(B) The rate of reaction is defined as:$-\frac{1}{2} \frac{d[N_2O_5]}{dt} = \frac{1}{4} \frac{d[NO_2]}{dt} = \frac{d[O_2]}{dt}$Substituting the given

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(B) The rate of reaction is defined as:$-\frac{1}{2} \frac{d[N_2O_5]}{dt} = \frac{1}{4} \frac{d[NO_2]}{dt} = \frac{d[O_2]}{dt}$Substituting the given rate expressions:$\frac{1}{2} k[N_2O_5] = \frac{1}{4} k'[N_2O_5] = k''[N_2O_5]$Dividing by $[N_2O_5]$:$\frac{k}{2} = \frac{k'}{4} = k''$From $\frac{k}{2} = \frac{k'}{4}$,we get $k' = 2k$.From $\frac{k}{2} = k''$,we get $k'' = \frac{k}{2}$.

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

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The rate of the reaction: $2N_2O_5 \rightarrow 4NO_2 + O_2$ can be written in three ways.
$-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$
$\frac{d[NO_2]}{dt} = k'[N_2O_5]$ ; $\frac{d[O_2]}{dt} = k''[N_2O_5]$
The relationship between $k$ and $k'$ and between $k$ and $k''$ are:

AIPMT 2011 All AIPMT

A
$k' = 2k$ ; $k'' = k$
B
$k' = 2k$ ; $k'' = k/2$
C
$k' = 2k$ ; $k'' = 2k$
D
$k' = k$ ; $k'' = k$

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Class 12

Chemistry Questions

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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AIPMT 2011 Paper All AIPMT years →

For the decomposition of a compound $AB$ at $600 \ K$,the following data were obtained:
$[AB] \ (mol \ dm^{-3})$ Rate of decomposition of $AB \ (mol \ dm^{-3} \ s^{-1})$
$0.20$ $2.75 \times 10^{-8}$
$0.40$ $11.0 \times 10^{-8}$
$0.60$ $24.75 \times 10^{-8}$

The order for the decomposition of $AB$ is:

DifficultKCET 2009

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What is the order of the following reaction: $2 H_2 O_{2(g)} \longrightarrow 2 H_2 O_{(l)} + O_{2(g)}$?

EasyMHT CET 2024

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In the hydrolysis of an organic chloride in the presence of a large excess of water,the reaction is $RCl + H_2O \longrightarrow ROH + HCl$. Determine the molecularity and order of the reaction.

Medium

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For a reaction whose rate expression is: Rate $= k[A]^{1/2}[B]^{3/2}$,the order would be

Medium

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The reaction between $A$ and $B$ is first order with respect to $A$ and zero order with respect to $B$. Fill in the blanks in the following table:

Experiment $[A] / mol \, L^{-1}$ $[B] / mol \, L^{-1}$ Initial rate / $mol \, L^{-1} \, min^{-1}$

$I$ $0.1$ $0.1$ $2.0 \times 10^{-2}$

$II$ $-$ $0.2$ $4.0 \times 10^{-2}$

$III$ $0.4$ $0.4$ $-$

$IV$ $-$ $0.2$ $2.0 \times 10^{-2}$

Experiment	$[A] / mol \, L^{-1}$	$[B] / mol \, L^{-1}$	Initial rate / $mol \, L^{-1} \, min^{-1}$
$I$	$0.1$	$0.1$	$2.0 \times 10^{-2}$
$II$	$-$	$0.2$	$4.0 \times 10^{-2}$
$III$	$0.4$	$0.4$	$-$
$IV$	$-$	$0.2$	$2.0 \times 10^{-2}$

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$[AB] \ (mol \ dm^{-3})$	Rate of decomposition of $AB \ (mol \ dm^{-3} \ s^{-1})$
$0.20$	$2.75 \times 10^{-8}$
$0.40$	$11.0 \times 10^{-8}$
$0.60$	$24.75 \times 10^{-8}$

The rate of the reaction: $2N_2O_5 \rightarrow 4NO_2 + O_2$ can be written in three ways.$-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$$\frac{d[NO_2]}{dt} = k'[N_2O_5]$ ; $\frac{d[O_2]}{dt} = k''[N_2O_5]$The relationship between $k$ and $k'$ and between $k$ and $k''$ are:

Similar Questions

For the decomposition of a compound $AB$ at $600 \ K$,the following data were obtained: $[AB] \ (mol \ dm^{-3})$Rate of decomposition of $AB \ (mol \ dm^{-3} \ s^{-1})$$0.20$$2.75 \times 10^{-8}$$0.40$$11.0 \times 10^{-8}$$0.60$$24.75 \times 10^{-8}$ The order for the decomposition of $AB$ is:

What is the order of the following reaction: $2 H_2 O_{2(g)} \longrightarrow 2 H_2 O_{(l)} + O_{2(g)}$?

In the hydrolysis of an organic chloride in the presence of a large excess of water,the reaction is $RCl + H_2O \longrightarrow ROH + HCl$. Determine the molecularity and order of the reaction.

For a reaction whose rate expression is: Rate $= k[A]^{1/2}[B]^{3/2}$,the order would be

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The rate of the reaction: $2N_2O_5 \rightarrow 4NO_2 + O_2$ can be written in three ways.
$-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$
$\frac{d[NO_2]}{dt} = k'[N_2O_5]$ ; $\frac{d[O_2]}{dt} = k''[N_2O_5]$
The relationship between $k$ and $k'$ and between $k$ and $k''$ are: