(C) The rate of the reaction is determined by the slow step:$r = k[A][B_2]$From the fast equilibrium step,$A_2 \rightleftharpoons A + A$,the equilibri

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(C) The rate of the reaction is determined by the slow step:$r = k[A][B_2]$From the fast equilibrium step,$A_2 \rightleftharpoons A + A$,the equilibrium constant $K_{eq}$ is:$K_{eq} = \frac{[A]^2}{[A_2]}$Therefore,$[A] = K_{eq}^{1/2} [A_2]^{1/2}$Substituting this into the rate law:$r = k \times K_{eq}^{1/2} [A_2]^{1/2} [B_2]^1$The overall order of the reaction is the sum of the exponents of the concentration terms:Order $= 0.5 + 1 = 1.5$ or $1\frac{1}{2}$.

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

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The hypothetical reaction $A_2 + B_2 \rightarrow 2AB$ follows the mechanism given below. What is the overall order of the reaction?
$A_2 \rightleftharpoons A + A$ ...... (fast);
$A + B_2 \rightarrow AB + B$ ...... (slow);
$A + B \rightarrow AB$ ...... (fast)

A
$2$
B
$1$
C
$1.5$
D
$0$

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Class 12

Chemistry Questions

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

What is rate law? Give a relation between rate of reaction and concentration of reactants.

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For a reaction scheme $A$ $\xrightarrow{k_1} B$ $\xrightarrow{k_2} C$,if the rate of formation of $B$ is set to be zero,then the concentration of $B$ is given by:

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If the value of the rate constant $K = 2.3 \times 10^{-5} \ L \ mol^{-1} \ s^{-1}$,then identify the reaction order:

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For a reaction,$A + 2B \longrightarrow C$,the rate is given by $+\frac{d[C]}{dt} = k[A][B]$. Hence,the order of the reaction is:

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For the chemical reaction $2O_3 \rightarrow 3O_2$,the mechanism is given below. What will be the rate law expression?
$O_3 \rightleftharpoons O_2 + O$ ...... (fast)
$O + O_3 \rightarrow 2O_2$ ...... (slow)

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The hypothetical reaction $A_2 + B_2 \rightarrow 2AB$ follows the mechanism given below. What is the overall order of the reaction?$A_2 \rightleftharpoons A + A$ ...... (fast);$A + B_2 \rightarrow AB + B$ ...... (slow);$A + B \rightarrow AB$ ...... (fast)

Similar Questions

What is rate law? Give a relation between rate of reaction and concentration of reactants.

For a reaction scheme $A$ $\xrightarrow{k_1} B$ $\xrightarrow{k_2} C$,if the rate of formation of $B$ is set to be zero,then the concentration of $B$ is given by:

If the value of the rate constant $K = 2.3 \times 10^{-5} \ L \ mol^{-1} \ s^{-1}$,then identify the reaction order:

For a reaction,$A + 2B \longrightarrow C$,the rate is given by $+\frac{d[C]}{dt} = k[A][B]$. Hence,the order of the reaction is:

For the chemical reaction $2O_3 \rightarrow 3O_2$,the mechanism is given below. What will be the rate law expression?$O_3 \rightleftharpoons O_2 + O$ ...... (fast)$O + O_3 \rightarrow 2O_2$ ...... (slow)

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The hypothetical reaction $A_2 + B_2 \rightarrow 2AB$ follows the mechanism given below. What is the overall order of the reaction?
$A_2 \rightleftharpoons A + A$ ...... (fast);
$A + B_2 \rightarrow AB + B$ ...... (slow);
$A + B \rightarrow AB$ ...... (fast)

For the chemical reaction $2O_3 \rightarrow 3O_2$,the mechanism is given below. What will be the rate law expression?
$O_3 \rightleftharpoons O_2 + O$ ...... (fast)
$O + O_3 \rightarrow 2O_2$ ...... (slow)