(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

The rate constant of the reaction,$2 H_2O_2 \rightarrow 2 H_2O + O_2$ is $3 \times 10^{-3} \ min^{-1}$. At what concentration of $H_2O_2$ will the rate of reaction be $2 \times 10^{-4} \ M \ s^{-1}$?

Medium

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The data for the reaction $A + B \to C$ is given below. The rate law corresponding to the above data is:

$Exp.$ $[A]_0$ $[B]_0$ Initial rate

$(1)$ $0.012$ $0.035$ $0.10$

$(2)$ $0.024$ $0.070$ $0.80$

$(3)$ $0.024$ $0.035$ $0.10$

$(4)$ $0.012$ $0.070$ $0.80$

$Exp.$	$[A]_0$	$[B]_0$	Initial rate
$(1)$	$0.012$	$0.035$	$0.10$
$(2)$	$0.024$	$0.070$	$0.80$
$(3)$	$0.024$	$0.035$	$0.10$
$(4)$	$0.012$	$0.070$	$0.80$

MediumAIPMT 1994

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Calculate the order of the reaction with respect to $A$ and $B$ based on the following data:

$[A] \ (mol/L)$ $[B] \ (mol/L)$ Rate $(mol/L \cdot s)$

$0.05$ $0.05$ $1.2 \times 10^{-3}$

$0.10$ $0.05$ $2.4 \times 10^{-3}$

$0.05$ $0.10$ $1.2 \times 10^{-3}$

Easy

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If the concentration of reactant $B$ is doubled,the rate of the reaction between reactants $A$ and $B$ becomes $1/4$ of the initial rate. The order of the reaction with respect to reactant $B$ is ......

Medium

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........ of a reaction cannot be determined experimentally.

EasyAP EAMCET 2021

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$[A] \ (mol/L)$	$[B] \ (mol/L)$	Rate $(mol/L \cdot s)$
$0.05$	$0.05$	$1.2 \times 10^{-3}$
$0.10$	$0.05$	$2.4 \times 10^{-3}$
$0.05$	$0.10$	$1.2 \times 10^{-3}$

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

The rate constant of the reaction,$2 H_2O_2 \rightarrow 2 H_2O + O_2$ is $3 \times 10^{-3} \ min^{-1}$. At what concentration of $H_2O_2$ will the rate of reaction be $2 \times 10^{-4} \ M \ s^{-1}$?

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

Calculate the order of the reaction with respect to $A$ and $B$ based on the following data: $[A] \ (mol/L)$ $[B] \ (mol/L)$ Rate $(mol/L \cdot s)$ $0.05$ $0.05$ $1.2 \times 10^{-3}$ $0.10$ $0.05$ $2.4 \times 10^{-3}$ $0.05$ $0.10$ $1.2 \times 10^{-3}$

If the concentration of reactant $B$ is doubled,the rate of the reaction between reactants $A$ and $B$ becomes $1/4$ of the initial rate. The order of the reaction with respect to reactant $B$ is ......

........ of a reaction cannot be determined experimentally.

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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.

The data for the reaction $A + B \to C$ is given below. The rate law corresponding to the above data is:

$Exp.$ $[A]_0$ $[B]_0$ Initial rate

$(1)$ $0.012$ $0.035$ $0.10$

$(2)$ $0.024$ $0.070$ $0.80$

$(3)$ $0.024$ $0.035$ $0.10$

$(4)$ $0.012$ $0.070$ $0.80$

Calculate the order of the reaction with respect to $A$ and $B$ based on the following data:

$[A] \ (mol/L)$ $[B] \ (mol/L)$ Rate $(mol/L \cdot s)$

$0.05$ $0.05$ $1.2 \times 10^{-3}$

$0.10$ $0.05$ $2.4 \times 10^{-3}$

$0.05$ $0.10$ $1.2 \times 10^{-3}$