Identify the order of reaction if its rate constant is $x \ sec^{-1}$.

Match List-$I$ with List-$II$:

List-$I$ (Order of Reaction)	List-$II$ (Unit of rate constant)
$A$. Zero order	$I$. $mol^{-1} L s^{-1}$
$B$. First order	$II$. $mol^{-2} L^{2} s^{-1}$
$C$. Second order	$III$. $s^{-1}$
$D$. Third order	$IV$. $mol L^{-1} s^{-1}$

For the reaction $2A + B \rightarrow C + D$,select the correct rate law based on the following data:
$1$. $[A] = 0.1, [B] = 0.1, \text{Initial Rate} = 7.5 \times 10^{-3}$
$2$. $[A] = 0.3, [B] = 0.2, \text{Initial Rate} = 9.0 \times 10^{-2}$
$3$. $[A] = 0.3, [B] = 0.4, \text{Initial Rate} = 3.6 \times 10^{-1}$
$4$. $[A] = 0.4, [B] = 0.1, \text{Initial Rate} = 3.0 \times 10^{-2}$

The following are the rate constants of two different reactions. What is the overall order of each reaction?
$(a)$ $2.1 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$
$(b)$ $4.5 \times 10^{-3} \ min^{-1}$

Identify the reaction intermediate of the following reaction sequence:
$(i)$ $2 SO_{2(g)} + 2 NO_{2(g)} \rightarrow 2 SO_{3(g)} + 2 NO_{(g)}$
$(ii)$ $2 NO_{(g)} + O_{2(g)} \rightarrow 2 NO_{2(g)}$
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Overall: $2 SO_{2(g)} + O_{2(g)} \rightarrow 2 SO_{3(g)}$

The reaction $2N_2O_5 \rightleftharpoons 4NO_2 + O_2$ follows first order kinetics. Hence,the molecularity of the reaction is