(B) The rate law is given by: $\text{Rate} = k[A_2]^x[B_2]^y$.From experiment $1$ and $2$,keeping $[A_2]$ constant:$\frac{3.2 \times 10^{-4}}{1.6 \tim

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(B) The rate law is given by: $\text{Rate} = k[A_2]^x[B_2]^y$.From experiment $1$ and $2$,keeping $[A_2]$ constant:$\frac{3.2 \times 10^{-4}}{1.6 \times 10^{-4}} = \left(\frac{0.2}{0.1}\right)^y \implies 2 = 2^y \implies y = 1$.From experiment $1$ and $3$,keeping $[B_2]$ constant:$\frac{3.2 \times 10^{-4}}{1.6 \times 10^{-4}} = \left(\frac{0.2}{0.1}\right)^x \implies 2 = 2^x \implies x = 1$.The overall order of the reaction is $x + y = 1 + 1 = 2$.

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

Medium

For the reaction $A_2 + B_2 \to 2AB$,the experimental data is given below. Determine the order of the reaction.

Experiment No. $[A_2] \text{ (M)}$ $[B_2] \text{ (M)}$ Rate $(M \cdot s^{-1})$

$1$ $0.1$ $0.1$ $1.6 \times 10^{-4}$

$2$ $0.1$ $0.2$ $3.2 \times 10^{-4}$

$3$ $0.2$ $0.1$ $3.2 \times 10^{-4}$

A
$1$
B
$2$
C
$0$
D
$3$

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Class 12 Questions

Class 12

Chemistry Questions

Chapter

Chemical Kinetics

Subtopic

Rate law , Rate constant , Order of Reaction and Molecularity

With the help of an example,explain what is meant by a pseudo first order reaction.

Medium

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Reaction: $KClO_3 + 6FeSO_4 + 3H_2SO_4 \to KCl + 3Fe_2(SO_4)_3 + 3H_2O$
Which is True $(T)$ and False $(F)$ in the following statement?
The order of this reaction is $1$.

Easy

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For the reaction $2A + B \to C$,the values of initial rate at different reactant concentrations are given in the table below: The rate law for the reaction is

$[A] \ (mol \ L^{-1})$ $[B] \ (mol \ L^{-1})$ Initial Rate $(mol \ L^{-1} \ s^{-1})$

$0.05$ $0.05$ $0.045$

$0.10$ $0.05$ $0.090$

$0.20$ $0.10$ $0.72$

DifficultJEE MAIN 2019

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If doubling the concentration of a reactant $A$ increases the rate $4$ times and tripling the concentration of $A$ increases the rate $9$ times,the rate is proportional to

MediumAIIMS 1991

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The rate law for the reaction below is given by the expression $Rate = k[A][B]$.
$A + B \to \text{Product}$
If the concentration of $B$ is increased from $0.1 \ M$ to $0.3 \ M$,keeping the concentration of $A$ constant at $0.1 \ M$,the rate constant $(k)$ will be:

DifficultJEE MAIN 2016

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Experiment No.	$[A_2] \text{ (M)}$	$[B_2] \text{ (M)}$	Rate $(M \cdot s^{-1})$
$1$	$0.1$	$0.1$	$1.6 \times 10^{-4}$
$2$	$0.1$	$0.2$	$3.2 \times 10^{-4}$
$3$	$0.2$	$0.1$	$3.2 \times 10^{-4}$

$[A] \ (mol \ L^{-1})$	$[B] \ (mol \ L^{-1})$	Initial Rate $(mol \ L^{-1} \ s^{-1})$
$0.05$	$0.05$	$0.045$
$0.10$	$0.05$	$0.090$
$0.20$	$0.10$	$0.72$

Similar Questions

With the help of an example,explain what is meant by a pseudo first order reaction.

Reaction: $KClO_3 + 6FeSO_4 + 3H_2SO_4 \to KCl + 3Fe_2(SO_4)_3 + 3H_2O$Which is True $(T)$ and False $(F)$ in the following statement?The order of this reaction is $1$.

If doubling the concentration of a reactant $A$ increases the rate $4$ times and tripling the concentration of $A$ increases the rate $9$ times,the rate is proportional to

The rate law for the reaction below is given by the expression $Rate = k[A][B]$.$A + B \to \text{Product}$If the concentration of $B$ is increased from $0.1 \ M$ to $0.3 \ M$,keeping the concentration of $A$ constant at $0.1 \ M$,the rate constant $(k)$ will be:

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Reaction: $KClO_3 + 6FeSO_4 + 3H_2SO_4 \to KCl + 3Fe_2(SO_4)_3 + 3H_2O$
Which is True $(T)$ and False $(F)$ in the following statement?
The order of this reaction is $1$.

The rate law for the reaction below is given by the expression $Rate = k[A][B]$.
$A + B \to \text{Product}$
If the concentration of $B$ is increased from $0.1 \ M$ to $0.3 \ M$,keeping the concentration of $A$ constant at $0.1 \ M$,the rate constant $(k)$ will be: