(D) The reaction $H_2 + Br_2 \rightarrow 2HBr$ follows a rate law of $Rate = k[H_2][Br_2]^{1/2}$.Thus,the order of the reaction is $1 + 0.5 = 1.5$.The

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Combination of $H_2$ and $Br_2$ to give $HBr$ $-$ Zero order reaction

(D) The reaction $H_2 + Br_2 \rightarrow 2HBr$ follows a rate law of $Rate = k[H_2][Br_2]^{1/2}$.Thus,the order of the reaction is $1 + 0.5 = 1.5$.Therefore,the statement in option $D$ is wrongly matched.

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

Medium

Which one of the following is wrongly matched?

A
Saponification of $CH_3COOC_2H_5$ $-$ Second order reaction
B
Hydrolysis of $CH_3COOCH_3$ $-$ Pseudo uni-molecular reaction
C
Decomposition of $H_2O_2$ $-$ First order reaction
D
Combination of $H_2$ and $Br_2$ to give $HBr$ $-$ Zero order reaction

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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

In the reaction sequence $A$ $\xrightarrow{K_1} B$ $\xrightarrow{K_2} C$ $\xrightarrow{K_3} D$,where $K_3 > K_2 > K_1$,which step determines the rate of the reaction?

Easy

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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 rate law equation for a reaction between $A$,$B$ and $C$ is $r = k[A][B][C]^2$. What will be the new rate of reaction if the concentration of both $A$ and $B$ are doubled (in $r$)?

MediumMHT CET 2021

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For the reaction $2A + B \rightarrow \text{Product}$,the half-life remains unchanged when the concentration of $A$ is doubled. When the concentration of $B$ is doubled,the rate of reaction increases by a factor of $2$. What is the unit of the rate constant for this reaction?

Easy

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Write the unit of the rate constant for the following reactions:
$1.$ Zero order
$2.$ Second order

Medium

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Which one of the following is wrongly matched?

Similar Questions

In the reaction sequence $A$ $\xrightarrow{K_1} B$ $\xrightarrow{K_2} C$ $\xrightarrow{K_3} D$,where $K_3 > K_2 > K_1$,which step determines the rate of the reaction?

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

The rate law equation for a reaction between $A$,$B$ and $C$ is $r = k[A][B][C]^2$. What will be the new rate of reaction if the concentration of both $A$ and $B$ are doubled (in $r$)?

For the reaction $2A + B \rightarrow \text{Product}$,the half-life remains unchanged when the concentration of $A$ is doubled. When the concentration of $B$ is doubled,the rate of reaction increases by a factor of $2$. What is the unit of the rate constant for this reaction?

Write the unit of the rate constant for the following reactions:$1.$ Zero order$2.$ Second order

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Write the unit of the rate constant for the following reactions:
$1.$ Zero order
$2.$ Second order