(D) The rate law for the reaction $A \to B$ is given by $r = k[A]^x$,where $x$ is the order of reaction.For the first condition: $2.40 \times 10^{-4}

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(D) The rate law for the reaction $A \to B$ is given by $r = k[A]^x$,where $x$ is the order of reaction.For the first condition: $2.40 \times 10^{-4} = k(2 \times 10^{-3})^x$ $(i)$For the second condition: $0.60 \times 10^{-4} = k(1 \times 10^{-3})^x$ $(ii)$Dividing equation $(i)$ by equation $(ii)$:$\frac{2.40 \times 10^{-4}}{0.60 \times 10^{-4}} = \frac{k(2 \times 10^{-3})^x}{k(1 \times 10^{-3})^x}$$4 = (2)^x$Since $4 = 2^2$,we have $x = 2$.Therefore,the order of reaction with respect to $A$ is $2$.

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

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In a chemical reaction $A$ is converted into $B$. The rates of reaction,starting with initial concentrations of $A$ as $2 \times 10^{-3} \ M$ and $1 \times 10^{-3} \ M$,are equal to $2.40 \times 10^{-4} \ M s^{-1}$ and $0.60 \times 10^{-4} \ M s^{-1}$ respectively. The order of reaction with respect to reactant $A$ will be

AIEEE 2012 All AIEEE

A
$0$
B
$1.5$
C
$1$
D
$2$

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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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........ of a reaction cannot be determined experimentally.

EasyTS EAMCET 2004

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The mechanism of the reaction $A + 2B \to D$ is given by:
$2B \xrightarrow{k} B_2$ [Slow]
$B_2 + A \to D$ [Fast]
The rate law expression,order with respect to $A$,order with respect to $B$,and overall order are respectively:

Medium

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The rate law for the reaction below is given by the expression $Rate = k[A][B]$.
$A + B \to \text{Product}$
If the concentration of $B$ is increased from $0.1 \ M$ to $0.3 \ M$,keeping the concentration of $A$ constant at $0.1 \ M$,the rate constant $(k)$ will be:

DifficultJEE MAIN 2016

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For the catalytic decomposition of $AB_3$, the half-life period is $4 \, \text{hours}$ at $50 \, \text{mm}$ and $2 \, \text{hours}$ at $100 \, \text{mm}$. What is the order of the reaction?

Medium

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The rate equation for the reaction $2A + B \to C$ is found to be: $\text{rate} = k[A][B]$. The correct statement in relation to this reaction is that the

MediumAIEEE 2004

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........ of a reaction cannot be determined experimentally.

The mechanism of the reaction $A + 2B \to D$ is given by:$2B \xrightarrow{k} B_2$ [Slow]$B_2 + A \to D$ [Fast]The rate law expression,order with respect to $A$,order with respect to $B$,and overall order are respectively:

The rate law for the reaction below is given by the expression $Rate = k[A][B]$.$A + B \to \text{Product}$If the concentration of $B$ is increased from $0.1 \ M$ to $0.3 \ M$,keeping the concentration of $A$ constant at $0.1 \ M$,the rate constant $(k)$ will be:

For the catalytic decomposition of $AB_3$, the half-life period is $4 \, \text{hours}$ at $50 \, \text{mm}$ and $2 \, \text{hours}$ at $100 \, \text{mm}$. What is the order of the reaction?

The rate equation for the reaction $2A + B \to C$ is found to be: $\text{rate} = k[A][B]$. The correct statement in relation to this reaction is that the

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The mechanism of the reaction $A + 2B \to D$ is given by:
$2B \xrightarrow{k} B_2$ [Slow]
$B_2 + A \to D$ [Fast]
The rate law expression,order with respect to $A$,order with respect to $B$,and overall order are respectively:

The rate law for the reaction below is given by the expression $Rate = k[A][B]$.
$A + B \to \text{Product}$
If the concentration of $B$ is increased from $0.1 \ M$ to $0.3 \ M$,keeping the concentration of $A$ constant at $0.1 \ M$,the rate constant $(k)$ will be: