(C) The initial rate law is given by $r = K[A][B][C]^2$. If the concentration of $A$ is halved,the new concentration becomes $[A]' = \frac{[A]}{2}$. T

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(C) The initial rate law is given by $r = K[A][B][C]^2$. If the concentration of $A$ is halved,the new concentration becomes $[A]' = \frac{[A]}{2}$. The new rate of reaction $r'$ is given by $r' = K[A]'][B][C]^2 = K(\frac{[A]}{2})[B][C]^2$. Substituting the initial rate expression,we get $r' = \frac{1}{2} K[A][B][C]^2 = \frac{1}{2} r$. Therefore,the rate of reaction decreases $\frac{1}{2}$ times.

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

Medium

The rate law for a reaction between reactants $A$,$B$,and $C$ is $r = K[A][B][C]^2$. If the concentration of $A$ is halved,then the rate of reaction:

MHT CET 2022 All MHT CET

A
increases $\frac{1}{2}$ times
B
remains the same
C
decreases $\frac{1}{2}$ times
D
increases $2$ times

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Class 12 Questions

Class 12

Chemistry Questions

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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For the reaction $NO_2 + CO \rightarrow CO_2 + NO$,the rate law is given as $\text{Rate} = K [NO_2]^2$. What is the number of $CO$ molecules participating in the slow step?

Easy

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$A$ reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is $(i)$ doubled $(ii)$ reduced to half?

Medium

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If the reaction between $A$ and $B$ to give $C$ shows first-order kinetics in $A$ and second-order in $B$,the rate equation can be written as:

Easy

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

Experiment $[A] \ (M), [B] \ (M)$ and Initial rate of formation of $D$

$i. \ [A]=0.1, [B]=0.1$ $6.0 \times 10^{-3} \ M \ s^{-1}$

$ii. \ [A]=0.3, [B]=0.2$ $7.2 \times 10^{-2} \ M \ s^{-1}$

$iii. \ [A]=0.3, [B]=0.4$ $2.88 \times 10^{-1} \ M \ s^{-1}$

$iv. \ [A]=0.4, [B]=0.1$ $2.40 \times 10^{-2} \ M \ s^{-1}$

Based on the above data,the overall order of the reaction is:

Experiment	$[A] \ (M), [B] \ (M)$ and Initial rate of formation of $D$
$i. \ [A]=0.1, [B]=0.1$	$6.0 \times 10^{-3} \ M \ s^{-1}$
$ii. \ [A]=0.3, [B]=0.2$	$7.2 \times 10^{-2} \ M \ s^{-1}$
$iii. \ [A]=0.3, [B]=0.4$	$2.88 \times 10^{-1} \ M \ s^{-1}$
$iv. \ [A]=0.4, [B]=0.1$	$2.40 \times 10^{-2} \ M \ s^{-1}$

MediumJEE MAIN 2024

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Which of the following rate laws has an overall order of $0.5$ for a reaction involving substances $x$,$y$,and $z$?

MediumAIIMS 1983

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The rate law for a reaction between reactants $A$,$B$,and $C$ is $r = K[A][B][C]^2$. If the concentration of $A$ is halved,then the rate of reaction:

Similar Questions

For the reaction $NO_2 + CO \rightarrow CO_2 + NO$,the rate law is given as $\text{Rate} = K [NO_2]^2$. What is the number of $CO$ molecules participating in the slow step?

$A$ reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is $(i)$ doubled $(ii)$ reduced to half?

If the reaction between $A$ and $B$ to give $C$ shows first-order kinetics in $A$ and second-order in $B$,the rate equation can be written as:

Which of the following rate laws has an overall order of $0.5$ for a reaction involving substances $x$,$y$,and $z$?

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