
$0.2$	$0.2$	$0.04$
$0.1$	$0.4$	$0.04$
$0.2$	$0.4$	$0.08$

Order of reaction with respect to $A_2$ and $B_2$ are respectively:

For the following graphs,choose the correct option regarding the order of reaction:

For the reaction $Cl_{2(aq)} + H_2S_{(aq)} \to S_{(s)} + 2H^{+}_{(aq)} + 2Cl^{-}_{(aq)}$,the rate law is $r = K[Cl_2][H_2S]$. Which of the following mechanisms is/are consistent with this rate law?
$A. \ H_2S \rightleftharpoons H^{+} + HS^{-}$ (fast)
$Cl_2 + HS^{-} \to 2Cl^{-} + H^{+} + S$ (slow)
$B. \ Cl_2 + H_2S \to H^{+} + Cl^{-} + Cl^{+} + HS^{-}$ (slow)
$Cl^{+} + HS^{-} \to H^{+} + Cl^{-} + S$ (fast)