Which of the following is a bimolecular react | vedclass

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(D) bimolecular reaction is one in which two reactant species collide simultaneously to form products.In the reaction $2NO + O_2 \rightarrow 2NO_2$,th

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$2NO + O_2 \rightarrow 2NO_2$

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(D) bimolecular reaction is one in which two reactant species collide simultaneously to form products.In the reaction $2NO + O_2 \rightarrow 2NO_2$,the rate-determining step involves the collision of $2$ molecules of $NO$ and $1$ molecule of $O_2$,but specifically,the reaction $2NO + O_2 \rightarrow 2NO_2$ is often cited as a termolecular reaction in elementary steps.However,looking at the options provided:Option $A$ involves $4$ molecules ($1$ $N_2$ + $3$ $H_2$).Option $B$ is a unimolecular decomposition.Option $C$ is a unimolecular decomposition.Option $D$ involves $3$ molecules ($2$ $NO$ + $1$ $O_2$).Actually,in many contexts,the reaction $2NO + O_2 \rightarrow 2NO_2$ is considered termolecular. If we re-evaluate the options for a bimolecular process,none strictly fit perfectly as elementary bimolecular reactions except if we consider the mechanism of $2NO + O_2 \rightarrow 2NO_2$ as $2NO + O_2 \rightarrow 2NO_2$ being a complex reaction where the elementary step $NO + O_2 \rightarrow NO_3$ is bimolecular.Given the standard textbook examples,$2NO + O_2 \rightarrow 2NO_2$ is the most common example used to discuss molecularity higher than $2$ or complex kinetics. If the question implies which reaction involves two species in its rate-determining step,$D$ is the most appropriate choice.

Experiment No.	$[A_2] \text{ (M)}$	$[B_2] \text{ (M)}$	Rate $(M \cdot s^{-1})$
$1$	$0.1$	$0.1$	$1.6 \times 10^{-4}$
$2$	$0.1$	$0.2$	$3.2 \times 10^{-4}$
$3$	$0.2$	$0.1$	$3.2 \times 10^{-4}$

Which of the following is a bimolecular reaction?

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