(D) Let the order of reaction with respect to $A$ and $B$ be $m$ and $n$ respectively.Then,$rate = k[A]^{m}[B]^{n}$From the table:$2 = k[0.2]^{m}[0.2]

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(D) Let the order of reaction with respect to $A$ and $B$ be $m$ and $n$ respectively.Then,$rate = k[A]^{m}[B]^{n}$From the table:$2 = k[0.2]^{m}[0.2]^{n}$ $(i)$$4 = k[0.2]^{m}[0.4]^{n}$ $(ii)$$36 = k[0.6]^{m}[0.4]^{n}$ $(iii)$On comparing Eqs. $(i)$ and $(ii)$:$\frac{4}{2} = \frac{k[0.2]^{m}[0.4]^{n}}{k[0.2]^{m}[0.2]^{n}}$$2 = (\frac{0.4}{0.2})^{n} = 2^{n}$$n = 1$On comparing Eqs. $(ii)$ and $(iii)$:$\frac{36}{4} = \frac{k[0.6]^{m}[0.4]^{n}}{k[0.2]^{m}[0.4]^{n}}$$9 = (\frac{0.6}{0.2})^{m} = 3^{m}$$3^{2} = 3^{m}$$m = 2$Therefore,the rate law is $r = k[A]^{2}[B]$.

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

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For a reaction,$A + B \rightarrow$ products,the rate of the reaction at various concentrations is given below. The rate law for the above reaction is:
Expt. no. $[A]$ $[B]$ Rate $(\text{mol} \ \text{dm}^{-3} \ \text{s}^{-1})$
$1$ $0.2$ $0.2$ $2$
$2$ $0.2$ $0.4$ $4$
$3$ $0.6$ $0.4$ $36$

Expt. no.	$[A]$	$[B]$	Rate $(\text{mol} \ \text{dm}^{-3} \ \text{s}^{-1})$
$1$	$0.2$	$0.2$	$2$
$2$	$0.2$	$0.4$	$4$
$3$	$0.6$	$0.4$	$36$

KCET 2012 All KCET

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

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Class 12

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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KCET 2012 Paper All KCET years →

Reaction : $2Br^{-} + H_2O_2 + 2H^{+} \to Br_2 + 2H_2O$
takes place in two steps :
$(a)$ $Br^{-} + H^{+} + H_2O_2 \xrightarrow{slow} HOBr + H_2O$
$(b)$ $HOBr + Br^{-} + H^{+} \xrightarrow{fast} H_2O + Br_2$
The order of the reaction is

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Consider the gaseous reaction $A_2 + B_2 \rightarrow 2 AB$. The following data was obtained for the above reaction:
$[A_2]_0$ $[B_2]_0$ Initial rate of formation of $AB$ $(mol \ L^{-1} s^{-1})$
$0.1 \ M$ $0.1 \ M$ $2.5 \times 10^{-4}$
$0.2 \ M$ $0.1 \ M$ $5.0 \times 10^{-4}$
$0.2 \ M$ $0.2 \ M$ $1.0 \times 10^{-3}$

The value of the rate constant for the above reaction is:

DifficultTS EAMCET 2024

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For a reaction whose rate expression is: Rate $= k[A]^{1/2}[B]^{3/2}$,the order would be

Medium

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$A_{(g)} + 2B_{(g)} \to$ product is an elementary reaction. Which of the following is incorrect?

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The numerical values of rate constants are same for first,second and third order reactions. Which one is true at a moment for rate of these three reactions if concentration of reactants is same and lesser than $1 \ M$?

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$[A_2]_0$	$[B_2]_0$	Initial rate of formation of $AB$ $(mol \ L^{-1} s^{-1})$
$0.1 \ M$	$0.1 \ M$	$2.5 \times 10^{-4}$
$0.2 \ M$	$0.1 \ M$	$5.0 \times 10^{-4}$
$0.2 \ M$	$0.2 \ M$	$1.0 \times 10^{-3}$

For a reaction,$A + B \rightarrow$ products,the rate of the reaction at various concentrations is given below. The rate law for the above reaction is:Expt. no.$[A]$$[B]$Rate $(\text{mol} \ \text{dm}^{-3} \ \text{s}^{-1})$$1$$0.2$$0.2$$2$$2$$0.2$$0.4$$4$$3$$0.6$$0.4$$36$

Similar Questions

Reaction : $2Br^{-} + H_2O_2 + 2H^{+} \to Br_2 + 2H_2O$takes place in two steps :$(a)$ $Br^{-} + H^{+} + H_2O_2 \xrightarrow{slow} HOBr + H_2O$$(b)$ $HOBr + Br^{-} + H^{+} \xrightarrow{fast} H_2O + Br_2$The order of the reaction is

For a reaction whose rate expression is: Rate $= k[A]^{1/2}[B]^{3/2}$,the order would be

$A_{(g)} + 2B_{(g)} \to$ product is an elementary reaction. Which of the following is incorrect?

The numerical values of rate constants are same for first,second and third order reactions. Which one is true at a moment for rate of these three reactions if concentration of reactants is same and lesser than $1 \ M$?

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For a reaction,$A + B \rightarrow$ products,the rate of the reaction at various concentrations is given below. The rate law for the above reaction is:
Expt. no. $[A]$ $[B]$ Rate $(\text{mol} \ \text{dm}^{-3} \ \text{s}^{-1})$
$1$ $0.2$ $0.2$ $2$
$2$ $0.2$ $0.4$ $4$
$3$ $0.6$ $0.4$ $36$

Reaction : $2Br^{-} + H_2O_2 + 2H^{+} \to Br_2 + 2H_2O$
takes place in two steps :
$(a)$ $Br^{-} + H^{+} + H_2O_2 \xrightarrow{slow} HOBr + H_2O$
$(b)$ $HOBr + Br^{-} + H^{+} \xrightarrow{fast} H_2O + Br_2$
The order of the reaction is