(A) Let the rate law be $r = k[A_2]^a[B_2]^b$.From the table:$1) 0.04 = k(0.2)^a(0.2)^b$$2) 0.04 = k(0.1)^a(0.4)^b$$3) 0.08 = k(0.2)^a(0.4)^b$Dividing

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(A) Let the rate law be $r = k[A_2]^a[B_2]^b$.From the table:$1) 0.04 = k(0.2)^a(0.2)^b$$2) 0.04 = k(0.1)^a(0.4)^b$$3) 0.08 = k(0.2)^a(0.4)^b$Dividing $(3)$ by $(1)$:$\frac{0.08}{0.04} = \frac{k(0.2)^a(0.4)^b}{k(0.2)^a(0.2)^b} \implies 2 = (2)^b \implies b = 1$.Dividing $(3)$ by $(2)$:$\frac{0.08}{0.04} = \frac{k(0.2)^a(0.4)^b}{k(0.1)^a(0.4)^b} \implies 2 = (2)^a \implies a = 1$.Thus,$a = 1$ and $b = 1$.

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

Medium

$A_2 + B_2 \to 2AB$; $R.O.R = k[A_2]^a[B_2]^b$

Initial $[A_2]$ Initial $[B_2]$ $R.O.R. (r) \ M s^{-1}$

$0.2$ $0.2$ $0.04$

$0.1$ $0.4$ $0.04$

$0.2$ $0.4$ $0.08$

Order of reaction with respect to $A_2$ and $B_2$ are respectively:

Initial $[A_2]$	Initial $[B_2]$	$R.O.R. (r) \ M s^{-1}$
$0.2$	$0.2$	$0.04$
$0.1$	$0.4$	$0.04$
$0.2$	$0.4$	$0.08$

A
$a = 1, b = 1$
B
$a = 2, b = 0$
C
$a = 2, b = 1$
D
None

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Class 12 Questions

Class 12

Chemistry Questions

Chapter

Chemical Kinetics

Subtopic

Rate law , Rate constant , Order of Reaction and Molecularity

The reaction $2 \ NO + Br_2 \rightarrow 2 \ NOBr$ takes place through the mechanism given below:
$NO + Br_2 \Leftrightarrow NOBr_2$ (fast)
$NOBr_2 + NO \rightarrow 2 \ NOBr$ (slow)
The overall order of the reaction is $.....$.

MediumJEE MAIN 2023

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For the reaction: $KClO_3 + 6FeSO_4 + 3H_2SO_4 \to KCl + 3Fe_2(SO_4)_3 + 3H_2O$. Determine if the following statement is True $(T)$ or False $(F)$: The reaction is elementary.

Easy

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For the reaction $2A + B \rightarrow C$,the rate law is given by $\text{Rate} = k[A][B]$. Which of the following statements is correct for this reaction?

Medium

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For a gaseous reaction,the rate is given by $Rate = k [A] [B]$. If the volume of the container is reduced to $1/4$ of its initial volume,the rate of the reaction will become how many times the initial rate?

Medium

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For the non-stoichiometric reaction $2A + B \to C + D$,the following kinetic data were obtained in three separate experiments,all at $298 \ K$.

Initial Conc. $(A)$ Initial Conc. $(B)$ Initial rate of formation of $C \ (mol \ L^{-1} \ s^{-1})$

$0.1 \ M$ $0.1 \ M$ $1.2 \times 10^{-3}$

$0.1 \ M$ $0.2 \ M$ $1.2 \times 10^{-3}$

$0.2 \ M$ $0.1 \ M$ $2.4 \times 10^{-3}$

For the reaction,the rate of formation of $C$ will be:

Medium

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Initial Conc. $(A)$	Initial Conc. $(B)$	Initial rate of formation of $C \ (mol \ L^{-1} \ s^{-1})$
$0.1 \ M$	$0.1 \ M$	$1.2 \times 10^{-3}$
$0.1 \ M$	$0.2 \ M$	$1.2 \times 10^{-3}$
$0.2 \ M$	$0.1 \ M$	$2.4 \times 10^{-3}$

$A_2 + B_2 \to 2AB$; $R.O.R = k[A_2]^a[B_2]^b$ Initial $[A_2]$ Initial $[B_2]$ $R.O.R. (r) \ M s^{-1}$ $0.2$ $0.2$ $0.04$ $0.1$ $0.4$ $0.04$ $0.2$ $0.4$ $0.08$ Order of reaction with respect to $A_2$ and $B_2$ are respectively:

Similar Questions

The reaction $2 \ NO + Br_2 \rightarrow 2 \ NOBr$ takes place through the mechanism given below:$NO + Br_2 \Leftrightarrow NOBr_2$ (fast)$NOBr_2 + NO \rightarrow 2 \ NOBr$ (slow)The overall order of the reaction is $.....$.

For the reaction: $KClO_3 + 6FeSO_4 + 3H_2SO_4 \to KCl + 3Fe_2(SO_4)_3 + 3H_2O$. Determine if the following statement is True $(T)$ or False $(F)$: The reaction is elementary.

For the reaction $2A + B \rightarrow C$,the rate law is given by $\text{Rate} = k[A][B]$. Which of the following statements is correct for this reaction?

For a gaseous reaction,the rate is given by $Rate = k [A] [B]$. If the volume of the container is reduced to $1/4$ of its initial volume,the rate of the reaction will become how many times the initial rate?

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$A_2 + B_2 \to 2AB$; $R.O.R = k[A_2]^a[B_2]^b$

Initial $[A_2]$ Initial $[B_2]$ $R.O.R. (r) \ M s^{-1}$

$0.2$ $0.2$ $0.04$

$0.1$ $0.4$ $0.04$

$0.2$ $0.4$ $0.08$

Order of reaction with respect to $A_2$ and $B_2$ are respectively:

The reaction $2 \ NO + Br_2 \rightarrow 2 \ NOBr$ takes place through the mechanism given below:
$NO + Br_2 \Leftrightarrow NOBr_2$ (fast)
$NOBr_2 + NO \rightarrow 2 \ NOBr$ (slow)
The overall order of the reaction is $.....$.