Molecularity of a Reaction

Consider the reaction: ${\mathrm{Cl}}_2\left(\mathrm{aq}\right)+{\mathrm{H}}_2\mathrm{S}\left(\mathrm{aq}\right)\to \mathrm{S}\left(\mathrm{s}\right)+2{\mathrm{H}}^{+}\left(\mathrm{aq}\right)+2{\mathrm{Cl}}^{-}\left(\mathrm{aq}\right)$

The rate equation for this reaction is:

$\mathrm{Rate}=\mathrm{K}\left[{\mathrm{Cl}}_2\right]\left[{\mathrm{H}}_2\mathrm{S}\right]$

The following are the suggested mechanisms.

$\begin{array}{l}\left(\mathrm{A}\right) {\mathrm{Cl}}_2+{\mathrm{H}}_2\mathrm{S}\to {\mathrm{H}}^{+}+{\mathrm{Cl}}^{-}+{\mathrm{Cl}}^{+}+{\mathrm{HS}}^{-}\left(\mathrm{slow}\right) \\ {\mathrm{Cl}}^{+}+{\mathrm{HS}}^{-}\to {\mathrm{H}}^{+}+{\mathrm{Cl}}^{-}+\mathrm{S} \left(\mathrm{fast}\right)\end{array}$

$\begin{array}{ll}\left(\mathrm{B}\right) {\mathrm{H}}_2\mathrm{S}\rightleftharpoons {\mathrm{H}}^{+}+{\mathrm{HS}}^{-}& (\mathrm{fast} \mathrm{equilibrium}) \\ {\mathrm{Cl}}_2+{\mathrm{HS}}^{-}\to 2{\mathrm{Cl}}^{-}+{\mathrm{H}}^{+}+\mathrm{S}& \mathrm{ }\left(\mathrm{slow}\right)\mathrm{ }\end{array}$

What is the correct mechanism that gives the above rate equation?

Which statement about molecularity of reaction is not correct?

For a unimolecular reaction:

$2 \mathrm{HI} \to {\mathrm{H}}_2+{\mathrm{I}}_2$ 

The above reaction is an example of 

$2 \mathrm{HI} \to {\mathrm{H}}_2+{\mathrm{I}}_2$ 

What is the molecularity of the above reaction?

Trimolecular reactions are uncommon because:

If two reactants take part in a reaction, then:

Which of the reactions shows this kind of example ?

$2\mathrm{NO} + {\mathrm{O}}_2 \to 2{\mathrm{NO}}_2$

If in a unimolecular reaction, $\text{A}\left(\mathrm{g}\right)⟶\text{Products}$ takes place according to the mechanism

I. $\text{A}+\text{A}\underset{{\text{k}}_{-1}}{\overset{{\text{k}}_1}{\rightleftharpoons }}{\text{A}}^{*}+\text{A}$

II. ${\text{A}}^{*}\underset{{\text{k}}_2}{⟶}\text{P}$

where ${\text{k}}_1\text{, }{\text{k}}_{-1}$ ${\text{k}}_2$ are the rate constants and P, $\mathrm{A}$ and ${\text{A}}^{*}$ stand for product molecule, normal molecules of reactants and activated molecules of reactants respectively.

Which of the following statements are correct?

For next two question please follow the same

 If in a unimolecular reaction, $\text{A}\left(\mathrm{g}\right)⟶$ products takes place according to the mechanism

I. $\text{A}+\text{A}\underset{{\text{k}}_{-1}}{\overset{{\text{k}}_1}{\rightleftharpoons }}{\text{A}}^{*}+\text{A}$

II. ${\text{A}}^{*}\underset{{\text{k}}_2}{⟶}\text{P}$

where ${\text{k}}_1\text{, }{\text{k}}_{-1}$ ${\text{k}}_2$ are the rate constants and P, $\mathrm{A}$ and ${\text{A}}^{*}$ stand for product molecule, normal molecules of reactants and activated molecules of reactants respectively.

Which of the following expressions are correct?

The reaction between ${\mathrm{H}}_2 \left(\mathrm{g}\right)$ and $\mathrm{ICl} \left(\mathrm{g}\right)$occurs in the following steps:
$\text{ (i) }{\mathrm{H}}_2+\mathrm{ICl}⟶\mathrm{HI}+\mathrm{HCl}$

$\text{ (ii) }\mathrm{HI}+\mathrm{ICl}⟶{\mathrm{I}}_2+\mathrm{HCl}$

The reaction intermediate in the reaction is

Molecularity of an elementary reaction

Identify the correct potential energy vs reaction co-ordinate graph, which is consistent with given mechanism.

The mechanism of esterification in presence of acid catalyst (H₂SO₄) is proposed as follows:

Two different reactants involving in a reaction can not be :

Collision theory is true for

The interest rate on debentures is typically:

Planning may not work in a dynamic environment due to which of the following reasons?

What characteristic describes planning as a process that involves setting objectives and determining a course of action?

By using following mechanism determine the order of the reaction
$\left(\mathrm{i}\right)$ ${\mathrm{A}}_2\to \mathrm{A}+\mathrm{A}$ (fast)
$\left(\mathrm{i}\mathrm{i}\right)\mathrm{}\mathrm{A}+{\mathrm{B}}_2\to \mathrm{A}\mathrm{B}+\mathrm{B}$ (slow)
$\left(\mathrm{i}\mathrm{i}\mathrm{i}\right)$ $\mathrm{A}+\mathrm{B}\to$ (fast)

Consider the reaction
$2\mathrm{N}{\mathrm{O}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_3\left(\mathrm{g}\right)\to {\mathrm{N}}_2{\mathrm{O}}_5\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)$
The reaction of nitrogen dioxide and ozone represents is first order in $\mathrm{N}{\mathrm{O}}_2\left(\mathrm{g}\right)$ and in ${\mathrm{O}}_3\left(\mathrm{g}\right)$ . Which of these possible reaction mechanism is consistent with the rate law?