(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

Difficult

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

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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 following homogeneous reaction scheme,the rate constant has units for the reaction $A + B \xrightarrow{K} C$:

Easy

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Write the general reaction and its rate law.

Medium

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The reaction $2X + Y \to X_2Y$ follows the mechanism given below:
$2X \rightleftharpoons X_2$ (Fast)
$X_2 + Y \to X_2Y$ (Slow)
Determine the order of the reaction.

Medium

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The reaction $A_2 + B_2 \rightarrow 2AB$ follows the mechanism $A_2 \underset{k_{-1}}{\stackrel{k_1}{\rightleftharpoons}} 2A$ (fast),$A + B_2 \xrightarrow{k_2} AB + B$ (slow),$A + B \rightarrow AB$ (fast). The overall order of the reaction is:

MediumJEE MAIN 2025

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The rate of the reaction $2A + 3B \rightarrow 2C + D$ is $6 \times 10^{-4} \text{ mol dm}^{-3} \text{ s}^{-1}$, when $[A] = [B] = 0.3 \text{ mol dm}^{-3}$. If the reaction is of first order with respect to $A$ and zeroth order with respect to $B$, find the rate constant $k$.

DifficultMHT CET 2026

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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:

Similar Questions

For the following homogeneous reaction scheme,the rate constant has units for the reaction $A + B \xrightarrow{K} C$:

Write the general reaction and its rate law.

The reaction $2X + Y \to X_2Y$ follows the mechanism given below:$2X \rightleftharpoons X_2$ (Fast)$X_2 + Y \to X_2Y$ (Slow)Determine the order of the reaction.

The reaction $A_2 + B_2 \rightarrow 2AB$ follows the mechanism $A_2 \underset{k_{-1}}{\stackrel{k_1}{\rightleftharpoons}} 2A$ (fast),$A + B_2 \xrightarrow{k_2} AB + B$ (slow),$A + B \rightarrow AB$ (fast). The overall order of the reaction is:

The rate of the reaction $2A + 3B \rightarrow 2C + D$ is $6 \times 10^{-4} \text{ mol dm}^{-3} \text{ s}^{-1}$, when $[A] = [B] = 0.3 \text{ mol dm}^{-3}$. If the reaction is of first order with respect to $A$ and zeroth order with respect to $B$, find the rate constant $k$.

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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:

The reaction $2X + Y \to X_2Y$ follows the mechanism given below:
$2X \rightleftharpoons X_2$ (Fast)
$X_2 + Y \to X_2Y$ (Slow)
Determine the order of the reaction.