(B) The rate of the reaction is determined by the slow step: $r = k_2[O][O_3]$.From the fast equilibrium step: $K_{eq} = \frac{[O_2][O]}{[O_3]}$,which

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(B) The rate of the reaction is determined by the slow step: $r = k_2[O][O_3]$.From the fast equilibrium step: $K_{eq} = \frac{[O_2][O]}{[O_3]}$,which gives $[O] = K_{eq} \frac{[O_3]}{[O_2]}$.Substituting the value of $[O]$ into the rate expression: $r = k_2 \times K_{eq} \frac{[O_3]}{[O_2]} \times [O_3]$.Since $k_2 \times K_{eq}$ is a constant $K$,the rate law is $r = K \frac{[O_3]^2}{[O_2]}$ or $r = K[O_3]^2[O_2]^{-1}$.

Class 12 Chemistry Chemical Kinetics Rate law , Rate constant , Order of Reaction and Molecularity

Medium

For the chemical reaction $2O_3 \rightarrow 3O_2$,the mechanism is given below. What will be the rate law expression?
$O_3 \rightleftharpoons O_2 + O$ ...... (fast)
$O + O_3 \rightarrow 2O_2$ ...... (slow)

A
$r = K[O_3]^2$
B
$r = K[O_3]^2 [O_2]^{-1}$
C
$r = K[O_3][O_2]$
D
Cannot be determined

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Class 12

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant.
$(i)$ $3 NO_{(g)} \rightarrow N_2O_{(g)}$ Rate $= k[NO]^2$

Medium

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The reaction $N_2O_5$ (in $CCl_4$ solution) $\to 2NO_2$ (solution) $+ \frac{1}{2}O_{2(g)}$ is of first order in $N_2O_5$ with rate constant $6.2 \times 10^{-1} \, s^{-1}$. What is the value of the rate of reaction when $[N_2O_5] = 1.25 \, mol \, L^{-1}$?

Easy

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What is the order of reaction $A + B \to C$?

Observation $[A] \ (mol \ L^{-1})$ $[B] \ (mol \ L^{-1})$ Rate $(mol \ L^{-1} \ sec^{-1})$

$1$ $0.1$ $0.1$ $2 \times 10^{-3}$

$2$ $0.4$ $0.1$ $3.2 \times 10^{-3}$

$3$ $0.1$ $0.2$ $8 \times 10^{-3}$

Observation	$[A] \ (mol \ L^{-1})$	$[B] \ (mol \ L^{-1})$	Rate $(mol \ L^{-1} \ sec^{-1})$
$1$	$0.1$	$0.1$	$2 \times 10^{-3}$
$2$	$0.4$	$0.1$	$3.2 \times 10^{-3}$
$3$	$0.1$	$0.2$	$8 \times 10^{-3}$

Difficult

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The following are the rate constants of two different reactions. What is the overall order of reaction for each?
$(a)$ $2.418 \times 10^{-5} \ hr^{-1}$
$(b)$ $7.1 \times 10^{-4} \ atm \ s^{-1}$

Medium

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Why can’t molecularity of any reaction be equal to zero?

Easy

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For the chemical reaction $2O_3 \rightarrow 3O_2$,the mechanism is given below. What will be the rate law expression?$O_3 \rightleftharpoons O_2 + O$ ...... (fast)$O + O_3 \rightarrow 2O_2$ ...... (slow)

Similar Questions

From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant.$(i)$ $3 NO_{(g)} \rightarrow N_2O_{(g)}$ Rate $= k[NO]^2$

The reaction $N_2O_5$ (in $CCl_4$ solution) $\to 2NO_2$ (solution) $+ \frac{1}{2}O_{2(g)}$ is of first order in $N_2O_5$ with rate constant $6.2 \times 10^{-1} \, s^{-1}$. What is the value of the rate of reaction when $[N_2O_5] = 1.25 \, mol \, L^{-1}$?

What is the order of reaction $A + B \to C$? Observation $[A] \ (mol \ L^{-1})$ $[B] \ (mol \ L^{-1})$ Rate $(mol \ L^{-1} \ sec^{-1})$ $1$ $0.1$ $0.1$ $2 \times 10^{-3}$ $2$ $0.4$ $0.1$ $3.2 \times 10^{-3}$ $3$ $0.1$ $0.2$ $8 \times 10^{-3}$

The following are the rate constants of two different reactions. What is the overall order of reaction for each?$(a)$ $2.418 \times 10^{-5} \ hr^{-1}$$(b)$ $7.1 \times 10^{-4} \ atm \ s^{-1}$

Why can’t molecularity of any reaction be equal to zero?

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For the chemical reaction $2O_3 \rightarrow 3O_2$,the mechanism is given below. What will be the rate law expression?
$O_3 \rightleftharpoons O_2 + O$ ...... (fast)
$O + O_3 \rightarrow 2O_2$ ...... (slow)

From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant.
$(i)$ $3 NO_{(g)} \rightarrow N_2O_{(g)}$ Rate $= k[NO]^2$

What is the order of reaction $A + B \to C$?

Observation $[A] \ (mol \ L^{-1})$ $[B] \ (mol \ L^{-1})$ Rate $(mol \ L^{-1} \ sec^{-1})$

$1$ $0.1$ $0.1$ $2 \times 10^{-3}$

$2$ $0.4$ $0.1$ $3.2 \times 10^{-3}$

$3$ $0.1$ $0.2$ $8 \times 10^{-3}$

The following are the rate constants of two different reactions. What is the overall order of reaction for each?
$(a)$ $2.418 \times 10^{-5} \ hr^{-1}$
$(b)$ $7.1 \times 10^{-4} \ atm \ s^{-1}$