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

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(A) The initial rate is given by $R = k[A]^n[B]^m$. When the concentration of $A$ is doubled $([A]' = 2[A])$ and the concentration of $B$ is halved $([B]' = \frac{B}{2})$,the new rate $R'$ is: $R' = k[2A]^n[\frac{B}{2}]^m$ $R' = k \cdot 2^n [A]^n \cdot 2^{-m} [B]^m$ $R' = k[A]^n[B]^m \cdot 2^{n - m}$ $R' = R \cdot 2^{n - m}$ Therefore,the ratio of the new rate to the earlier rate is: $\frac{R'}{R} = 2^{n - m}$.

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

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The rate law for a reaction between the substances $A$ and $B$ is given by,$rate = k[A]^n[B]^m$. On doubling the concentration of $A$ and halving the concentration of $B$,the ratio of the new rate to the earlier rate of the reaction will be as

AIEEE 2003 All AIEEE

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

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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AIEEE 2003 Paper All AIEEE years →

Write the differential rate expression for the following reactions and determine their order of reaction:
$1) \ 2 \ HI \rightarrow H_2 + I_2$
$2) \ 2 \ NO_{(g)} + O_{2(g)} \rightarrow 2 \ NO_{2(g)}$

Medium

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For a gaseous reaction $2A + B \rightarrow C + D$,the rate of reaction is given by $Rate = K[A][B]$. If the volume of the container is reduced to $1/4$ of its original volume,what will be the ratio of the new rate to the original rate?

Medium

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Consider the following reaction: $A \longrightarrow \text{Products}$. This reaction is completed in $100 \ min$. The rate constant of this reaction at $t_1 = 10 \ min$ is $10^{-2} \ min^{-1}$. What is the rate constant (in $min^{-1}$) at $t_2 = 20 \ min$?

MediumAP EAMCET 2022

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Consider the following two reactions:
$A \to \text{Product}; -\frac{d[A]}{dt} = k_1[A]^0$
$B \to \text{Product}; -\frac{d[B]}{dt} = k_2[B]$
The units of $k_1$ and $k_2$ are expressed in terms of molarity $(M)$ and time $(sec^{-1})$ as:

Medium

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Inversion of cane sugar in dilute acid (conversion into glucose and fructose) is a:

Easy

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The rate law for a reaction between the substances $A$ and $B$ is given by,$rate = k[A]^n[B]^m$. On doubling the concentration of $A$ and halving the concentration of $B$,the ratio of the new rate to the earlier rate of the reaction will be as

Similar Questions

Write the differential rate expression for the following reactions and determine their order of reaction:$1) \ 2 \ HI \rightarrow H_2 + I_2$$2) \ 2 \ NO_{(g)} + O_{2(g)} \rightarrow 2 \ NO_{2(g)}$

For a gaseous reaction $2A + B \rightarrow C + D$,the rate of reaction is given by $Rate = K[A][B]$. If the volume of the container is reduced to $1/4$ of its original volume,what will be the ratio of the new rate to the original rate?

Consider the following reaction: $A \longrightarrow \text{Products}$. This reaction is completed in $100 \ min$. The rate constant of this reaction at $t_1 = 10 \ min$ is $10^{-2} \ min^{-1}$. What is the rate constant (in $min^{-1}$) at $t_2 = 20 \ min$?

Consider the following two reactions:$A \to \text{Product}; -\frac{d[A]}{dt} = k_1[A]^0$$B \to \text{Product}; -\frac{d[B]}{dt} = k_2[B]$The units of $k_1$ and $k_2$ are expressed in terms of molarity $(M)$ and time $(sec^{-1})$ as:

Inversion of cane sugar in dilute acid (conversion into glucose and fructose) is a:

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Write the differential rate expression for the following reactions and determine their order of reaction:
$1) \ 2 \ HI \rightarrow H_2 + I_2$
$2) \ 2 \ NO_{(g)} + O_{2(g)} \rightarrow 2 \ NO_{2(g)}$

Consider the following two reactions:
$A \to \text{Product}; -\frac{d[A]}{dt} = k_1[A]^0$
$B \to \text{Product}; -\frac{d[B]}{dt} = k_2[B]$
The units of $k_1$ and $k_2$ are expressed in terms of molarity $(M)$ and time $(sec^{-1})$ as: