(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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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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The velocity constant of a reaction is $K$. Which of the following statements is not true regarding $K$?

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For the reaction $A + B \rightarrow \text{product}$,the rate of reaction is $3.6 \times 10^{-2} \ mol \ dm^{-3} \ sec^{-1}$. When $[A] = 0.2 \ mol \ dm^{-3}$ and $[B] = 0.1 \ mol \ dm^{-3}$,calculate the rate constant of the reaction if the reaction is first order in $A$ and second order in $B$.

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$A$ chemical reaction proceeds through the following steps:
Step-$I$: $2A \rightleftharpoons X$ (fast)
Step-$II$: $X + B \rightarrow Y$ (slow)
Step-$III$: $Y + B \rightarrow \text{Product}$ (fast)
The rate law for the overall reaction is:

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For the following homogeneous reaction scheme,the rate constant has units for the reaction $A + B \xrightarrow{K} C$:

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The reaction $2NO + O_2 \rightarrow 2NO_2$ is an example of which order of reaction?

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The velocity constant of a reaction is $K$. Which of the following statements is not true regarding $K$?

For the reaction $A + B \rightarrow \text{product}$,the rate of reaction is $3.6 \times 10^{-2} \ mol \ dm^{-3} \ sec^{-1}$. When $[A] = 0.2 \ mol \ dm^{-3}$ and $[B] = 0.1 \ mol \ dm^{-3}$,calculate the rate constant of the reaction if the reaction is first order in $A$ and second order in $B$.

$A$ chemical reaction proceeds through the following steps:Step-$I$: $2A \rightleftharpoons X$ (fast)Step-$II$: $X + B \rightarrow Y$ (slow)Step-$III$: $Y + B \rightarrow \text{Product}$ (fast)The rate law for the overall reaction is:

For the following homogeneous reaction scheme,the rate constant has units for the reaction $A + B \xrightarrow{K} C$:

The reaction $2NO + O_2 \rightarrow 2NO_2$ is an example of which order of reaction?

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$A$ chemical reaction proceeds through the following steps:
Step-$I$: $2A \rightleftharpoons X$ (fast)
Step-$II$: $X + B \rightarrow Y$ (slow)
Step-$III$: $Y + B \rightarrow \text{Product}$ (fast)
The rate law for the overall reaction is: