(D) For the reaction $2A + B \to C$,the rate law is given as $\text{rate} = k[A][B]$.According to the Arrhenius equation,$k = Ae^{-E_a/RT}$.This shows

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Value of $k$ is independent of the initial concentrations of $A$ and $B$

(D) For the reaction $2A + B \to C$,the rate law is given as $\text{rate} = k[A][B]$.According to the Arrhenius equation,$k = Ae^{-E_a/RT}$.This shows that the rate constant $k$ depends only on temperature and the activation energy $(E_a)$,not on the initial concentrations of the reactants $A$ and $B$.Therefore,the value of $k$ is independent of the initial concentrations of $A$ and $B$.

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

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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

AIEEE 2004 All AIEEE

A
Rate of formation of $C$ is twice the rate of disappearance of $A$
B
$t_{1/2}$ is a constant
C
Unit of $k$ must be $s^{-1}$
D
Value of $k$ is independent of the initial concentrations of $A$ and $B$

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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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Which is the unit of the rate constant for a second-order reaction?

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For a reaction,$A + B \rightarrow \text{Product}$; the rate law is given by,$r = k[A]^{1/2}[B]^2$. What is the order of the reaction?

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Which of the following statements is false?

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Determine the order of reaction on the basis of following data for the reaction $A + B \to C$.
Exp. $[A]$ $[B]$ Rate of reaction $(mol \ L^{-1} \ s^{-1})$
$1$ $0.1$ $0.1$ $2 \times 10^{-3}$
$2$ $0.4$ $0.1$ $0.8 \times 10^{-2}$
$3$ $0.1$ $0.2$ $1.6 \times 10^{-2}$
(in $.5$)

Exp.	$[A]$	$[B]$	Rate of reaction $(mol \ L^{-1} \ s^{-1})$
$1$	$0.1$	$0.1$	$2 \times 10^{-3}$
$2$	$0.4$	$0.1$	$0.8 \times 10^{-2}$
$3$	$0.1$	$0.2$	$1.6 \times 10^{-2}$

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

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

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

$2$ $0.4$ $0.1$ $3.2 \times 10^{-3}$

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

Observation	$[A] \ (mol \ L^{-1})$	$[B] \ (mol \ L^{-1})$	Rate $(mol \ L^{-1} \ sec^{-1})$
$1$	$0.1$	$0.1$	$2 \times 10^{-3}$
$2$	$0.4$	$0.1$	$3.2 \times 10^{-3}$
$3$	$0.1$	$0.2$	$8 \times 10^{-3}$

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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

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Which is the unit of the rate constant for a second-order reaction?

For a reaction,$A + B \rightarrow \text{Product}$; the rate law is given by,$r = k[A]^{1/2}[B]^2$. What is the order of the reaction?

Which of the following statements is false?

Determine the order of reaction on the basis of following data for the reaction $A + B \to C$.Exp.$[A]$$[B]$Rate of reaction $(mol \ L^{-1} \ s^{-1})$$1$$0.1$$0.1$$2 \times 10^{-3}$$2$$0.4$$0.1$$0.8 \times 10^{-2}$$3$$0.1$$0.2$$1.6 \times 10^{-2}$ (in $.5$)

What is the order of reaction $A + B \to C$? Observation $[A] \ (mol \ L^{-1})$ $[B] \ (mol \ L^{-1})$ Rate $(mol \ L^{-1} \ sec^{-1})$ $1$ $0.1$ $0.1$ $2 \times 10^{-3}$ $2$ $0.4$ $0.1$ $3.2 \times 10^{-3}$ $3$ $0.1$ $0.2$ $8 \times 10^{-3}$

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Determine the order of reaction on the basis of following data for the reaction $A + B \to C$.
Exp. $[A]$ $[B]$ Rate of reaction $(mol \ L^{-1} \ s^{-1})$
$1$ $0.1$ $0.1$ $2 \times 10^{-3}$
$2$ $0.4$ $0.1$ $0.8 \times 10^{-2}$
$3$ $0.1$ $0.2$ $1.6 \times 10^{-2}$
(in $.5$)

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

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

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

$2$ $0.4$ $0.1$ $3.2 \times 10^{-3}$

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