Molecularity of a Reaction

The reaction $2\mathrm{NO}+{\mathrm{Br}}_2\to 2\mathrm{NOBr}$ takes place through the mechanism given below

$\mathrm{NO}+{\mathrm{Br}}_2\stackrel{}{\rightleftharpoons }{\mathrm{NOBr}}_2 \left(\mathrm{fast}\right)$

${\mathrm{NOBr}}_2+\mathrm{NO}\to 2\mathrm{NOBr} \left(\mathrm{slow}\right)$

The overall order of the reaction is _____.

For the chemical reaction

$4\mathrm{HBr}+{\mathrm{O}}_2\stackrel{}{\to }2{\mathrm{H}}_2\mathrm{O}+2{\mathrm{O}}_2$

Rate$=\mathrm{k}\left[\mathrm{HBr}\right]\left[{\mathrm{O}}_2\right]$

What is the probable mechanism of the reaction?

For the reaction ${\mathrm{C}}_{12}{\mathrm{H}}_{22}{\mathrm{O}}_{11}+{\mathrm{H}}_2\mathrm{O}\stackrel{ {\mathrm{H}}^{+} }{\to }{\mathrm{C}}_6{\mathrm{H}}_{12}{\mathrm{O}}_6+{\mathrm{C}}_6{\mathrm{H}}_{12}{\mathrm{O}}_6$, write molecularity.

Explain with suitable example, how the molecularity of a reaction is different from the order of a reaction?

Give any four differences between order of a reaction and its molecularity.

Nitric oxide, $\mathrm{NO}$, reacts with oxygen to produce nitrogen dioxide, $2\mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\stackrel{ }{\to }2{\mathrm{NO}}_2\left(\mathrm{g}\right)$. The rate law for this reaction is $\mathrm{rate}=\mathrm{k} {\left[\mathrm{NO}\right]}^2\left[{\mathrm{O}}_2\right]$.  Propose a mechanism for the above reaction.

The rate expression of a reaction is given below:

${\mathrm{NO}}_2+\mathrm{CO}\stackrel{ }{\to }{\mathrm{CO}}_2+\mathrm{NO}$, $\mathrm{rate}=\mathrm{k} {\left[{\mathrm{NO}}_2\right]}^2$

Propose the possible mechanism of the reaction.

The rate expression of a reaction is given below:

$2{\mathrm{NO}}_2+{\mathrm{F}}_2\stackrel{ }{\to }2{\mathrm{NO}}_2\mathrm{F}$, $\mathrm{rate}=\mathrm{k} \left[{\mathrm{NO}}_2\right]\left[{\mathrm{F}}_2\right]$

Propose the possible mechanism of the reaction.

The rate expression of a reaction is given below:

$2{\mathrm{N}}_2{\mathrm{O}}_5\stackrel{ }{\to }4{\mathrm{NO}}_2+{\mathrm{O}}_2$, $\mathrm{rate}=\mathrm{k} \left[{\mathrm{N}}_2{\mathrm{O}}_5\right]$

Propose the possible mechanism of the reaction.

What is meant by the rate controlling step in a reaction?

Comment on the statement that molecularity of the slowest step in a reaction gives the overall molecularity of the reaction.

Define and explain the term molecularity of a reaction with suitable example.

Define the following:
Molecularity of a reaction.

Discuss the difference between order and molecularity of a chemical reaction.

For the reaction ${\mathrm{NO}}_2+\mathrm{CO}\stackrel{ }{\to }{\mathrm{CO}}_2+\mathrm{NO}$, the rate law is $\mathrm{rate}=\mathrm{k} {\left[{\mathrm{NO}}_2\right]}^2$. Propose the probable mechanism of this reaction.
 

What is the molecularity of the reaction, $\mathrm{Cl}\stackrel{ }{\to }\frac{1}{2}{\mathrm{Cl}}_2\left(\mathrm{g}\right)$?

What is meant by an elementary reaction?

What is the rate determining step of a reaction? 

Define 'molecularity of a reaction'.

Consider the decomposition of hydrogen peroxide in alkaline medium which is catalysed by iodide ions:

$2{\mathrm{H}}_2{\mathrm{O}}_2\stackrel{{\mathrm{OH}}^{-}}{⟶}2{\mathrm{H}}_2\mathrm{O}+{\mathrm{O}}_2$

This reaction takes place in two steps as given below :

Step-I. ${\mathrm{H}}_2{\mathrm{O}}_2+{\mathrm{I}}^{-}⟶{\mathrm{H}}_2\mathrm{O}+{\mathrm{IO}}^{-}\left(\mathrm{slow}\right)$

Step-II. ${\mathrm{H}}_2{\mathrm{O}}_2+{\mathrm{IO}}^{-}⟶{\mathrm{H}}_2\mathrm{O}+{\mathrm{I}}^{-}+{\mathrm{O}}_2 \left(\mathrm{fast}\right)$

What is the molecularity of each individual step?