Molecularity of a 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

In the steady state approximation, if $\mathrm{I}$ is the intermediate formed, then

The mechanism of esterification in presence of acid catalyst $\left(H_{2}S{O}_4\right)$ is proposed as follows:



Which of the following potential energy vs reaction co-ordinate diagram is consistent with given mechanism?

STATEMENT-1: $\mathrm{N}{\mathrm{O}}_2+\mathrm{C}\mathrm{O}\to \mathrm{C}{\mathrm{O}}_2+\mathrm{N}\mathrm{O}$

$\mathrm{r}=\mathrm{k}\left[\mathrm{N}{\mathrm{O}}_2\right]$

The rate of the above reaction is independent of the concentration of CO

STATEMENT-2: The rate does not depend upon [CO] because it is involved in fast step.

A hypothetical reaction ${\mathrm{A}}_2+{\mathrm{B}}_2\to 2\mathrm{A}\mathrm{B}$ follows the mechanism as given below:

${\mathrm{A}}_2{}_{\leftarrow }{}^{\to }\mathrm{A}+\mathrm{A}\left(\mathrm{fast}\right)$
$\mathrm{A}+{\mathrm{B}}_2\to \mathrm{A}\mathrm{B}+\mathrm{B}\mathrm{ }\left(\mathrm{s}\mathrm{l}\mathrm{o}\mathrm{w}\right)$

$\mathrm{A}+\mathrm{B}\to \mathrm{A}\mathrm{B}\mathrm{ }\left(\mathrm{f}\mathrm{a}\mathrm{s}\mathrm{t}\right)$

What will be the order of the overall reaction?

A reaction involving two different reactants:

The reaction: $2\mathrm{N}\mathrm{O}+2{\mathrm{H}}_2\to {\mathrm{N}}_2+2{\mathrm{H}}_2\mathrm{O}$ has been assigned to follow given mechanism:

I. $\mathrm{N}\mathrm{O}+\mathrm{N}\mathrm{O}\rightleftharpoons {\mathrm{N}}_2{\mathrm{O}}_2\mathrm{ }\left(\mathrm{f}\mathrm{a}\mathrm{s}\mathrm{t}\right)$

II. ${\mathrm{N}}_2{\mathrm{O}}_2+{\mathrm{H}}_2\to {\mathrm{N}}_2\mathrm{O}+{\mathrm{H}}_2\mathrm{O}\mathrm{ }\left(\mathrm{s}\mathrm{l}\mathrm{o}\mathrm{w}\right)$

III. ${\mathrm{N}}_2\mathrm{O}+{\mathrm{H}}_2\to {\mathrm{N}}_2+{\mathrm{H}}_2\mathrm{O}\mathrm{ }\left(\mathrm{f}\mathrm{a}\mathrm{s}\mathrm{t}\right)$

The rate constant of step II is $1.2\times {10}^4\mathrm{ }\mathrm{m}\mathrm{o}\mathrm{l}{\mathrm{e}}^{-1}\mathrm{ }\mathrm{L}\mathrm{ }{\mathrm{m}\mathrm{i}\mathrm{n}}^{-1}$ while equilibrium constant of step I is $1.4\times {10}^2$ . What is the rate of reaction when concentration of $\mathrm{NO}$ and ${\mathrm{H}}_2$ each is $0.5$mole ${\mathrm{L}}^{-1}$

The mechanism of the following reaction is:

$2\mathrm{N}\left(\mathrm{g}\right)+2{\mathrm{H}}_2\mathrm{ }\left(\mathrm{g}\right)\mathrm{ }⟶{\mathrm{N}}_2\mathrm{ }\left(\mathrm{g}\right)+2{\mathrm{H}}_2\left(\mathrm{g}\right)$

Step 1$:2\mathrm{N}\left(\mathrm{g}\right)+2{\mathrm{H}}_2\mathrm{ }\left(\mathrm{g}\right)\mathrm{ }\stackrel{\mathrm{slow}}{\to }{\mathrm{N}}_2\mathrm{ }\left(\mathrm{g}\right)+{\mathrm{H}}_2$

Step 2$:2{\mathrm{H}}_2+{\mathrm{O}}_2\stackrel{\mathrm{f}\mathrm{a}\mathrm{s}\mathrm{t}}{\to }\mathrm{ }2{\mathrm{H}}_2\mathrm{O}$

Which of the following statements is true-

As per the following consecutive reactions the r.d.s. is

(P) $\stackrel{\mathrm{k}=2\times {10}^{-5}{\mathrm{s}}^{-1}}{\to }$

(Q) $\stackrel{\mathrm{k}=8\times {10}^{-6}{\mathrm{s}}^{-1}}{\to }$

(R) $\stackrel{\mathrm{k}=3\times {10}^{-3}{\mathrm{s}}^{-1}}{\to }$

(S)