(C) The rate law for the reaction is given by $Rate = k[A]^2[B]^1$. Let the initial rate be $R_1 = k[A]^2[B]$. When the concentration of $A$ is double

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(C) The rate law for the reaction is given by $Rate = k[A]^2[B]^1$. Let the initial rate be $R_1 = k[A]^2[B]$. When the concentration of $A$ is doubled $(2[A])$ and the concentration of $B$ is halved $(0.5[B])$,the new rate $R_2$ is: $R_2 = k(2[A])^2(0.5[B])$ $R_2 = k(4[A]^2)(0.5[B])$ $R_2 = 2 \times k[A]^2[B]$ $R_2 = 2 \times R_1$. Therefore,the rate of the reaction increases by two times.

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

Easy

In the reaction $2A + B \to A_2B$,if the concentration of $A$ is doubled and the concentration of $B$ is halved,then the rate of the reaction will:

AIPMT 2000 All AIPMT

A
Increase by four times
B
Decrease by two times
C
Increase by two times
D
Remain the same

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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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$p \ (mm \ Hg)$	$50$	$100$	$200$	$400$
Relative $t_{1/2} \ (s)$	$4$	$2$	$1$	$0.5$

In the reaction $2A + B \to A_2B$,if the concentration of $A$ is doubled and the concentration of $B$ is halved,then the rate of the reaction will:

Similar Questions

The reaction $2 A + B + C \longrightarrow D + E$ is found to be first order in $A$,second order in $B$,and zero order in $C$. What is the effect of increasing the concentration of all reactants twice?

$A$ student has studied the decomposition of a gas $AB_3$ at $25^{\circ} C$. He obtained the following data. $p \ (mm \ Hg)$ $50$ $100$ $200$ $400$ Relative $t_{1/2} \ (s)$ $4$ $2$ $1$ $0.5$ The order of the reaction is

The half-life of a reaction is found to be inversely proportional to the cube of its initial concentration. The order of the reaction is:

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Vedclass Test Series

Exam Paper Generator

Online Exam Module

$A$ student has studied the decomposition of a gas $AB_3$ at $25^{\circ} C$. He obtained the following data.

$p \ (mm \ Hg)$ $50$ $100$ $200$ $400$

Relative $t_{1/2} \ (s)$ $4$ $2$ $1$ $0.5$

The order of the reaction is