Molecularity of a 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.

Describe the experiment to determine the effect of temperature on the rate of reaction between potassium persulphate and potassium iodide. What is the conclusion drawn from the experiment?

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?

The possible mechanism for the reaction: $2{\mathrm{H}}_2+2\mathrm{NO}⟶{\mathrm{N}}_2+2{\mathrm{H}}_2\mathrm{O}$ is

(i) $2\mathrm{NO}\rightleftharpoons {\mathrm{N}}_2{\mathrm{O}}_2$ (ii) ${\mathrm{N}}_2{\mathrm{O}}_2+{\mathrm{H}}_2\to {\mathrm{N}}_2\mathrm{O}+{\mathrm{H}}_2\mathrm{O}$ (slow) (iii) ${\mathrm{N}}_2\mathrm{O}+{\mathrm{H}}_2\to {\mathrm{N}}_2+{\mathrm{H}}_2\mathrm{O}$ (fast)

What is the rate law for the reaction?