(A) The rate of reaction is given by: $\text{Rate} = k[A]^x$. The unit of rate is $\text{mol} \ L^{-1} \ sec^{-1}$. The unit of concentration $[A]$ is

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$mol^{1-x} \ L^{x-1} \ sec^{-1}$

(A) The rate of reaction is given by: $\text{Rate} = k[A]^x$. The unit of rate is $\text{mol} \ L^{-1} \ sec^{-1}$. The unit of concentration $[A]$ is $\text{mol} \ L^{-1}$. Substituting these into the rate law equation: $\text{mol} \ L^{-1} \ sec^{-1} = k \times (\text{mol} \ L^{-1})^x$. Solving for $k$: $k = \frac{\text{mol} \ L^{-1} \ sec^{-1}}{(\text{mol} \ L^{-1})^x} = (\text{mol} \ L^{-1})^{1-x} \ sec^{-1}$. Expanding this,we get: $k = \text{mol}^{1-x} \ L^{-(1-x)} \ sec^{-1} = \text{mol}^{1-x} \ L^{x-1} \ sec^{-1}$.

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

Medium

If the rate law of a reaction $n A \rightarrow B$ is expressed as Rate $= -\frac{1}{n} \frac{d[A]}{dt} = \frac{d[B]}{dt} = k[A]^{x}$,the unit of rate constant $k$ will be:

A
$mol^{1-x} \ L^{x-1} \ sec^{-1}$
B
$L^{x-1} \ mol^{1-x} \ sec^{-1}$
C
$mol^{x-1} \ L^{1-x} \ sec^{-1}$
D
$L^{x} \ mol^{-x} \ sec^{-1}$

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Class 12 Questions

Class 12

Chemistry Questions

Chapter

Chemical Kinetics

Subtopic

Rate law , Rate constant , Order of Reaction and Molecularity

Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$

$Expt. \ No.$ $[A]$ $[B]$ $Initial \ Rate$

$1$ $0.012$ $0.035$ $0.10$

$2$ $0.024$ $0.070$ $0.80$

$3$ $0.024$ $0.035$ $0.10$

$4$ $0.012$ $0.070$ $0.80$

$Expt. \ No.$	$[A]$	$[B]$	$Initial \ Rate$
$1$	$0.012$	$0.035$	$0.10$
$2$	$0.024$	$0.070$	$0.80$
$3$	$0.024$	$0.035$	$0.10$
$4$	$0.012$	$0.070$	$0.80$

DifficultAIIMS 2015

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What is the order of reaction for $A + B \to C$?

$Observation$ $[A] \ (mol \ L^{-1})$ $[B] \ (mol \ L^{-1})$ $Rate \ (mol \ L^{-1} \ sec^{-1})$

$1$ $0.1$ $0.1$ $2 \times 10^{-3}$

$2$ $0.2$ $0.1$ $4 \times 10^{-3}$

$3$ $0.1$ $0.2$ $8 \times 10^{-3}$

Medium

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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 reaction $2N_2O_5 \to 4NO_2 + O_2$,the rate of reaction and rate constant are $1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$ and $3.4 \times 10^{-5} \ s^{-1}$ respectively. The concentration of $N_2O_5$ at that time will be:

Medium

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The rate of the reaction: $2N_2O_5 \rightarrow 4NO_2 + O_2$ can be written in three ways.
$-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$
$\frac{d[NO_2]}{dt} = k'[N_2O_5]$ ; $\frac{d[O_2]}{dt} = k''[N_2O_5]$
The relationship between $k$ and $k'$ and between $k$ and $k''$ are:

DifficultAIPMT 2011

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$Observation$	$[A] \ (mol \ L^{-1})$	$[B] \ (mol \ L^{-1})$	$Rate \ (mol \ L^{-1} \ sec^{-1})$
$1$	$0.1$	$0.1$	$2 \times 10^{-3}$
$2$	$0.2$	$0.1$	$4 \times 10^{-3}$
$3$	$0.1$	$0.2$	$8 \times 10^{-3}$

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

If the rate law of a reaction $n A \rightarrow B$ is expressed as Rate $= -\frac{1}{n} \frac{d[A]}{dt} = \frac{d[B]}{dt} = k[A]^{x}$,the unit of rate constant $k$ will be:

Similar Questions

Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$ $Expt. \ No.$ $[A]$ $[B]$ $Initial \ Rate$ $1$ $0.012$ $0.035$ $0.10$ $2$ $0.024$ $0.070$ $0.80$ $3$ $0.024$ $0.035$ $0.10$ $4$ $0.012$ $0.070$ $0.80$

What is the order of reaction for $A + B \to C$? $Observation$ $[A] \ (mol \ L^{-1})$ $[B] \ (mol \ L^{-1})$ $Rate \ (mol \ L^{-1} \ sec^{-1})$ $1$ $0.1$ $0.1$ $2 \times 10^{-3}$ $2$ $0.2$ $0.1$ $4 \times 10^{-3}$ $3$ $0.1$ $0.2$ $8 \times 10^{-3}$

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 reaction $2N_2O_5 \to 4NO_2 + O_2$,the rate of reaction and rate constant are $1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$ and $3.4 \times 10^{-5} \ s^{-1}$ respectively. The concentration of $N_2O_5$ at that time will be:

The rate of the reaction: $2N_2O_5 \rightarrow 4NO_2 + O_2$ can be written in three ways.$-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$$\frac{d[NO_2]}{dt} = k'[N_2O_5]$ ; $\frac{d[O_2]}{dt} = k''[N_2O_5]$The relationship between $k$ and $k'$ and between $k$ and $k''$ are:

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Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$

$Expt. \ No.$ $[A]$ $[B]$ $Initial \ Rate$

$1$ $0.012$ $0.035$ $0.10$

$2$ $0.024$ $0.070$ $0.80$

$3$ $0.024$ $0.035$ $0.10$

$4$ $0.012$ $0.070$ $0.80$

What is the order of reaction for $A + B \to C$?

$Observation$ $[A] \ (mol \ L^{-1})$ $[B] \ (mol \ L^{-1})$ $Rate \ (mol \ L^{-1} \ sec^{-1})$

$1$ $0.1$ $0.1$ $2 \times 10^{-3}$

$2$ $0.2$ $0.1$ $4 \times 10^{-3}$

$3$ $0.1$ $0.2$ $8 \times 10^{-3}$

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 -

The rate of the reaction: $2N_2O_5 \rightarrow 4NO_2 + O_2$ can be written in three ways.
$-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$
$\frac{d[NO_2]}{dt} = k'[N_2O_5]$ ; $\frac{d[O_2]}{dt} = k''[N_2O_5]$
The relationship between $k$ and $k'$ and between $k$ and $k''$ are: