(B) Given rate of reaction $r = 3.6 \times 10^{-2} \ mol \ dm^{-3} \ s^{-1}$.Rate law is $r = k[A][B]^2$.Given concentrations are $[A] = 0.2 \ M$ and

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$18 \ mol^{-2} \ dm^6 \ s^{-1}$

(B) Given rate of reaction $r = 3.6 \times 10^{-2} \ mol \ dm^{-3} \ s^{-1}$.Rate law is $r = k[A][B]^2$.Given concentrations are $[A] = 0.2 \ M$ and $[B] = 0.1 \ M$.Substituting the values in the rate law:$3.6 \times 10^{-2} = k \times (0.2) \times (0.1)^2$$3.6 \times 10^{-2} = k \times (0.2) \times (0.01)$$3.6 \times 10^{-2} = k \times (0.002)$$k = \frac{3.6 \times 10^{-2}}{2 \times 10^{-3}}$$k = 1.8 \times 10^1 = 18 \ mol^{-2} \ dm^6 \ s^{-1}$.Thus,the correct option is $B$.

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

Easy

Rate of the reaction $A + B \rightarrow \text{product}$ is $3.6 \times 10^{-2} \ mol \ dm^{-3} \ s^{-1}$ and rate law is $r = k[A][B]^2$. What is the rate constant of the reaction if $[A] = 0.2 \ M$ and $[B] = 0.1 \ M$?

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A
$10 \ mol^{-2} \ dm^6 \ s^{-1}$
B
$18 \ mol^{-2} \ dm^6 \ s^{-1}$
C
$24 \ mol^{-2} \ dm^6 \ s^{-1}$
D
$4.8 \ mol^{-2} \ dm^6 \ s^{-1}$

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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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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The rate law for the reaction $A^{+} + B^{+} + C \longrightarrow \text{Product}$ is expressed as $\text{Rate} = k[A]^{2}[B]^{1}[C]^{0}$. What is the overall order of the reaction?

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The data for the reaction $A + B \to C$ is given below:

$Exp$ $[A]_0$ $[B]_0$ Initial Rate

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

$2$ $0.024$ $0.035$ $0.80$

$3$ $0.012$ $0.070$ $0.10$

$4$ $0.024$ $0.070$ $0.80$

Determine the rate law for the reaction.

$Exp$	$[A]_0$	$[B]_0$	Initial Rate
$1$	$0.012$	$0.035$	$0.10$
$2$	$0.024$	$0.035$	$0.80$
$3$	$0.012$	$0.070$	$0.10$
$4$	$0.024$	$0.070$	$0.80$

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For a certain reaction,the expression for half-life is $t_{1/2} \propto \frac{1}{a^{n-1}}$. What is the order of the reaction?

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The reaction $3ClO^{-} \rightarrow ClO_{3}^{-} + 2Cl^{-}$ occurs in the following two steps:
$(i)$ $ClO^{-} + ClO^{-} \xrightarrow{K_{1}} ClO_{2}^{-} + Cl^{-}$ (Slow step)
$(ii)$ $ClO_{2}^{-} + ClO^{-} \xrightarrow{K_{2}} ClO_{3}^{-} + Cl^{-}$ (Fast step)
Then the rate of the given reaction is equal to . . . . . . .

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Rate of the reaction $A + B \rightarrow \text{product}$ is $3.6 \times 10^{-2} \ mol \ dm^{-3} \ s^{-1}$ and rate law is $r = k[A][B]^2$. What is the rate constant of the reaction if $[A] = 0.2 \ M$ and $[B] = 0.1 \ M$?

Similar Questions

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

The rate law for the reaction $A^{+} + B^{+} + C \longrightarrow \text{Product}$ is expressed as $\text{Rate} = k[A]^{2}[B]^{1}[C]^{0}$. What is the overall order of the reaction?

The data for the reaction $A + B \to C$ is given below: $Exp$ $[A]_0$ $[B]_0$ Initial Rate $1$ $0.012$ $0.035$ $0.10$ $2$ $0.024$ $0.035$ $0.80$ $3$ $0.012$ $0.070$ $0.10$ $4$ $0.024$ $0.070$ $0.80$ Determine the rate law for the reaction.

For a certain reaction,the expression for half-life is $t_{1/2} \propto \frac{1}{a^{n-1}}$. What is the order of the reaction?

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The data for the reaction $A + B \to C$ is given below:

$Exp$ $[A]_0$ $[B]_0$ Initial Rate

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

$2$ $0.024$ $0.035$ $0.80$

$3$ $0.012$ $0.070$ $0.10$

$4$ $0.024$ $0.070$ $0.80$

Determine the rate law for the reaction.