(A) The rate of reaction is given by:$r = -\frac{d[N_2O_5]}{dt} = \frac{1}{2} \frac{d[NO_2]}{dt} = \frac{1}{1/2} \frac{d[O_2]}{dt}$Substituting the gi

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(A) The rate of reaction is given by:$r = -\frac{d[N_2O_5]}{dt} = \frac{1}{2} \frac{d[NO_2]}{dt} = \frac{1}{1/2} \frac{d[O_2]}{dt}$Substituting the given rate expressions:$K_1[N_2O_5] = \frac{1}{2} K_2[N_2O_5] = 2 K_3[N_2O_5]$Dividing by $[N_2O_5]$:$K_1 = \frac{K_2}{2} = 2K_3$Multiplying by $2$:$2K_1 = K_2 = 4K_3$

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

Difficult

For the reaction $N_2O_5 \rightarrow 2NO_2 + \frac{1}{2} O_2$,given that:
$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$,
$\frac{d[NO_2]}{dt} = K_2[N_2O_5]$,
$\frac{d[O_2]}{dt} = K_3[N_2O_5]$
What is the relationship between $K_1$,$K_2$,and $K_3$?

A
$2K_1 = K_2 = 4K_3$
B
$K_1 = K_2 = K_3$
C
$2K_1 = 4K_2 = K_3$
D
None of these

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

For a reaction $A \to B$,the rate of reaction quadrupled when the concentration of $A$ is doubled. The rate expression of the reaction is $r = K[A]^n$. The value of $n$ is

Easy

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Write the differential rate expression for the following reactions and determine their order of reaction:
$1) \ 2 \ HI \rightarrow H_2 + I_2$
$2) \ 2 \ NO_{(g)} + O_{2(g)} \rightarrow 2 \ NO_{2(g)}$

Medium

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Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$

$Expt. \ No.$ $[A]$ $[B]$ $Initial \ Rate$

$1$ $0.012$ $0.035$ $0.10$

$2$ $0.024$ $0.070$ $0.80$

$3$ $0.024$ $0.035$ $0.10$

$4$ $0.012$ $0.070$ $0.80$

$Expt. \ No.$	$[A]$	$[B]$	$Initial \ Rate$
$1$	$0.012$	$0.035$	$0.10$
$2$	$0.024$	$0.070$	$0.80$
$3$	$0.024$	$0.035$	$0.10$
$4$	$0.012$	$0.070$	$0.80$

DifficultAIIMS 2012

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The rate constant of a reaction is $1.388 \times 10^{-3} \ mol^{-2} \ L^{2} \ s^{-1}$. The order of the reaction is:

Medium

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The reaction rate between two substances $A$ and $B$ is expressed as: $\text{rate} = k[A]^n[B]^m$. If the concentration of $A$ is doubled and the concentration of $B$ is halved,the ratio of the new rate to the initial rate will be:

MediumAIEEE 2012

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For the reaction $N_2O_5 \rightarrow 2NO_2 + \frac{1}{2} O_2$,given that:$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$,$\frac{d[NO_2]}{dt} = K_2[N_2O_5]$,$\frac{d[O_2]}{dt} = K_3[N_2O_5]$What is the relationship between $K_1$,$K_2$,and $K_3$?

Similar Questions

For a reaction $A \to B$,the rate of reaction quadrupled when the concentration of $A$ is doubled. The rate expression of the reaction is $r = K[A]^n$. The value of $n$ is

Write the differential rate expression for the following reactions and determine their order of reaction:$1) \ 2 \ HI \rightarrow H_2 + I_2$$2) \ 2 \ NO_{(g)} + O_{2(g)} \rightarrow 2 \ NO_{2(g)}$

Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$ $Expt. \ No.$ $[A]$ $[B]$ $Initial \ Rate$ $1$ $0.012$ $0.035$ $0.10$ $2$ $0.024$ $0.070$ $0.80$ $3$ $0.024$ $0.035$ $0.10$ $4$ $0.012$ $0.070$ $0.80$

The rate constant of a reaction is $1.388 \times 10^{-3} \ mol^{-2} \ L^{2} \ s^{-1}$. The order of the reaction is:

The reaction rate between two substances $A$ and $B$ is expressed as: $\text{rate} = k[A]^n[B]^m$. If the concentration of $A$ is doubled and the concentration of $B$ is halved,the ratio of the new rate to the initial rate will be:

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For the reaction $N_2O_5 \rightarrow 2NO_2 + \frac{1}{2} O_2$,given that:
$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$,
$\frac{d[NO_2]}{dt} = K_2[N_2O_5]$,
$\frac{d[O_2]}{dt} = K_3[N_2O_5]$
What is the relationship between $K_1$,$K_2$,and $K_3$?

Write the differential rate expression for the following reactions and determine their order of reaction:
$1) \ 2 \ HI \rightarrow H_2 + I_2$
$2) \ 2 \ NO_{(g)} + O_{2(g)} \rightarrow 2 \ NO_{2(g)}$

Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$

$Expt. \ No.$ $[A]$ $[B]$ $Initial \ Rate$

$1$ $0.012$ $0.035$ $0.10$

$2$ $0.024$ $0.070$ $0.80$

$3$ $0.024$ $0.035$ $0.10$

$4$ $0.012$ $0.070$ $0.80$