(A) The rate law is given by $r = k[A_2]^x[B]^y$.From the first two experiments,keeping $[B]$ constant at $0.2 \, M$:$1 \times 10^{-2} = k(0.1)^x(0.2)

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(A) The rate law is given by $r = k[A_2]^x[B]^y$.From the first two experiments,keeping $[B]$ constant at $0.2 \, M$:$1 \times 10^{-2} = k(0.1)^x(0.2)^y$$2 \times 10^{-2} = k(0.2)^x(0.2)^y$Dividing the equations: $2 = (2)^x$,so $x = 1$.From the second and third experiments,keeping $[A_2]$ constant at $0.2 \, M$:$2 \times 10^{-2} = k(0.2)^x(0.2)^y$$8 \times 10^{-2} = k(0.2)^x(0.4)^y$Dividing the equations: $4 = (2)^y$,so $y = 2$.Thus,the order with respect to $A_2$ is $1$ and with respect to $B$ is $2$.

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

Medium

$A_2 + 2 \, B \to 2 \, AB$

$[A_2]$ $[B]$ $-d[A_2]/dt$

$0.1$ $0.2$ $1 \times 10^{-2} \, M \, s^{-1}$

$0.2$ $0.2$ $2 \times 10^{-2} \, M \, s^{-1}$

$0.2$ $0.4$ $8 \times 10^{-2} \, M \, s^{-1}$

The order of reaction with respect to $A_2$ and $B$ are respectively:

$[A_2]$	$[B]$	$-d[A_2]/dt$
$0.1$	$0.2$	$1 \times 10^{-2} \, M \, s^{-1}$
$0.2$	$0.2$	$2 \times 10^{-2} \, M \, s^{-1}$
$0.2$	$0.4$	$8 \times 10^{-2} \, M \, s^{-1}$

A
$1, 2$
B
$2, 1$
C
$1, 1$
D
$2, 2$

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Class 12

Chemistry Questions

Chapter

Chemical Kinetics

Subtopic

Rate law , Rate constant , Order of Reaction and Molecularity

For a reaction $A + B \rightarrow \text{product}$,if $[A]$ is doubled keeping $[B]$ constant,the rate of reaction doubles. Calculate the order of reaction with respect to $A$.

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

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

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

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

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

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

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

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For a gaseous reaction $2A + B \rightarrow C + D$,the rate of reaction is given by $Rate = K[A][B]$. If the volume of the container is reduced to $1/4$ of its original volume,what will be the ratio of the new rate to the original rate?

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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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The rate constant of a reaction is $1.388 \times 10^{-3} \ mol^{-2} \ L^{2} \ s^{-1}$. The order of the reaction is:

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$A_2 + 2 \, B \to 2 \, AB$ $[A_2]$ $[B]$ $-d[A_2]/dt$ $0.1$ $0.2$ $1 \times 10^{-2} \, M \, s^{-1}$ $0.2$ $0.2$ $2 \times 10^{-2} \, M \, s^{-1}$ $0.2$ $0.4$ $8 \times 10^{-2} \, M \, s^{-1}$ The order of reaction with respect to $A_2$ and $B$ are respectively:

Similar Questions

For a reaction $A + B \rightarrow \text{product}$,if $[A]$ is doubled keeping $[B]$ constant,the rate of reaction doubles. Calculate the order of reaction with respect to $A$.

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

For a gaseous reaction $2A + B \rightarrow C + D$,the rate of reaction is given by $Rate = K[A][B]$. If the volume of the container is reduced to $1/4$ of its original volume,what will be the ratio of the new rate to the original rate?

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 $.5$)

The rate constant of a reaction is $1.388 \times 10^{-3} \ mol^{-2} \ L^{2} \ s^{-1}$. The order of the reaction is:

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$A_2 + 2 \, B \to 2 \, AB$

$[A_2]$ $[B]$ $-d[A_2]/dt$

$0.1$ $0.2$ $1 \times 10^{-2} \, M \, s^{-1}$

$0.2$ $0.2$ $2 \times 10^{-2} \, M \, s^{-1}$

$0.2$ $0.4$ $8 \times 10^{-2} \, M \, s^{-1}$

The order of reaction with respect to $A_2$ and $B$ are respectively:

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

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

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

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

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

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

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 $.5$)