catalyst: Laboratory and Industrial Catalysts

Laboratory and Industrial Catalysts

Catalysis is also important in chemical laboratories and in industry. Some reactions occur faster in the presence of a small amount of an acid or base and are said to be acid catalyzed or base catalyzed. For example, the hydrolysis of esters is catalyzed by the presence of a small amount of base. In this reaction, it is the hydroxide ion, OH⁻, that reacts with the ester, and the concentration of the hydroxide ion is greatly increased over that of pure water by the presence of the base. Although some of the hydroxide ions provided by the base are used up in the first part of the reaction, they are regenerated in a later step from water molecules; the net amount of hydroxide ion present is the same at the beginning and end of the reaction, so the base is thought of as a catalyst and not as a reactant.

Finely divided metals are often used as catalysts; they adsorb the reactants onto their surfaces (see adsorption), where the reaction can occur more readily. For example, hydrogen and oxygen gases can be mixed without reacting to form water, but if a small amount of powdered platinum is added to the gas mixture, the gases react rapidly. Hydrogenation reactions, e.g., the formation of hard cooking fats from vegetable oils, are catalyzed by finely divided metals or metal oxides. The commercial preparation of sulfuric acid and nitric acid also depends on such surface catalysis. Other commonly used surface catalysts, in addition to platinum, are copper, iron, nickel, palladium, rhodium, ruthenium, silica gel (silicon dioxide), and vanadium oxide.

Sections in this article:

Introduction
Laboratory and Industrial Catalysts
Enzymes: Natural Catalysts
Mechanism of Catalysis

See more Encyclopedia articles on: Chemistry: General