(C) The initial rate is $R_1 = k[A]^n[B]^m$. When the concentration of $A$ is doubled $([A]' = 2[A])$ and the concentration of $B$ is halved $([B]' =

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(C) The initial rate is $R_1 = k[A]^n[B]^m$. When the concentration of $A$ is doubled $([A]' = 2[A])$ and the concentration of $B$ is halved $([B]' = \frac{1}{2}[B])$,the new rate $R_2$ is: $R_2 = k(2[A])^n(\frac{1}{2}[B])^m$ $R_2 = k \times 2^n \times [A]^n \times (\frac{1}{2})^m \times [B]^m$ $R_2 = 2^n \times 2^{-m} \times k[A]^n[B]^m$ $R_2 = 2^{(n-m)} \times R_1$ Therefore,the ratio of the new rate to the initial rate is $\frac{R_2}{R_1} = 2^{(n-m)}$.

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

Easy

The rate law for the reaction between substances $A$ and $B$ is given by $\text{Rate} = k[A]^n[B]^m$. If the concentration of $A$ is doubled and the concentration of $B$ is halved,what is the ratio of the new rate to the initial rate?

A
$2^{(n+m)}$
B
$\frac{1}{2^{(m-n)}}$
C
$2^{(n-m)}$
D
$2^{(m-n)}$

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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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The rate law for the reaction between substances $A$ and $B$ is given by $\text{Rate} = k[A]^n[B]^m$. If the concentration of $A$ is doubled and the concentration of $B$ is halved,what is the ratio of the new rate to the initial rate?

Similar Questions

What is the order of reaction for the decomposition of gaseous acetaldehyde?

For the reaction $A + B \to C$,it is found that doubling the concentration of $A$ increases the rate by $4$ times,and doubling the concentration of $B$ doubles the reaction rate. What is the overall order of the reaction?

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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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