(B) The rate law for the reaction $H_{2(g)} + I_{2(g)} \longrightarrow 2 HI_{(g)}$ is given by $Rate = k[H_2][I_2]$.Since the sum of the powers of the

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$H_{2(g)} + I_{2(g)} \longrightarrow 2 HI_{(g)}$

(B) The rate law for the reaction $H_{2(g)} + I_{2(g)} \longrightarrow 2 HI_{(g)}$ is given by $Rate = k[H_2][I_2]$.Since the sum of the powers of the concentration terms in the rate law is $1 + 1 = 2$,this reaction is a second-order reaction.Option $B$ is the correct answer.

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

Medium

Which of the following is an example of a second-order reaction?

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A
$2 H_2 O_{2(g)} \longrightarrow 2 H_2 O_{(l)} + O_{2(g)}$
B
$H_{2(g)} + I_{2(g)} \longrightarrow 2 HI_{(g)}$
C
$CH_3 CHO_{(g)} \longrightarrow CH_{4(g)} + CO_{(g)}$
D
$2 NO_{(g)} + 2 H_{2(g)} \longrightarrow N_{2(g)} + 2 H_2 O_{(g)}$

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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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The rate constant for the reaction $A \longrightarrow B$ is $2 \times 10^{-4} \ L \ mol^{-1} \ min^{-1}$. The concentration of $A$ at which the rate of the reaction is $(1 / 12) \times 10^{-5} \ M \ sec^{-1}$ is :-

Medium

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In the reaction $A + B \to \text{Products}$,the initial concentration of both $A$ and $B$ is $0.1 \, M$. When the concentration decreases to $1.0 \times 10^{-2} \, M$,the half-life period increases by ten times. The rate of the reaction is:

Medium

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From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant: $(iv) \ C_{2}H_{5}Cl_{(g)} \rightarrow C_{2}H_{4(g)} + HCl_{(g)} \quad \text{Rate} = k[C_{2}H_{5}Cl]$

Medium

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The rate law for the reaction $\text{Sucrose} + \text{Water} \xrightarrow{H^+} \text{Glucose} + \text{Fructose}$ is given by:

Easy

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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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Which of the following is an example of a second-order reaction?

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The rate constant for the reaction $A \longrightarrow B$ is $2 \times 10^{-4} \ L \ mol^{-1} \ min^{-1}$. The concentration of $A$ at which the rate of the reaction is $(1 / 12) \times 10^{-5} \ M \ sec^{-1}$ is :-

In the reaction $A + B \to \text{Products}$,the initial concentration of both $A$ and $B$ is $0.1 \, M$. When the concentration decreases to $1.0 \times 10^{-2} \, M$,the half-life period increases by ten times. The rate of the reaction is:

From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant: $(iv) \ C_{2}H_{5}Cl_{(g)} \rightarrow C_{2}H_{4(g)} + HCl_{(g)} \quad \text{Rate} = k[C_{2}H_{5}Cl]$

The rate law for the reaction $\text{Sucrose} + \text{Water} \xrightarrow{H^+} \text{Glucose} + \text{Fructose}$ is given by:

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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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