(B) The rate law for the reaction is given by: $\text{Rate} = k[A]^1[B]^2$.Given: $\text{Rate} = 4 \times 10^{-2} \text{ mol dm}^{-3} \text{ s}^{-1}$,

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

$20 \text{ mol}^{-2} \text{ dm}^6 \text{ s}^{-1}$

(B) The rate law for the reaction is given by: $\text{Rate} = k[A]^1[B]^2$.Given: $\text{Rate} = 4 \times 10^{-2} \text{ mol dm}^{-3} \text{ s}^{-1}$, $[A] = 0.2 \text{ mol dm}^{-3}$, $[B] = 0.1 \text{ mol dm}^{-3}$.Substituting the values into the rate law: $4 \times 10^{-2} = k(0.2)^1(0.1)^2$.$4 \times 10^{-2} = k(0.2)(0.01)$.$4 \times 10^{-2} = k(0.002)$.$k = \frac{4 \times 10^{-2}}{2 \times 10^{-3}} = 2 \times 10^1 = 20 \text{ mol}^{-2} \text{ dm}^6 \text{ s}^{-1}$.

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

Difficult

The rate of reaction $A + B \rightarrow P$ is $4 \times 10^{-2} \text{ mol dm}^{-3} \text{ s}^{-1}$. When $[A] = 0.2 \text{ mol dm}^{-3}$ and $[B] = 0.1 \text{ mol dm}^{-3}$, what is the rate constant of the reaction, if it is first order with respect to $A$ and second order with respect to $B$?

MHT CET 2026 All MHT CET

A
$10 \text{ mol}^{-2} \text{ dm}^6 \text{ s}^{-1}$
B
$20 \text{ mol}^{-2} \text{ dm}^6 \text{ s}^{-1}$
C
$25 \text{ mol}^{-2} \text{ dm}^6 \text{ s}^{-1}$
D
$40 \text{ mol}^{-2} \text{ dm}^6 \text{ s}^{-1}$

Explore More

Browse All

Question Bank

All Subjects

Class 12 Questions

Class 12

Chemistry Questions

Chapter

Chemical Kinetics

Subtopic

Rate law , Rate constant , Order of Reaction and Molecularity

Previous Year

MHT CET 2026 Paper All MHT CET years →

The following are the rate constants of two different reactions. What is the overall order of reaction for each?
$(a)$ $2.418 \times 10^{-5} \ hr^{-1}$
$(b)$ $7.1 \times 10^{-4} \ atm \ s^{-1}$

Medium

View Solution

Assertion : The kinetics of the reaction $mA + nB + pC \to m'X + n'Y + p'Z$ obey the rate expression as $\frac{dX}{dt} = k[A]^m[B]^n$.
Reason : The rate of the reaction does not depend upon the concentration of $C$.

DifficultAIIMS 2011

View Solution

The reaction between $X$ and $Y$ is first order with respect to $X$ and zero order with respect to $Y$.

$Experiment$ $[X] / (mol \ L^{-1})$ $[Y] / (mol \ L^{-1})$ $\text{Initial rate} / (mol \ L^{-1} \ min^{-1})$

$I$ $0.1$ $0.1$ $2 \times 10^{-3}$

$II$ $0.2$ $0.2$ $4 \times 10^{-3}$

$III$ $0.4$ $0.4$ $M \times 10^{-3}$

$IV$ $0.1$ $0.2$ $2 \times 10^{-3}$

Examine the data of the table and calculate the ratio of the numerical value of $M$ to $0.2$.

MediumJEE MAIN 2022

View Solution

The hydrolysis of ethyl acetate is a reaction of $.........$ order.
$CH_3COOEt + H_2O \xrightarrow{H^{+}} CH_3COOH + EtOH$

Medium

View Solution

$A$ reaction is first order in $A$ and second order in $B$.
$(i)$ Write the differential rate equation.
$(ii)$ How is the rate affected on increasing the concentration of $B$ three times?
$(iii)$ How is the rate affected when the concentrations of both $A$ and $B$ are doubled?

Difficult

View Solution

Vedclass Products

For Students

Vedclass Test Series

Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.

Start Free Trial

For Teachers

Exam Paper Generator

Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.

Try Free

For Institutes

Online Exam Module

Live online exams with unlimited students, 360° analytics & white-label branding.

See Demo

$Experiment$	$[X] / (mol \ L^{-1})$	$[Y] / (mol \ L^{-1})$	$\text{Initial rate} / (mol \ L^{-1} \ min^{-1})$
$I$	$0.1$	$0.1$	$2 \times 10^{-3}$
$II$	$0.2$	$0.2$	$4 \times 10^{-3}$
$III$	$0.4$	$0.4$	$M \times 10^{-3}$
$IV$	$0.1$	$0.2$	$2 \times 10^{-3}$

The rate of reaction $A + B \rightarrow P$ is $4 \times 10^{-2} \text{ mol dm}^{-3} \text{ s}^{-1}$. When $[A] = 0.2 \text{ mol dm}^{-3}$ and $[B] = 0.1 \text{ mol dm}^{-3}$, what is the rate constant of the reaction, if it is first order with respect to $A$ and second order with respect to $B$?

Similar Questions

The following are the rate constants of two different reactions. What is the overall order of reaction for each?$(a)$ $2.418 \times 10^{-5} \ hr^{-1}$$(b)$ $7.1 \times 10^{-4} \ atm \ s^{-1}$

Assertion : The kinetics of the reaction $mA + nB + pC \to m'X + n'Y + p'Z$ obey the rate expression as $\frac{dX}{dt} = k[A]^m[B]^n$.Reason : The rate of the reaction does not depend upon the concentration of $C$.

The hydrolysis of ethyl acetate is a reaction of $.........$ order.$CH_3COOEt + H_2O \xrightarrow{H^{+}} CH_3COOH + EtOH$

$A$ reaction is first order in $A$ and second order in $B$.$(i)$ Write the differential rate equation.$(ii)$ How is the rate affected on increasing the concentration of $B$ three times?$(iii)$ How is the rate affected when the concentrations of both $A$ and $B$ are doubled?

Vedclass Test Series

Exam Paper Generator

Online Exam Module

The following are the rate constants of two different reactions. What is the overall order of reaction for each?
$(a)$ $2.418 \times 10^{-5} \ hr^{-1}$
$(b)$ $7.1 \times 10^{-4} \ atm \ s^{-1}$

Assertion : The kinetics of the reaction $mA + nB + pC \to m'X + n'Y + p'Z$ obey the rate expression as $\frac{dX}{dt} = k[A]^m[B]^n$.
Reason : The rate of the reaction does not depend upon the concentration of $C$.

The hydrolysis of ethyl acetate is a reaction of $.........$ order.
$CH_3COOEt + H_2O \xrightarrow{H^{+}} CH_3COOH + EtOH$

$A$ reaction is first order in $A$ and second order in $B$.
$(i)$ Write the differential rate equation.
$(ii)$ How is the rate affected on increasing the concentration of $B$ three times?
$(iii)$ How is the rate affected when the concentrations of both $A$ and $B$ are doubled?