(B) The rate-determining step $(RDS)$ is the slow step: $NOBr_2 + NO \rightarrow 2 \ NOBr$.The rate law is given by: $r = k [NOBr_2] [NO]$ ---- $(i)$F

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(B) The rate-determining step $(RDS)$ is the slow step: $NOBr_2 + NO \rightarrow 2 \ NOBr$.The rate law is given by: $r = k [NOBr_2] [NO]$ ---- $(i)$From the fast equilibrium step: $K_{eq} = \frac{[NOBr_2]}{[NO] [Br_2]}$,which implies $[NOBr_2] = K_{eq} [NO] [Br_2]$ ---- $(ii)$Substituting $(ii)$ into $(i)$:$r = k \cdot K_{eq} [NO] [Br_2] [NO]$$r = k' [NO]^2 [Br_2]^1$The overall order of the reaction is the sum of the powers of the concentration terms in the rate law: $2 + 1 = 3$.

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

Medium

The reaction $2 \ NO + Br_2 \rightarrow 2 \ NOBr$ takes place through the mechanism given below:
$NO + Br_2 \Leftrightarrow NOBr_2$ (fast)
$NOBr_2 + NO \rightarrow 2 \ NOBr$ (slow)
The overall order of the reaction is $.....$.

JEE MAIN 2023 All JEE MAIN

A
$4$
B
$3$
C
$5$
D
$6$

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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For the catalytic decomposition of $AB_3$, the half-life period is $4 \, \text{hours}$ at $50 \, \text{mm}$ and $2 \, \text{hours}$ at $100 \, \text{mm}$. What is the order of the reaction?

Medium

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$A$ chemical reaction takes place in two steps as follows:
$(i) \ NO_2Cl_{(g)} \xrightarrow{K_1} NO_{2(g)} + Cl_{(g)}$
$(ii) \ NO_2Cl_{(g)} + Cl_{(g)} \xrightarrow{K_2} NO_{2(g)} + Cl_{2(g)}$
Identify the reaction intermediate.

MediumMHT CET 2016

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Which of the following is an example of a second-order reaction?

MediumMHT CET 2026

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The mechanism of the reaction $A + 2B \to D$ is given by:
$2B \xrightarrow{k} B_2$ [Slow]
$B_2 + A \to D$ [Fast]
The rate law expression,order with respect to $A$,order with respect to $B$,and overall order are respectively:

Medium

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The rate constant for the reaction,$2N_2O_5 \to 4NO_2 + O_2$ is $3 \times 10^{-5} \, s^{-1}$. If the rate is $2.40 \times 10^{-5} \, mol \, L^{-1} \, s^{-1}$,then the concentration of $N_2O_5$ (in $mol \, L^{-1}$) is

MediumIIT 2000

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The reaction $2 \ NO + Br_2 \rightarrow 2 \ NOBr$ takes place through the mechanism given below:$NO + Br_2 \Leftrightarrow NOBr_2$ (fast)$NOBr_2 + NO \rightarrow 2 \ NOBr$ (slow)The overall order of the reaction is $.....$.

Similar Questions

For the catalytic decomposition of $AB_3$, the half-life period is $4 \, \text{hours}$ at $50 \, \text{mm}$ and $2 \, \text{hours}$ at $100 \, \text{mm}$. What is the order of the reaction?

$A$ chemical reaction takes place in two steps as follows:$(i) \ NO_2Cl_{(g)} \xrightarrow{K_1} NO_{2(g)} + Cl_{(g)}$$(ii) \ NO_2Cl_{(g)} + Cl_{(g)} \xrightarrow{K_2} NO_{2(g)} + Cl_{2(g)}$Identify the reaction intermediate.

Which of the following is an example of a second-order reaction?

The mechanism of the reaction $A + 2B \to D$ is given by:$2B \xrightarrow{k} B_2$ [Slow]$B_2 + A \to D$ [Fast]The rate law expression,order with respect to $A$,order with respect to $B$,and overall order are respectively:

The rate constant for the reaction,$2N_2O_5 \to 4NO_2 + O_2$ is $3 \times 10^{-5} \, s^{-1}$. If the rate is $2.40 \times 10^{-5} \, mol \, L^{-1} \, s^{-1}$,then the concentration of $N_2O_5$ (in $mol \, L^{-1}$) is

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The reaction $2 \ NO + Br_2 \rightarrow 2 \ NOBr$ takes place through the mechanism given below:
$NO + Br_2 \Leftrightarrow NOBr_2$ (fast)
$NOBr_2 + NO \rightarrow 2 \ NOBr$ (slow)
The overall order of the reaction is $.....$.

$A$ chemical reaction takes place in two steps as follows:
$(i) \ NO_2Cl_{(g)} \xrightarrow{K_1} NO_{2(g)} + Cl_{(g)}$
$(ii) \ NO_2Cl_{(g)} + Cl_{(g)} \xrightarrow{K_2} NO_{2(g)} + Cl_{2(g)}$
Identify the reaction intermediate.

The mechanism of the reaction $A + 2B \to D$ is given by:
$2B \xrightarrow{k} B_2$ [Slow]
$B_2 + A \to D$ [Fast]
The rate law expression,order with respect to $A$,order with respect to $B$,and overall order are respectively: