(B) The rate of the reaction is determined by the slow step: $r = K_2 [I]^2 [H_2]$. Since $I$ is an intermediate,we use the equilibrium step to expre

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$r = K_2 \frac{K_1}{K_{-1}} [H_2] [I_2]$

(B) The rate of the reaction is determined by the slow step: $r = K_2 [I]^2 [H_2]$. Since $I$ is an intermediate,we use the equilibrium step to express its concentration. For the fast equilibrium step: $K_{eq} = \frac{K_1}{K_{-1}} = \frac{[I]^2}{[I_2]}$. Therefore,$[I]^2 = \frac{K_1}{K_{-1}} [I_2]$. Substituting this into the rate expression: $r = K_2 (\frac{K_1}{K_{-1}} [I_2]) [H_2]$. Thus,$r = K_2 \frac{K_1}{K_{-1}} [H_2] [I_2]$.

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

Medium

For the reaction ${H_{2(g)} + I_{2(g)} \to 2HI_{(g)}}$,the possible mechanism is given below:
$I_2 \underset{k_{-1}}{\stackrel{k_1}{\rightleftharpoons}} 2 I$ (fast step)
${2I + H_2 \xrightarrow{K_2} 2HI}$ (slow step)
Determine the rate law for the reaction.

A
$r = K_2 K_1 [H_2] [I_2]$
B
$r = K_2 \frac{K_1}{K_{-1}} [H_2] [I_2]$
C
$r = K_2 \sqrt{\frac{K_1}{K_{-1}}} [H_2] [I_2]$
D
$r = K_2 \frac{K_1}{K_{-1}} [H_2] [I_2]^2$

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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 rate constant of the reaction,$2 H_2O_2 \rightarrow 2 H_2O + O_2$ is $3 \times 10^{-3} \ min^{-1}$. At what concentration of $H_2O_2$ will the rate of reaction be $2 \times 10^{-4} \ M \ s^{-1}$?

Medium

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The given data are for the reaction:
$2NO_{(g)} + Cl_{2(g)} \to 2NOCl_{(g)}$ at $298 \ K$
Experiment $[Cl_2] \ (M)$ $[NO] \ (M)$ Rate $(mol \ L^{-1} \sec^{-1})$
$I$ $0.05$ $0.05$ $1 \times 10^{-3}$
$II$ $0.15$ $0.05$ $3 \times 10^{-3}$
$III$ $0.05$ $0.15$ $9 \times 10^{-3}$

The rate law for the reaction is:

Medium

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Write the general reaction,its differential rate equation,and the rate law.

Difficult

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Which of the following is an elementary reaction?

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The reaction $2NO + O_2 \rightarrow 2NO_2$ is an example of which order of reaction?

Easy

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Experiment	$[Cl_2] \ (M)$	$[NO] \ (M)$	Rate $(mol \ L^{-1} \sec^{-1})$
$I$	$0.05$	$0.05$	$1 \times 10^{-3}$
$II$	$0.15$	$0.05$	$3 \times 10^{-3}$
$III$	$0.05$	$0.15$	$9 \times 10^{-3}$

For the reaction ${H_{2(g)} + I_{2(g)} \to 2HI_{(g)}}$,the possible mechanism is given below: $I_2 \underset{k_{-1}}{\stackrel{k_1}{\rightleftharpoons}} 2 I$ (fast step) ${2I + H_2 \xrightarrow{K_2} 2HI}$ (slow step) Determine the rate law for the reaction.

Similar Questions

The rate constant of the reaction,$2 H_2O_2 \rightarrow 2 H_2O + O_2$ is $3 \times 10^{-3} \ min^{-1}$. At what concentration of $H_2O_2$ will the rate of reaction be $2 \times 10^{-4} \ M \ s^{-1}$?

The given data are for the reaction:$2NO_{(g)} + Cl_{2(g)} \to 2NOCl_{(g)}$ at $298 \ K$Experiment$[Cl_2] \ (M)$$[NO] \ (M)$Rate $(mol \ L^{-1} \sec^{-1})$$I$$0.05$$0.05$$1 \times 10^{-3}$$II$$0.15$$0.05$$3 \times 10^{-3}$$III$$0.05$$0.15$$9 \times 10^{-3}$The rate law for the reaction is:

Write the general reaction,its differential rate equation,and the rate law.

Which of the following is an elementary reaction?

The reaction $2NO + O_2 \rightarrow 2NO_2$ is an example of which order of reaction?

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For the reaction ${H_{2(g)} + I_{2(g)} \to 2HI_{(g)}}$,the possible mechanism is given below:
$I_2 \underset{k_{-1}}{\stackrel{k_1}{\rightleftharpoons}} 2 I$ (fast step)
${2I + H_2 \xrightarrow{K_2} 2HI}$ (slow step)
Determine the rate law for the reaction.