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

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Why can’t molecularity of any reaction be equal to zero?

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(N/A) Molecularity is defined as the number of reacting species (atoms,ions,or molecules) taking part in an elementary reaction,which must collide in order to bring about a chemical reaction. Since a chemical reaction cannot occur without the participation of at least one reactant molecule,the minimum value for molecularity is $1$. Therefore,molecularity cannot be zero.

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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

For a certain reaction,the expression for half-life is $t_{1/2} \propto \frac{1}{a^{n-1}}$. What is the order of the reaction?

Medium

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$A_2 + 2 \, B \to 2 \, AB$

$[A_2]$ $[B]$ $-d[A_2]/dt$

$0.1$ $0.2$ $1 \times 10^{-2} \, M \, s^{-1}$

$0.2$ $0.2$ $2 \times 10^{-2} \, M \, s^{-1}$

$0.2$ $0.4$ $8 \times 10^{-2} \, M \, s^{-1}$

The order of reaction with respect to $A_2$ and $B$ are respectively:

$[A_2]$	$[B]$	$-d[A_2]/dt$
$0.1$	$0.2$	$1 \times 10^{-2} \, M \, s^{-1}$
$0.2$	$0.2$	$2 \times 10^{-2} \, M \, s^{-1}$
$0.2$	$0.4$	$8 \times 10^{-2} \, M \, s^{-1}$

Medium

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For a reaction of order $(n - 1)$,what is the relationship between the half-life period $(t_{1/2})$ and the initial concentration of the reactant $([R]_0)$?

Easy

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Rate law for the reaction,$C_2H_5I_{(g)} \rightarrow C_2H_{4_{(g)}} + HI_{(g)}$ is $r = k[C_2H_5I]$. What is the order and molecularity of this reaction?

EasyMHT CET 2025

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For a chemical reaction,$m A \rightarrow x B$,the rate law is $r = k[A]^{2}$. If the concentration of $A$ is doubled,the reaction rate will be,

MediumKCET 2016

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Why can’t molecularity of any reaction be equal to zero?

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For a certain reaction,the expression for half-life is $t_{1/2} \propto \frac{1}{a^{n-1}}$. What is the order of the reaction?

$A_2 + 2 \, B \to 2 \, AB$ $[A_2]$ $[B]$ $-d[A_2]/dt$ $0.1$ $0.2$ $1 \times 10^{-2} \, M \, s^{-1}$ $0.2$ $0.2$ $2 \times 10^{-2} \, M \, s^{-1}$ $0.2$ $0.4$ $8 \times 10^{-2} \, M \, s^{-1}$ The order of reaction with respect to $A_2$ and $B$ are respectively:

For a reaction of order $(n - 1)$,what is the relationship between the half-life period $(t_{1/2})$ and the initial concentration of the reactant $([R]_0)$?

Rate law for the reaction,$C_2H_5I_{(g)} \rightarrow C_2H_{4_{(g)}} + HI_{(g)}$ is $r = k[C_2H_5I]$. What is the order and molecularity of this reaction?

For a chemical reaction,$m A \rightarrow x B$,the rate law is $r = k[A]^{2}$. If the concentration of $A$ is doubled,the reaction rate will be,

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$A_2 + 2 \, B \to 2 \, AB$

$[A_2]$ $[B]$ $-d[A_2]/dt$

$0.1$ $0.2$ $1 \times 10^{-2} \, M \, s^{-1}$

$0.2$ $0.2$ $2 \times 10^{-2} \, M \, s^{-1}$

$0.2$ $0.4$ $8 \times 10^{-2} \, M \, s^{-1}$

The order of reaction with respect to $A_2$ and $B$ are respectively: