(B) The rate law for the reaction with respect to reactant $B$ is given by $R = k[B]^n$,where $n$ is the order of reaction with respect to $B$. Accord

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(B) The rate law for the reaction with respect to reactant $B$ is given by $R = k[B]^n$,where $n$ is the order of reaction with respect to $B$. According to the problem,if the concentration of $B$ is doubled $([B]' = 2[B])$,the rate becomes one-fourth of the original rate $(R' = \frac{1}{4}R)$. Substituting these into the rate law: $\frac{1}{4}R = k(2[B])^n$ Dividing the new rate equation by the original rate equation: $\frac{\frac{1}{4}R}{R} = \frac{k(2[B])^n}{k[B]^n}$ $\frac{1}{4} = 2^n$ $2^{-2} = 2^n$ Therefore,$n = -2$.

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

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The rate of reaction between two reactants $A$ and $B$ decreases by a factor of $4$ if the concentration of reactant $B$ is doubled. The order of this reaction with respect to reactant $B$ is

AIPMT 2005 All AIPMT

A
$-1$
B
$-2$
C
$1$
D
$2$

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Class 12

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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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

Medium

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The rate constant of esterification is given by $k = k^{\prime} [H_2O]$. If the rate constant $k = 2.0 \times 10^{-3} \ min^{-1}$,calculate $k^{\prime}$. (Assume $[H_2O] = 55.5 \ mol \ L^{-1}$)

Medium

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The unit of rate constant for a second-order reaction is usually expressed as:

Easy

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For conversion of compound $A \rightarrow B$,the rate constant of the reaction was found to be $4.6 \times 10^{-5} \ L \ mol^{-1} \ s^{-1}$. The order of the reaction is $..........$

MediumJEE MAIN 2023

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

The rate of reaction between two reactants $A$ and $B$ decreases by a factor of $4$ if the concentration of reactant $B$ is doubled. The order of this reaction with respect to reactant $B$ 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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