Assuming the reaction 2NO_{(g)} + Cl_{2(g)} l | vedclass

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(D) For an elementary reaction,the rate law is determined directly from the stoichiometry of the balanced chemical equation.Since the reaction $2NO_{(

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the order of the reaction is equal to the molecularity

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(D) For an elementary reaction,the rate law is determined directly from the stoichiometry of the balanced chemical equation.Since the reaction $2NO_{(g)} + Cl_{2(g)} \longrightarrow 2NOCl_{(g)}$ is given as an elementary step,the rate law is $Rate = k[NO]^2[Cl_2]^1$.The order of the reaction is the sum of the powers of the concentration terms in the rate law,which is $2 + 1 = 3$.The molecularity of an elementary reaction is the number of reacting species taking part in the elementary step,which is $2 + 1 = 3$.Therefore,for any elementary reaction,the order of the reaction is equal to its molecularity.

Experiment	$[Cl_2] \ (M)$	$[NO] \ (M)$	Rate $(mol \ L^{-1} \sec^{-1})$
$I$	$0.05$	$0.05$	$1 \times 10^{-3}$
$II$	$0.15$	$0.05$	$3 \times 10^{-3}$
$III$	$0.05$	$0.15$	$9 \times 10^{-3}$

Rate $(mol \ L^{-1} \ s^{-1})$	$[A]$ $(mol \ L^{-1})$	$[B]$ $(mol \ L^{-1})$
$0.10$	$20$	$0.5$
$0.40$	$x$	$0.5$
$0.80$	$40$	$y$

Assuming the reaction $2NO_{(g)} + Cl_{2(g)} \longrightarrow 2NOCl_{(g)}$ occurs in a single elementary step,we can say that

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