(D) The rate law for the reaction $2AB + B \to A_2B_3$ is given by $r = k[AB]^2[B]^1$.Let the initial moles of $AB$ and $B$ be $n$ each.In vessel $1$

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(D) The rate law for the reaction $2AB + B \to A_2B_3$ is given by $r = k[AB]^2[B]^1$.Let the initial moles of $AB$ and $B$ be $n$ each.In vessel $1$ $(V_1 = 1 \ dm^3)$,the concentrations are $[AB]_1 = n/1 = n$ and $[B]_1 = n/1 = n$.So,$r_1 = k(n)^2(n) = kn^3$.In vessel $2$ $(V_2 = 2 \ dm^3)$,the concentrations are $[AB]_2 = n/2$ and $[B]_2 = n/2$.So,$r_2 = k(n/2)^2(n/2) = k(n^3/8) = kn^3/8$.The ratio $r_1/r_2 = (kn^3) / (kn^3/8) = 8/1$ or $8 : 1$.

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

Medium

The initial reaction $2AB + B \to A_2B_3$ is carried out in vessels of volume $1 \ dm^3$ and $2 \ dm^3$ respectively,using equal moles of reactants. The ratio of the reaction rates $(r_1/r_2)$ is:

A
$1 : 8$
B
$4 : 7$
C
$4 : 1$
D
$8 : 1$

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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

The following are the rate constants of two different reactions. Determine the overall order of reaction for each case:
$(a)$ $6.66 \times 10^{-3} \, s^{-1}$
$(b)$ $4.5 \times 10^{-2} \, mol^{-1} \, L \, s^{-1}$

Medium

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$A$ chemical reaction takes place in two steps as follows:
$(i) \ NO_2Cl_{(g)} \xrightarrow{K_1} NO_{2(g)} + Cl_{(g)}$
$(ii) \ NO_2Cl_{(g)} + Cl_{(g)} \xrightarrow{K_2} NO_{2(g)} + Cl_{2(g)}$
Identify the reaction intermediate.

MediumMHT CET 2016

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Write the equation for a pseudo first order reaction. Write the rate law and the rate constant.

Easy

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In a reaction between $A$ and $B$,the initial rate of reaction $(r_0)$ was measured for different initial concentrations of $A$ and $B$ as given below:

$A / mol \ L^{-1}$ $0.20$ $0.20$ $0.40$

$B / mol \ L^{-1}$ $0.30$ $0.10$ $0.05$

$r_0 / mol \ L^{-1} \ s^{-1}$ $5.07 \times 10^{-5}$ $5.07 \times 10^{-5}$ $1.43 \times 10^{-4}$

What is the order of the reaction with respect to $A$ and $B$?

Difficult

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With the help of an example,explain what is meant by a pseudo first order reaction.

Medium

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$A / mol \ L^{-1}$	$0.20$	$0.20$	$0.40$
$B / mol \ L^{-1}$	$0.30$	$0.10$	$0.05$
$r_0 / mol \ L^{-1} \ s^{-1}$	$5.07 \times 10^{-5}$	$5.07 \times 10^{-5}$	$1.43 \times 10^{-4}$

The initial reaction $2AB + B \to A_2B_3$ is carried out in vessels of volume $1 \ dm^3$ and $2 \ dm^3$ respectively,using equal moles of reactants. The ratio of the reaction rates $(r_1/r_2)$ is:

Similar Questions

The following are the rate constants of two different reactions. Determine the overall order of reaction for each case:$(a)$ $6.66 \times 10^{-3} \, s^{-1}$$(b)$ $4.5 \times 10^{-2} \, mol^{-1} \, L \, s^{-1}$

$A$ chemical reaction takes place in two steps as follows:$(i) \ NO_2Cl_{(g)} \xrightarrow{K_1} NO_{2(g)} + Cl_{(g)}$$(ii) \ NO_2Cl_{(g)} + Cl_{(g)} \xrightarrow{K_2} NO_{2(g)} + Cl_{2(g)}$Identify the reaction intermediate.

Write the equation for a pseudo first order reaction. Write the rate law and the rate constant.

With the help of an example,explain what is meant by a pseudo first order reaction.

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The following are the rate constants of two different reactions. Determine the overall order of reaction for each case:
$(a)$ $6.66 \times 10^{-3} \, s^{-1}$
$(b)$ $4.5 \times 10^{-2} \, mol^{-1} \, L \, s^{-1}$

$A$ chemical reaction takes place in two steps as follows:
$(i) \ NO_2Cl_{(g)} \xrightarrow{K_1} NO_{2(g)} + Cl_{(g)}$
$(ii) \ NO_2Cl_{(g)} + Cl_{(g)} \xrightarrow{K_2} NO_{2(g)} + Cl_{2(g)}$
Identify the reaction intermediate.