(D) The rate of the reaction is determined by the slow step $(II)$:$r = k_2 [N_2O_2] [H_2]$Since $N_2O_2$ is an intermediate,we express its concentrat

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(D) The rate of the reaction is determined by the slow step $(II)$:$r = k_2 [N_2O_2] [H_2]$Since $N_2O_2$ is an intermediate,we express its concentration using the equilibrium constant $(K_{eq})$ from the fast step $(I)$:$K_{eq} = \frac{[N_2O_2]}{[NO]^2} \implies [N_2O_2] = K_{eq} [NO]^2$Substituting this into the rate expression:$r = k_2 (K_{eq} [NO]^2) [H_2]$Let $k = k_2 K_{eq}$,then the rate law is:$r = k [NO]^2 [H_2]$

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

Medium

For the reaction $2H_2 + 2NO \to N_2 + 2H_2O$,the following mechanism has been proposed:
$I$. $2NO \rightleftharpoons N_2O_2$ (fast)
$II$. $N_2O_2 + H_2 \xrightarrow{k_2} N_2O + H_2O$ (slow)
$III$. $N_2O + H_2 \to N_2 + H_2O$ (fast)
What will be the rate law of this reaction?

A
$k[NO][H_2]^2$
B
$k[NO][H_2]$
C
$k[NO]^0[H_2]^3$
D
$k[NO]^2[H_2]$

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

The rate of reaction between two reactants $A$ and $B$ decreases by a factor of $4$ if the concentration of reactant $B$ is doubled. The order of this reaction with respect to reactant $B$ is

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DifficultJEE MAIN 2015

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What is the order of reaction for the decomposition of gaseous acetaldehyde?

EasyMHT CET 2020

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The reaction $2NO_{(g)} + O_{2(g)} \rightleftharpoons 2NO_{2(g)}$ is of first order. If the volume of the reaction vessel is reduced to $1/3$ of its original volume,the rate of reaction would be .......... times.

Easy

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For a chemical reaction,$m A \rightarrow x B$,the rate law is $r = k[A]^{2}$. If the concentration of $A$ is doubled,the reaction rate will be,

MediumKCET 2016

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For the reaction $2H_2 + 2NO \to N_2 + 2H_2O$,the following mechanism has been proposed:$I$. $2NO \rightleftharpoons N_2O_2$ (fast)$II$. $N_2O_2 + H_2 \xrightarrow{k_2} N_2O + H_2O$ (slow)$III$. $N_2O + H_2 \to N_2 + H_2O$ (fast)What will be the rate law of this reaction?

Similar Questions

The rate of reaction between two reactants $A$ and $B$ decreases by a factor of $4$ if the concentration of reactant $B$ is doubled. The order of this reaction with respect to reactant $B$ is

For the reaction $A + 2B \to C$,the rate equation is given as $\text{Rate} = K[A][B]$. If the concentration of $A$ is kept constant but that of $B$ is doubled,what will happen to the rate of the reaction?

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The reaction $2NO_{(g)} + O_{2(g)} \rightleftharpoons 2NO_{2(g)}$ is of first order. If the volume of the reaction vessel is reduced to $1/3$ of its original volume,the rate of reaction would be .......... times.

For a chemical reaction,$m A \rightarrow x B$,the rate law is $r = k[A]^{2}$. If the concentration of $A$ is doubled,the reaction rate will be,

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For the reaction $2H_2 + 2NO \to N_2 + 2H_2O$,the following mechanism has been proposed:
$I$. $2NO \rightleftharpoons N_2O_2$ (fast)
$II$. $N_2O_2 + H_2 \xrightarrow{k_2} N_2O + H_2O$ (slow)
$III$. $N_2O + H_2 \to N_2 + H_2O$ (fast)
What will be the rate law of this reaction?