For the reaction:2NO_{2(g)} + O_{3(g)} to N_2 | vedclass

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Question

(A) For a reaction mechanism to be consistent with the rate law,the rate-determining step (the slowest step) must involve the reactants in the same st

Vedclass · Accepted Answer

$I$ only

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(A) For a reaction mechanism to be consistent with the rate law,the rate-determining step (the slowest step) must involve the reactants in the same stoichiometric ratio as the rate law.In Mechanism $I$,the slow step is $NO_{2(g)} + O_{3(g)} 	o NO_{3(g)} + O_{2(g)}$. The rate of this step is $R = K[NO_2][O_3]$,which matches the given rate law.In Mechanism $II$,the slow step is $NO_{2(g)} + [O] 	o NO_3$. From the fast equilibrium $O_{3(g)} ightleftharpoons O_{2(g)} + [O]$,we have $K_{eq} = \frac{[O_2][O]}{[O_3]}$,so $[O] = K_{eq} \frac{[O_3]}{[O_2]}$. Substituting this into the rate expression for the slow step,$R = K'[NO_2][O] = K'[NO_2] 	imes K_{eq} \frac{[O_3]}{[O_2]} = K'' \frac{[NO_2][O_3]}{[O_2]}$. This does not match the given rate law.Therefore,only Mechanism $I$ is consistent.

$Exp. \ No.$	$[A]$	$[B]$	$Rate$
$1.$	$1.0$	$0.15$	$4.2 \times 10^{-6}$
$2.$	$2.0$	$0.15$	$8.4 \times 10^{-6}$
$3.$	$1.0$	$0.20$	$5.6 \times 10^{-6}$

$Expt. \ No.$	$[A]$	$[B]$	$Initial \ Rate$
$1$	$0.012$	$0.035$	$0.10$
$2$	$0.024$	$0.070$	$0.80$
$3$	$0.024$	$0.035$	$0.10$
$4$	$0.012$	$0.070$	$0.80$

Similar Questions

$A$ study of chemical kinetics of the reaction $A + B \to$ Products,gave the following data at $25 \ ^oC$.

$Exp. \ No.$ $[A]$ $[B]$ $Rate$

$1.$ $1.0$ $0.15$ $4.2 \times 10^{-6}$

$2.$ $2.0$ $0.15$ $8.4 \times 10^{-6}$

$3.$ $1.0$ $0.20$ $5.6 \times 10^{-6}$

Find out the rate law.

Mechanism of a hypothetical reaction $X_2 + Y_2 \rightarrow 2XY$ is given below:
$(i)$ $X_2 \rightarrow X + X$ (fast)
$(ii)$ $X + Y_2 \rightleftharpoons XY + Y$ (slow)
$(iii)$ $X + Y \rightarrow XY$ (fast)
The overall order of the reaction will be

Which of the following statements is $NOT$ true for a reaction having rate law $r=k[H_2][I_2]$?

For a given reaction $t_{1/2} = \frac{1}{k \cdot a}$,the order of reaction will be:

Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$

$Expt. \ No.$ $[A]$ $[B]$ $Initial \ Rate$

$1$ $0.012$ $0.035$ $0.10$

$2$ $0.024$ $0.070$ $0.80$

$3$ $0.024$ $0.035$ $0.10$

$4$ $0.012$ $0.070$ $0.80$

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