(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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The three experimental data for determining the differential rate of reaction $Cl_{2(g)} + 2NO_{(g)} \rightarrow 2NOCl_{(g)}$ at $310 \ K$ temperature are provided. $(a)$ Derive the differential rate of reaction. $(b)$ Calculate the order of reaction. $(c)$ Calculate the value of the rate constant.

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The rate law for the reaction,$NO_{2(g)} + CO_{(g)} \rightarrow NO_{(g)} + CO_{2(g)}$ is given as $R = k[NO_2]^2$. What is the order of reaction with respect to $CO$?

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For three reactions of first,second,and third order,the rate constants are numerically equal. If the concentration of the reactant is the same and greater than $1 \ M$,which of the following is true for the rates of these three reactions?

Medium

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$(a)$ Write the general reaction and derive the units of the rate constant. $(b)$ Based on that,write the rate constant units for zero,first,and $2^{nd}$ order reactions.

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For the gaseous reaction,$N_2O_5 \rightarrow 2NO_2 + \frac{1}{2}O_2$,the rate can be expressed as:
$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$
$+\frac{d[NO_2]}{dt} = K_2[N_2O_5]$
$+\frac{d[O_2]}{dt} = K_3[N_2O_5]$
The correct relation between $K_1, K_2$ and $K_3$ is:

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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

The three experimental data for determining the differential rate of reaction $Cl_{2(g)} + 2NO_{(g)} \rightarrow 2NOCl_{(g)}$ at $310 \ K$ temperature are provided. $(a)$ Derive the differential rate of reaction. $(b)$ Calculate the order of reaction. $(c)$ Calculate the value of the rate constant.

The rate law for the reaction,$NO_{2(g)} + CO_{(g)} \rightarrow NO_{(g)} + CO_{2(g)}$ is given as $R = k[NO_2]^2$. What is the order of reaction with respect to $CO$?

For three reactions of first,second,and third order,the rate constants are numerically equal. If the concentration of the reactant is the same and greater than $1 \ M$,which of the following is true for the rates of these three reactions?

$(a)$ Write the general reaction and derive the units of the rate constant. $(b)$ Based on that,write the rate constant units for zero,first,and $2^{nd}$ order reactions.

For the gaseous reaction,$N_2O_5 \rightarrow 2NO_2 + \frac{1}{2}O_2$,the rate can be expressed as:$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$$+\frac{d[NO_2]}{dt} = K_2[N_2O_5]$$+\frac{d[O_2]}{dt} = K_3[N_2O_5]$The correct relation between $K_1, K_2$ and $K_3$ is:

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For the gaseous reaction,$N_2O_5 \rightarrow 2NO_2 + \frac{1}{2}O_2$,the rate can be expressed as:
$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$
$+\frac{d[NO_2]}{dt} = K_2[N_2O_5]$
$+\frac{d[O_2]}{dt} = K_3[N_2O_5]$
The correct relation between $K_1, K_2$ and $K_3$ is: