(C) The rate of the reaction is determined by the slowest step,which is Step-$2$: $r = k_2[AE][A]$.Since $AE$ is an intermediate,we express its concen

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(C) The rate of the reaction is determined by the slowest step,which is Step-$2$: $r = k_2[AE][A]$.Since $AE$ is an intermediate,we express its concentration using the equilibrium constant $K_{eq}$ from the fast Step-$1$: $K_{eq} = \frac{[AE]}{[A][E]}$,which gives $[AE] = K_{eq}[A][E]$.Substituting this into the rate expression: $r = k_2(K_{eq}[A][E])[A] = k_2 K_{eq}[A]^2[E]$.Letting $k = k_2 K_{eq}$,the rate law becomes $r = k[A]^2[E]$.

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

Medium

The hypothetical reaction : $2A + B \to C + D$ is catalyzed by $E$ as indicated in the possible mechanism below -
Step-$1$ : $A + E \rightleftharpoons AE$ (fast)
Step-$2$ : $AE + A \to A_2 + E$ (slow)
Step-$3$ : $A_2 + B \to C + D$ (fast)
What rate law best agrees with this mechanism?

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

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Class 12 Questions

Class 12

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

The given reaction $2NO + O_2 \to 2NO_2$ is an example of

MediumAIPMT 2001

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If the rate of reaction is given by $Rate = K [A]^{3/2} [B]^{-1/2}$,then find the order of the reaction.

Medium

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The reaction $N_2O_5$ (in $CCl_4$ solution) $\to 2NO_2$ (solution) $+ \frac{1}{2}O_{2(g)}$ is of first order in $N_2O_5$ with rate constant $6.2 \times 10^{-1} \, s^{-1}$. What is the value of the rate of reaction when $[N_2O_5] = 1.25 \, mol \, L^{-1}$?

Easy

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What will be the unit of the rate constant for the following reaction?
$C_2H_{4(g)} + H_{2(g)} \rightarrow C_2H_{6(g)}$

GSEB 2023

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Differential form of the rate equation is $\frac{dx}{dt} = k[P][Q]^{0.5}[R]^{0.5}$. Which statement about the above equation is wrong?

Medium

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The hypothetical reaction : $2A + B \to C + D$ is catalyzed by $E$ as indicated in the possible mechanism below -Step-$1$ : $A + E \rightleftharpoons AE$ (fast)Step-$2$ : $AE + A \to A_2 + E$ (slow)Step-$3$ : $A_2 + B \to C + D$ (fast)What rate law best agrees with this mechanism?

Similar Questions

The given reaction $2NO + O_2 \to 2NO_2$ is an example of

If the rate of reaction is given by $Rate = K [A]^{3/2} [B]^{-1/2}$,then find the order of the reaction.

The reaction $N_2O_5$ (in $CCl_4$ solution) $\to 2NO_2$ (solution) $+ \frac{1}{2}O_{2(g)}$ is of first order in $N_2O_5$ with rate constant $6.2 \times 10^{-1} \, s^{-1}$. What is the value of the rate of reaction when $[N_2O_5] = 1.25 \, mol \, L^{-1}$?

What will be the unit of the rate constant for the following reaction?$C_2H_{4(g)} + H_{2(g)} \rightarrow C_2H_{6(g)}$

Differential form of the rate equation is $\frac{dx}{dt} = k[P][Q]^{0.5}[R]^{0.5}$. Which statement about the above equation is wrong?

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The hypothetical reaction : $2A + B \to C + D$ is catalyzed by $E$ as indicated in the possible mechanism below -
Step-$1$ : $A + E \rightleftharpoons AE$ (fast)
Step-$2$ : $AE + A \to A_2 + E$ (slow)
Step-$3$ : $A_2 + B \to C + D$ (fast)
What rate law best agrees with this mechanism?

What will be the unit of the rate constant for the following reaction?
$C_2H_{4(g)} + H_{2(g)} \rightarrow C_2H_{6(g)}$