Animated Solution for Chemistry - Surface Chemistry: Match the catalysts to the correct processes.

In the vast and fascinating world of industrial chemistry, reactions that would normally take centuries to complete are accelerated to mere seconds. The secret behind this chemical sorcery? Catalysts.

In this problem, we are presented with four legendary catalysts and four monumental industrial processes. Our mission is to pair them up correctly. Let's dive into the chemistry behind each of these pairings.

First on our list is Titanium Trichloride, or ${\text{TiCl}}_3$. When you see this compound, your mind should immediately jump to the world of polymers.

When ${\text{TiCl}}_3$ is combined with an organoaluminium compound like triethylaluminium ${\text{Al(C}}_2{\text{H}}_5{)}_3$, it forms the revolutionary Ziegler-Natta catalyst. This catalyst completely transformed the plastics industry by allowing the polymerisation of terminal alkenes (like ethene) at atmospheric pressure and room temperature, producing high-density polyethene (HDPE). Therefore, ${\text{TiCl}}_3$ perfectly matches with the Ziegler-Natta polymerisation.

Next, we encounter Palladium Dichloride, ${\text{PdCl}}_2$. This transition metal salt is the heart of the Wacker process.

The Wacker process is a brilliant example of homogeneous catalysis used to oxidize ethene into ethanal (acetaldehyde). The ${\text{PdCl}}_2$ coordinates with the ethene molecule, making it susceptible to nucleophilic attack by water. During this process, the palladium is reduced, and a co-catalyst (usually ${\text{CuCl}}_2$) is used to re-oxidize it back to its active state. Thus, ${\text{PdCl}}_2$ is the signature catalyst for the Wacker process.

Moving on to Copper Dichloride, ${\text{CuCl}}_2$. Imagine you have a massive industrial byproduct of hydrogen chloride ($\text{HCl}$) gas, and you need to convert it into valuable chlorine (${\text{Cl}}_2$) gas.

This is exactly what Deacon's process achieves. By reacting $\text{HCl}$ gas with atmospheric oxygen at high temperatures, chlorine gas is produced. The reaction is notoriously slow on its own, but the addition of ${\text{CuCl}}_2$ as a catalyst dramatically speeds it up. The copper cycles between its $+1$ and $+2$ oxidation states, facilitating the transfer of electrons. Hence, ${\text{CuCl}}_2$ is the champion of Deacon's process.

Finally, we arrive at Vanadium Pentoxide, ${\text{V}}_2{\text{O}}_5$. If there is one catalyst every chemistry student must know, it is this one.

${\text{V}}_2{\text{O}}_5$ is the star of the Contact process, which is the primary method for manufacturing sulphuric acid (${\text{H}}_2{\text{SO}}_4$). The critical and most difficult step in this process is the reversible oxidation of sulphur dioxide (${\text{SO}}_2$) to sulphur trioxide (${\text{SO}}_3$). Vanadium pentoxide provides the perfect solid surface for these gases to adsorb, react, and desorb efficiently. Therefore, ${\text{V}}_2{\text{O}}_5$ is inextricably linked to the Contact process.

By understanding the chemical narrative behind each catalyst, the matching becomes intuitive rather than a mere memory exercise.

- (A) ${\text{TiCl}}_3$ drives (ii) Ziegler-Natta polymerisation. - (B) ${\text{PdCl}}_2$ powers the (i) Wacker process. - (C) ${\text{CuCl}}_2$ accelerates (iv) Deacon's process. - (D) ${\text{V}}_2{\text{O}}_5$ is the backbone of the (iii) Contact process.

Mastering these associations not only secures marks in exams but also deepens your appreciation for the chemical engineering that builds our modern world.