(B) The rate law is given by $r = k[A][B]^{0.5}$.Concentration is defined as $C = n/V$,where $n$ is the number of moles and $V$ is the volume.If the v

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(B) The rate law is given by $r = k[A][B]^{0.5}$.Concentration is defined as $C = n/V$,where $n$ is the number of moles and $V$ is the volume.If the volume $V$ is reduced to $V/4$,the concentration becomes $C' = n/(V/4) = 4(n/V) = 4C$.Substituting the new concentrations $[A]' = 4[A]$ and $[B]' = 4[B]$ into the rate law:$r' = k[A]'([B]')^{0.5} = k(4[A])(4[B])^{0.5}$.$r' = k \times 4[A] \times 2[B]^{0.5} = 8 \times k[A][B]^{0.5}$.$r' = 8r$.Therefore,the rate of reaction increases by $8$ times.

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

Medium

For a particular reaction,the rate expression is given as $r = k[A][B]^{0.5}$. If the volume of the vessel is reduced to one-fourth of the initial volume,the rate of reaction would

A
decrease $1/4$ times
B
increase by $8$ times
C
decrease by $1/8$ times
D
remain unaffected

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Class 12

Chemistry Questions

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

Which of the following statements is true regarding the order of a reaction?

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For a reaction $2 \ A + B \rightarrow P$, when the concentration of $B$ alone is doubled, the rate does not change, and when the concentrations of both $A$ and $B$ are doubled, the rate increases by a factor of $4$. The unit of the rate constant is,

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$A$ complex reaction takes place in the following steps:
$NO_2Cl_{(g)} \longrightarrow NO_{2(g)} + Cl_{(g)}$ (slow)
$NO_2Cl_{(g)} + Cl_{(g)} \longrightarrow NO_{2(g)} + Cl_{2(g)}$ (fast)
Identify the rate law equation for this reaction.

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For the reaction $A + 2B \longrightarrow C$, the reaction rate is doubled if the concentration of $A$ is doubled. The rate is increased by four times when concentrations of both $A$ and $B$ are increased by four times. The order of the reaction is

EasyWBJEE 2015

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The rate of reaction $A + 2B \to 3C$ becomes $72$ times when the concentration of $A$ is tripled and the concentration of $B$ is doubled. The order of reaction with respect to $A$ and $B$ respectively is:

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For a particular reaction,the rate expression is given as $r = k[A][B]^{0.5}$. If the volume of the vessel is reduced to one-fourth of the initial volume,the rate of reaction would

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Which of the following statements is true regarding the order of a reaction?

For a reaction $2 \ A + B \rightarrow P$, when the concentration of $B$ alone is doubled, the rate does not change, and when the concentrations of both $A$ and $B$ are doubled, the rate increases by a factor of $4$. The unit of the rate constant is,

$A$ complex reaction takes place in the following steps:$NO_2Cl_{(g)} \longrightarrow NO_{2(g)} + Cl_{(g)}$ (slow)$NO_2Cl_{(g)} + Cl_{(g)} \longrightarrow NO_{2(g)} + Cl_{2(g)}$ (fast)Identify the rate law equation for this reaction.

For the reaction $A + 2B \longrightarrow C$, the reaction rate is doubled if the concentration of $A$ is doubled. The rate is increased by four times when concentrations of both $A$ and $B$ are increased by four times. The order of the reaction is

The rate of reaction $A + 2B \to 3C$ becomes $72$ times when the concentration of $A$ is tripled and the concentration of $B$ is doubled. The order of reaction with respect to $A$ and $B$ respectively is:

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$A$ complex reaction takes place in the following steps:
$NO_2Cl_{(g)} \longrightarrow NO_{2(g)} + Cl_{(g)}$ (slow)
$NO_2Cl_{(g)} + Cl_{(g)} \longrightarrow NO_{2(g)} + Cl_{2(g)}$ (fast)
Identify the rate law equation for this reaction.