Catalysis – Class 12 | Chapter – 5 | Surface Chemistry | Chemistry Short Notes Series PDF for NEET & JEE

Catalysis: Catalysis in surface chemistry refers to the process where the rate of a chemical reaction is enhanced by the presence of a substance known as a catalyst, which remains unchanged chemically after the reaction. The catalyst works by providing an alternative reaction pathway with lower activation energy, allowing the reaction to proceed more rapidly. In surface chemistry, catalysis often occurs on the surface of a solid catalyst, where reactant molecules adsorb and react to form products.

Types of Catalysis

There are two main types of catalysis that commonly occur in surface chemistry:

  • Heterogeneous Catalysis: Heterogeneous catalysis involves a catalyst that exists in a different phase (solid, liquid, or gas) from the reactants. In surface chemistry, solid catalysts are commonly used. The reactant molecules from the gas or liquid phase adsorb onto the surface of the solid catalyst, where the reaction takes place. The products then desorb from the surface, leaving the catalyst unchanged and free to catalyze further reactions. Heterogeneous catalysis is widely used in industrial processes, such as in the production of chemicals, petroleum refining, and environmental applications.

Example of Heterogeneous Catalysis: One classic example of heterogeneous catalysis is the Haber-Bosch process, where nitrogen and hydrogen gases are reacted over a solid iron catalyst to produce ammonia. The iron catalyst provides active sites on its surface where nitrogen and hydrogen molecules can interact and react to form ammonia.

  • Homogeneous Catalysis: Homogeneous catalysis involves a catalyst that is in the same phase as the reactants, usually a dissolved species in a liquid phase. However, in some cases, homogeneous catalysis can also occur in the gas phase. In surface chemistry, this type of catalysis may involve reactants that form a complex with the catalyst at the surface, leading to a faster reaction rate. Homogeneous catalysis is often more selective than heterogeneous catalysis because the catalyst can interact more directly with the reactant molecules.

Example of Homogeneous Catalysis: A well-known example of homogeneous catalysis is the reaction between hydrogen peroxide (H2O2) and iodide ions (I-) in the presence of a small amount of iodine (I2) acting as a catalyst. The iodine forms a complex with hydrogen peroxide at the surface, facilitating the reaction to produce water and oxygen.

Applications of Catalysis

Catalysis is a vital process with widespread applications, including:

  • Industrial processes: Catalysis is central to the production of various chemicals, fuels, and materials, contributing to the efficiency and sustainability of these processes.
  • Environmental applications: Catalytic converters in automobiles use catalysts to convert harmful exhaust gases into less toxic compounds, reducing air pollution.
  • Energy production: Catalysis is involved in various energy-related processes, such as fuel cells and hydrogen production.
  • Petrochemical refining: Catalysis is employed in refining crude oil to produce valuable products like gasoline, diesel, and other petroleum-based products.

Biology Quiz & Notes Physics Quiz & Notes Chemistry Quiz & Notes

Follow on Facebook

By Team Learning Mantras