(B) Let the rate law be $r = k [A]^x [B]^y$.Comparing $Exp$ $1$ and $Exp$ $2$ (where $[B]_0$ is constant):$\frac{r_2}{r_1} = \frac{k [A]_2^x [B]_2^y}{

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(B) Let the rate law be $r = k [A]^x [B]^y$.Comparing $Exp$ $1$ and $Exp$ $2$ (where $[B]_0$ is constant):$\frac{r_2}{r_1} = \frac{k [A]_2^x [B]_2^y}{k [A]_1^x [B]_1^y} \implies \frac{0.80}{0.10} = (\frac{0.024}{0.012})^x$$8 = (2)^x \implies x = 3$.Comparing $Exp$ $1$ and $Exp$ $3$ (where $[A]_0$ is constant):$\frac{r_3}{r_1} = \frac{k [A]_3^x [B]_3^y}{k [A]_1^x [B]_1^y} \implies \frac{0.10}{0.10} = (\frac{0.070}{0.035})^y$$1 = (2)^y \implies y = 0$.Thus,the rate law is $r = k [A]^3$.

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

Difficult

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
$1$	$0.012$	$0.035$	$0.10$
$2$	$0.024$	$0.035$	$0.80$
$3$	$0.012$	$0.070$	$0.10$
$4$	$0.024$	$0.070$	$0.80$

A
$r = k [B]^3$
B
$r = k [A]^3$
C
$r = k [A] [B]^4$
D
$r = k [A]^2 [B]^2$

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Class 12 Questions

Class 12

Chemistry Questions

Chapter

Chemical Kinetics

Subtopic

Rate law , Rate constant , Order of Reaction and Molecularity

Which of the following statements regarding the molecularity of a reaction is wrong?

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The following data is given for the reaction between $A$ and $B$:
$S.NO.$ $[A] \ mol \ L^{-1}$ $[B] \ mol \ L^{-1}$ $Rate \ mol \ L^{-1} \ sec^{-1}$
$I$ $1 \times 10^{-2}$ $2 \times 10^{-2}$ $2 \times 10^{-4}$
$II$ $2 \times 10^{-2}$ $2 \times 10^{-2}$ $4 \times 10^{-4}$
$III$ $2 \times 10^{-2}$ $4 \times 10^{-2}$ $8 \times 10^{-4}$

Which of the following are correct statements?
$(a)$ Rate constant of the reaction is $1 \ mol^{-1} \ L \ sec^{-1}$.
$(b)$ Rate law of the reaction is $k[A][B]$.
$(c)$ Rate of reaction increases four times on doubling the concentration of both the reactants.

Difficult

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

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The rate of reaction is determined by the slow step of the reaction. This step is called:

Easy

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For three reactions of first,second,and third order,the rate constants are numerically equal. If the concentration of the reactant is the same and greater than $1 \ M$,which of the following is true for the rates of these three reactions?

Medium

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$S.NO.$	$[A] \ mol \ L^{-1}$	$[B] \ mol \ L^{-1}$	$Rate \ mol \ L^{-1} \ sec^{-1}$
$I$	$1 \times 10^{-2}$	$2 \times 10^{-2}$	$2 \times 10^{-4}$
$II$	$2 \times 10^{-2}$	$2 \times 10^{-2}$	$4 \times 10^{-4}$
$III$	$2 \times 10^{-2}$	$4 \times 10^{-2}$	$8 \times 10^{-4}$

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.

Similar Questions

Which of the following statements regarding the molecularity of a reaction is wrong?

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

The rate of reaction is determined by the slow step of the reaction. This step is called:

For three reactions of first,second,and third order,the rate constants are numerically equal. If the concentration of the reactant is the same and greater than $1 \ M$,which of the following is true for the rates of these three reactions?

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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.