Molecularity of a Reaction

Which statement about molecularity of reaction is not correct?

For a unimolecular reaction:

Which reaction called Trimolecular reaction?

Write a very short note on bimolecular 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:

Give an example for trimolecular reaction ?

Define trimolecular or termolecular reaction.

Termolecular reactions involve simultaneous collision between _____ reacting species.(three/ four)

Which of the reactions shows this kind of example ?

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

Define unimolecuar reaction ?

Give an example for an unimolecular reaction.

Consider the reaction ${\mathrm{Tl}}^{+}\left(\mathrm{aq}\right)+2{\mathrm{Ce}}^{4+}+\left(\mathrm{aq}\right)\to {\mathrm{Tl}}^{3+}+\left(\mathrm{aq}\right)+2{\mathrm{Ce}}^{3+}\left(\mathrm{aq}\right)$ 

The rate law for the reaction is rate =$\mathrm{k}$ $\left[{\mathrm{Ce}}^{4+}\right] \left[{\mathrm{Mn}}^{2+}\right].$

In the presence of ${\mathrm{Mn}}^{2+}$the reaction occurs in the following elementary steps:

${\mathrm{Ce}}^{4+ }\left(\mathrm{aq}\right)+{\mathrm{Mn}}^{2+}\left(\mathrm{aq}\right) \to {\mathrm{Ce}}^{3+}\left(\mathrm{aq}\right)+{\mathrm{Mn}}^{3+} \left(\mathrm{aq}\right)$

${\mathrm{Ce}}^{4+}\left(\mathrm{aq}\right)+{\mathrm{Mn}}^{3+}\left(\mathrm{aq}\right)\to {\mathrm{Ce}}^{3+}\left(\mathrm{aq}\right)+{\mathrm{Mn}}^{4+}\left(\mathrm{aq}\right)$

${\mathrm{Tl}}^{+}\left(\mathrm{aq}\right)+{\mathrm{Mn}}^{4+}\left(\mathrm{aq}\right)⟶{\mathrm{Tl}}^{3+}\left(\mathrm{aq}\right)+{\mathrm{Mn}}^{2+}\left(\mathrm{aq}\right)$

Identify rate determining step.

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

The rate law for the reaction $2 {\mathrm{H}}_2 \left(\mathrm{g}\right) + 2\mathrm{NO} \left(\mathrm{g}\right) \to {\mathrm{N}}_2 \left(\mathrm{g}\right) + 2{\mathrm{H}}_2\mathrm{O} \left(\mathrm{g}\right)$ is given by rate $=\mathrm{K} \left[{\mathrm{H}}_2\right] [\mathrm{NO}{]}^2$. The reaction occurs in the following steps:

$$\begin{gathered} {\mathrm{H}}_2 + 2\mathrm{NO} \to {\mathrm{N}}_2\mathrm{O} + {\mathrm{H}}_2\mathrm{O} \\ {\mathrm{N}}_2\mathrm{O} + {\mathrm{H}}_2 \to {\mathrm{N}}_2 + {\mathrm{H}}_2\mathrm{O} \end{gathered}$$
Identify the slow step.

The rate law for the reaction $2 {\mathrm{H}}_2 \left(\mathrm{g}\right) + 2\mathrm{NO} \left(\mathrm{g}\right) \to {\mathrm{N}}_2 \left(\mathrm{g}\right) + 2{\mathrm{H}}_2\mathrm{O} \left(\mathrm{g}\right)$ is given by rate $=\mathrm{K} \left[{\mathrm{H}}_2\right] [\mathrm{NO}{]}^2$. The reaction occurs in the following steps:

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

$N_{2}O+H_2\to N_2+H_{2}O$

What is the role of ${\mathrm{N}}_2\mathrm{O}$ in the mechanism?

Molecularity of an elementary reaction

The rate law for the reaction $2\mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)\to 2\mathrm{NOCl}\left(\mathrm{g}\right)$ is given by rate $=\mathrm{k} \left[\mathrm{NO}\right] \left[{\mathrm{Cl}}_2\right]$ . The reaction occurs in the following steps:
(i) $\mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\to {\mathrm{NOCl}}_2\left(\mathrm{g}\right)$.

(ii) ${\mathrm{NOCl}}_2\left(\mathrm{g}\right)+\mathrm{NO}\left(\mathrm{g}\right)\to 2\mathrm{NOCl}\left(\mathrm{g}\right)$.

Identify the rate determining step.