(D) The rate law is given by $Rate = k [A] [B]$.Since concentration $[C] = n/V$,if the volume $V$ is reduced to $V/4$,the concentration of each reacta

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(D) The rate law is given by $Rate = k [A] [B]$.Since concentration $[C] = n/V$,if the volume $V$ is reduced to $V/4$,the concentration of each reactant becomes $4$ times the initial concentration.New rate $Rate' = k [4A] [4B] = 16 \times k [A] [B]$.Therefore,the rate of the reaction becomes $16$ times the initial rate.

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

Medium

For a gaseous reaction,the rate is given by $Rate = k [A] [B]$. If the volume of the container is reduced to $1/4$ of its initial volume,the rate of the reaction will become how many times the initial rate?

A
$1/8$
B
$8$
C
$1/16$
D
$16$

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Class 12 Questions

Class 12

Chemistry Questions

Chapter

Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

During the kinetic study of the reaction,$2A + B \rightarrow C + D,$ the following results were obtained:

$Run$ $[A] / mol \ L^{-1}$ $[B] / mol \ L^{-1}$ Initial rate of formation of $D / mol \ L^{-1} \ min^{-1}$

$I.$ $0.1$ $0.1$ $6.0 \times 10^{-3}$

$II.$ $0.3$ $0.2$ $7.2 \times 10^{-2}$

$III.$ $0.3$ $0.4$ $2.88 \times 10^{-1}$

$IV.$ $0.4$ $0.1$ $2.40 \times 10^{-2}$

Based on the above data,which one of the following is correct?

AIPMT 2010

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The alkaline hydrolysis of an ester is a ........ reaction.

Difficult

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The rate of reaction at $273 \ K$ is $R_0$. The rate of reaction at $313 \ K$ will be (Assuming temperature coefficient equal to $2$).

Medium

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For the reaction,$2N_2O_5 \to 4NO_2 + O_2$,the rate and rate constant are $1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$ and $3.4 \times 10^{-5} \ s^{-1}$ respectively. The concentration of $N_2O_5$ in $mol \ L^{-1}$ will be:

Medium

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What is the order and molecularity respectively for the elementary reaction given below?
$O_{3(g)} + O_{(g)} \rightarrow 2O_{2(g)}$ if $r = k[O_3][O]$

MediumMHT CET 2025

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$Run$	$[A] / mol \ L^{-1}$	$[B] / mol \ L^{-1}$	Initial rate of formation of $D / mol \ L^{-1} \ min^{-1}$
$I.$	$0.1$	$0.1$	$6.0 \times 10^{-3}$
$II.$	$0.3$	$0.2$	$7.2 \times 10^{-2}$
$III.$	$0.3$	$0.4$	$2.88 \times 10^{-1}$
$IV.$	$0.4$	$0.1$	$2.40 \times 10^{-2}$

For a gaseous reaction,the rate is given by $Rate = k [A] [B]$. If the volume of the container is reduced to $1/4$ of its initial volume,the rate of the reaction will become how many times the initial rate?

Similar Questions

The alkaline hydrolysis of an ester is a ........ reaction.

The rate of reaction at $273 \ K$ is $R_0$. The rate of reaction at $313 \ K$ will be (Assuming temperature coefficient equal to $2$).

For the reaction,$2N_2O_5 \to 4NO_2 + O_2$,the rate and rate constant are $1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$ and $3.4 \times 10^{-5} \ s^{-1}$ respectively. The concentration of $N_2O_5$ in $mol \ L^{-1}$ will be:

What is the order and molecularity respectively for the elementary reaction given below? $O_{3(g)} + O_{(g)} \rightarrow 2O_{2(g)}$ if $r = k[O_3][O]$

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What is the order and molecularity respectively for the elementary reaction given below?
$O_{3(g)} + O_{(g)} \rightarrow 2O_{2(g)}$ if $r = k[O_3][O]$