(C) Let the rate law be $r = k[A]^x[B]^y$.From experiment $1$ and $2$,$[B]$ is constant. Comparing the rates:$\frac{8.4 \times 10^{-6}}{4.2 \times 10^

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(C) Let the rate law be $r = k[A]^x[B]^y$.From experiment $1$ and $2$,$[B]$ is constant. Comparing the rates:$\frac{8.4 \times 10^{-6}}{4.2 \times 10^{-6}} = (\frac{2.0}{1.0})^x \implies 2 = 2^x \implies x = 1$.From experiment $1$ and $3$,$[A]$ is constant. Comparing the rates:$\frac{5.6 \times 10^{-6}}{4.2 \times 10^{-6}} = (\frac{0.20}{0.15})^y \implies \frac{4}{3} = (\frac{4}{3})^y \implies y = 1$.Thus,the rate law is $r = k[A]^1[B]^1$ or $r = k[A][B]$.

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

Medium

$A$ study of chemical kinetics of the reaction $A + B \to$ Products,gave the following data at $25 \ ^oC$.

$Exp. \ No.$ $[A]$ $[B]$ $Rate$

$1.$ $1.0$ $0.15$ $4.2 \times 10^{-6}$

$2.$ $2.0$ $0.15$ $8.4 \times 10^{-6}$

$3.$ $1.0$ $0.20$ $5.6 \times 10^{-6}$

Find out the rate law.

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

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Class 12 Questions

Class 12

Chemistry Questions

Chapter

Chemical Kinetics

Subtopic

Rate law , Rate constant , Order of Reaction and Molecularity

For a zero order reaction,will the molecularity be equal to zero? Explain.

Easy

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For the reaction $2A + B \rightarrow C + D$,select the correct rate law based on the following data:
$1$. $[A] = 0.1, [B] = 0.1, \text{Initial Rate} = 7.5 \times 10^{-3}$
$2$. $[A] = 0.3, [B] = 0.2, \text{Initial Rate} = 9.0 \times 10^{-2}$
$3$. $[A] = 0.3, [B] = 0.4, \text{Initial Rate} = 3.6 \times 10^{-1}$
$4$. $[A] = 0.4, [B] = 0.1, \text{Initial Rate} = 3.0 \times 10^{-2}$

Easy

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If the relation between half-life time $(t_{1/2})$ and initial concentration $[R]_0$ is given by $t_{1/2} \propto \frac{1}{[R]_0^{n-1}}$,what is the order of the reaction?

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The data for the reaction $A + B \to C$ is given below. 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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The rate law for the reaction between substances $A$ and $B$ is given by $\text{Rate} = k[A]^n[B]^m$. If the concentration of $A$ is doubled and the concentration of $B$ is halved,what is the ratio of the new rate to the initial rate?

Easy

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$Exp. \ No.$	$[A]$	$[B]$	$Rate$
$1.$	$1.0$	$0.15$	$4.2 \times 10^{-6}$
$2.$	$2.0$	$0.15$	$8.4 \times 10^{-6}$
$3.$	$1.0$	$0.20$	$5.6 \times 10^{-6}$

$A$ study of chemical kinetics of the reaction $A + B \to$ Products,gave the following data at $25 \ ^oC$. $Exp. \ No.$ $[A]$ $[B]$ $Rate$ $1.$ $1.0$ $0.15$ $4.2 \times 10^{-6}$ $2.$ $2.0$ $0.15$ $8.4 \times 10^{-6}$ $3.$ $1.0$ $0.20$ $5.6 \times 10^{-6}$ Find out the rate law.

Similar Questions

For a zero order reaction,will the molecularity be equal to zero? Explain.

If the relation between half-life time $(t_{1/2})$ and initial concentration $[R]_0$ is given by $t_{1/2} \propto \frac{1}{[R]_0^{n-1}}$,what is the order of 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 $(1)$ $0.012$ $0.035$ $0.10$ $(2)$ $0.024$ $0.070$ $0.80$ $(3)$ $0.024$ $0.035$ $0.10$ $(4)$ $0.012$ $0.070$ $0.80$

The rate law for the reaction between substances $A$ and $B$ is given by $\text{Rate} = k[A]^n[B]^m$. If the concentration of $A$ is doubled and the concentration of $B$ is halved,what is the ratio of the new rate to the initial rate?

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$A$ study of chemical kinetics of the reaction $A + B \to$ Products,gave the following data at $25 \ ^oC$.

$Exp. \ No.$ $[A]$ $[B]$ $Rate$

$1.$ $1.0$ $0.15$ $4.2 \times 10^{-6}$

$2.$ $2.0$ $0.15$ $8.4 \times 10^{-6}$

$3.$ $1.0$ $0.20$ $5.6 \times 10^{-6}$

Find out the rate law.

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

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

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

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

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