Catalysis

In chemistry and biology, catalysis refers to the acceleration of the rate of a chemical reaction by a substance, called a catalyst, that is itself unchanged by the overall reaction.

A common misunderstanding is that catalysis "makes the reaction happen": that the reaction would not otherwise proceed without the presence of the catalyst.

In biologically- or industrially-useful timescales, this may be true in a limited sense. However, a catalyst cannot make a thermodynamically unfavorable reaction proceed. Rather, it can only speed up a reaction that is already thermodynamically favorable. Such a reaction in the absence of a catalyst would proceed, even without the catalyst, although perhaps too slowly to be observed or of use in a given context.

Catalysts accelerate the chemical reaction by providing a lower energy pathway between the reactants and the products. This usually involves the formation of an intermediate, which cannot be formed without the catalyst. The formation of this intermediate and subsequent reaction generally has a much lower activation energy barrier than is required for the direct reaction of reactants to products.

Catalysis is a very important process from an industrial point of view since the production of most industrially important chemicals involve catalysis. Research into catalysis is a major field in applied science, and involves many fields of chemistry and physics.

Two types of catalysis are generally distinguished. In homogeneous catalysis the reactants and catalyst are in the same phase. For example acids (H⁺ ion donors) are common catalysts in many aqueous reactions. In this case both the reactants and the catalysts are in the aqueous phase. In heterogeneous catalysis the catalyst is in a different phase than the reactants and products. Usually, the catalyst is a solid and the reactants and products are gases or liquids. In order for the reaction to occur one or more of the reactants must diffuse to the catalyst surface and adsorb onto it. After reaction, the products must desorb from the surface and diffuse away from the solid surface. Frequently, this transport of reactants and products from one phase to another plays a dominant role in limiting the rate of reaction. Understanding these transport phenomena is an important area of heterogeneous catalyst research.

Important catalytic processes

• The Haber process for ammonia synthesis
• Steam reforming of hydrocarbons to produce synthesis gas
• Methanol synthesis
• Fischer-Tropsch synthesis
• Hydrogenation/dehydrogenation of organic compounds
• Sulfuric acid production
• Nitric acid production
• Maleic anhydride production
• Petroleum refining and processing
  • Hydrotreating - hydrogenation of hydrocarbons and removal of organic sulfur, nitrogen, oxygen, and metals
  • Catalytic cracking - breaking long-chain hydrocarbons into smaller pieces
  • Naptha reforming
  • Alkylation
• Industrial and automotive abatement of NO_x, CO, and hydrocarbons
• Nearly every chemical process associated with life!

See also

Carbonate Phosphodiesterase, Metabolic pathway, Protein phosphatase, Denaturation Protein kinase, Surface chemistry, Abzyme, Dispersion (materials science), Urea cycle, Urease, Adenylate cyclase, ATPase, EC number, Diastase, Alcohol dehydrogenase, Reverse transcriptase, Ozone hole, Catalyst, RNA world hypothesis, Cyclic adenosine monophosphate, Intron, Albert Szent-Györgyi, RNAse, Nobel Prize in Chemistry, Ribozyme, Enzyme, Michaelis-Menten kinetics, Mitochondrion