(C) The rate law can be expressed as $Rate = k[A]^x[B]^y$. When the concentration of $A$ is doubled, the rate doubles, which implies $2^x = 2$, so $x

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(C) The rate law can be expressed as $Rate = k[A]^x[B]^y$. When the concentration of $A$ is doubled, the rate doubles, which implies $2^x = 2$, so $x = 1$. When both concentrations are increased by four times, the rate increases by four times: $4^x \times 4^y = 4$. Substituting $x = 1$, we get $4^1 \times 4^y = 4$, which means $4^y = 1$, so $y = 0$. The total order of the reaction is $x + y = 1 + 0 = 1$.

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

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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

WBJEE 2015 All WBJEE

A
$3$
B
$0$
C
$1$
D
$2$

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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The half-life period of a gaseous reactant undergoing thermal decomposition was measured for various initial pressures $P_0$ as follows:
$P_0 \text{ (mmHg)}$ $250$ $300$
$t_{1/2} \text{ (minutes)}$ $135$ $112.5$

The order of reaction is -

Medium

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For the elementary reaction $M \rightarrow N$,the rate of disappearance of $M$ increases by a factor of $8$ upon doubling the concentration of $M$. The order of the reaction with respect to $M$ is :

MediumIIT 2014

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For a reaction $A + B \longrightarrow P$,the following data are provided. The rate constant for this reaction in standard units is:
Entry $[A]$ in $M$ $[B]$ in $M$ Initial rate $(M/s)$
$1$ $0.02$ $0.02$ $2 \times 10^{-2}$
$2$ $0.02$ $0.04$ $4 \times 10^{-2}$
$3$ $0.04$ $0.04$ $8 \times 10^{-2}$

Entry	$[A]$ in $M$	$[B]$ in $M$	Initial rate $(M/s)$
$1$	$0.02$	$0.02$	$2 \times 10^{-2}$
$2$	$0.02$	$0.04$	$4 \times 10^{-2}$
$3$	$0.04$	$0.04$	$8 \times 10^{-2}$

DifficultTS EAMCET 2021

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Write about elementary and complex reactions.

Medium

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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:

MediumMHT CET 2022

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$P_0 \text{ (mmHg)}$	$250$	$300$
$t_{1/2} \text{ (minutes)}$	$135$	$112.5$

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

Similar Questions

The half-life period of a gaseous reactant undergoing thermal decomposition was measured for various initial pressures $P_0$ as follows: $P_0 \text{ (mmHg)}$$250$$300$$t_{1/2} \text{ (minutes)}$$135$$112.5$The order of reaction is -

For the elementary reaction $M \rightarrow N$,the rate of disappearance of $M$ increases by a factor of $8$ upon doubling the concentration of $M$. The order of the reaction with respect to $M$ is :

For a reaction $A + B \longrightarrow P$,the following data are provided. The rate constant for this reaction in standard units is:Entry$[A]$ in $M$$[B]$ in $M$Initial rate $(M/s)$$1$$0.02$$0.02$$2 \times 10^{-2}$$2$$0.02$$0.04$$4 \times 10^{-2}$$3$$0.04$$0.04$$8 \times 10^{-2}$

Write about elementary and complex reactions.

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:

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The half-life period of a gaseous reactant undergoing thermal decomposition was measured for various initial pressures $P_0$ as follows:
$P_0 \text{ (mmHg)}$ $250$ $300$
$t_{1/2} \text{ (minutes)}$ $135$ $112.5$

The order of reaction is -

For a reaction $A + B \longrightarrow P$,the following data are provided. The rate constant for this reaction in standard units is:
Entry $[A]$ in $M$ $[B]$ in $M$ Initial rate $(M/s)$
$1$ $0.02$ $0.02$ $2 \times 10^{-2}$
$2$ $0.02$ $0.04$ $4 \times 10^{-2}$
$3$ $0.04$ $0.04$ $8 \times 10^{-2}$