(A) Molecularity of a reaction is defined as the number of reacting species (atoms, ions, or molecules) taking part in an elementary reaction, which m

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It may be whole number or fractional

(A) Molecularity of a reaction 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. Molecularity is always a whole number $(1, 2, 3, ...)$ and can never be zero, fractional, or negative. Therefore, the statement that it may be a fractional number is incorrect.

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

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Which one of the following is wrong about molecularity of a reaction?

WBJEE 2012 All WBJEE

A
It may be whole number or fractional
B
It is calculated from reaction mechanism
C
It is the number of molecules of the reactants taking part in a single step chemical reaction
D
It is always equal to the order of elementary reaction

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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Give the relation between half-life $(t_{1/2})$ and initial concentration of reactant $([R]_0)$ for an $(n-1)^{th}$ order reaction.

EasyGUJCET 2011

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For a reaction between $A$ and $B$,the order with respect to $A$ is $2$ and the order with respect to $B$ is $3$. If the concentrations of both $A$ and $B$ are doubled,the rate will increase by a factor of:

MediumNEET 2013

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For the reaction $A + B \xrightarrow{K} C$,identify the incorrect order of reaction indicated against the rate expression.

Easy

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The following data are for the decomposition of ammonium nitrate in aqueous solution. The order of the reaction is:
$N_2$ volume in $cc$ $(V_t)$ $6.25$ $9.50$ $11.42$ $13.65$ $35.05$ $(V_{\infty})$
Time $(t)$ in minutes $10$ $15$ $20$ $25$ $\infty$

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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$N_2$ volume in $cc$ $(V_t)$	$6.25$	$9.50$	$11.42$	$13.65$	$35.05$ $(V_{\infty})$
Time $(t)$ in minutes	$10$	$15$	$20$	$25$	$\infty$

Which one of the following is wrong about molecularity of a reaction?

Similar Questions

Give the relation between half-life $(t_{1/2})$ and initial concentration of reactant $([R]_0)$ for an $(n-1)^{th}$ order reaction.

For a reaction between $A$ and $B$,the order with respect to $A$ is $2$ and the order with respect to $B$ is $3$. If the concentrations of both $A$ and $B$ are doubled,the rate will increase by a factor of:

For the reaction $A + B \xrightarrow{K} C$,identify the incorrect order of reaction indicated against the rate expression.

The following data are for the decomposition of ammonium nitrate in aqueous solution. The order of the reaction is:$N_2$ volume in $cc$ $(V_t)$$6.25$$9.50$$11.42$$13.65$$35.05$ $(V_{\infty})$Time $(t)$ in minutes$10$$15$$20$$25$$\infty$

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:

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The following data are for the decomposition of ammonium nitrate in aqueous solution. The order of the reaction is:
$N_2$ volume in $cc$ $(V_t)$ $6.25$ $9.50$ $11.42$ $13.65$ $35.05$ $(V_{\infty})$
Time $(t)$ in minutes $10$ $15$ $20$ $25$ $\infty$