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[[File:Catalysts.JPG|Catalysts|thumb]] [[Image:Low_Temperature_Oxidation_Catalyst.jpeg|Low Temperature Oxidation Catalyst|thumb|left]] [[Image:CatalysisScheme-en.svg|CatalysisScheme-en|thumb|left]] [[File:Zeolite-ZSM-5-vdW.png|Zeolite-ZSM-5-vdW|thumb]] [[File:Ceolite_nax.JPG|Ceolite nax|thumb]] '''Catalysis''' is a process in which the rate of a [[chemical reaction]] is increased by a substance known as a [[catalyst]]. Catalysts are not consumed in the reaction and can continue to act repeatedly. Because of this, only very small amounts of catalyst are required to alter the reaction rate in principle. Catalysis plays an essential role in the chemical industry and in many industrial processes, where it facilitates reactions that would otherwise be prohibitively slow or would require more energy-intensive conditions.

==Types of Catalysis==
Catalysis can be broadly divided into two types: [[homogeneous catalysis]] and [[heterogeneous catalysis]].

===Homogeneous Catalysis===
In homogeneous catalysis, the catalyst is in the same phase (solid, liquid, or gas) as the reactants. This allows for easy mixing and often leads to efficient interaction between the catalyst and reactant molecules. Examples include acid-base catalysis and transition metal complex catalysis.

===Heterogeneous Catalysis===
In heterogeneous catalysis, the catalyst is in a different phase than the reactants. Typically, the catalyst is a solid, and the reactants are either gases or liquids. This type of catalysis is prevalent in the industry, especially in processes like the [[Haber-Bosch process]] for ammonia synthesis, where iron is used as a catalyst, and in the catalytic converters of automobiles, which use metals like platinum, palladium, and rhodium to reduce exhaust emissions.

==Mechanism of Catalysis==
The mechanism of catalysis involves the formation of an intermediate complex between the catalyst and the reactant molecules. This complex lowers the [[activation energy]] required for the reaction to proceed, leading to an increased reaction rate. The catalyst remains unchanged after the reaction and can participate in multiple reaction cycles.

==Importance of Catalysis==
Catalysis is crucial for a wide range of industrial and environmental processes. It enables the efficient production of chemicals, fuels, and pharmaceuticals, often under milder conditions than would otherwise be necessary, which can save energy and reduce the production of unwanted byproducts. Catalysis is also vital in pollution control, such as in the removal of harmful substances from industrial emissions and automotive exhaust.

==Enzyme Catalysis==
In biological systems, [[enzymes]] act as highly efficient catalysts for biochemical reactions. Enzyme catalysis is fundamental to all aspects of life, including metabolism, DNA replication, and the synthesis of macromolecules. Enzymes are proteins that can catalyze reactions with high specificity for their substrates, often at remarkable speeds and under mild conditions.

==Research and Development in Catalysis==
Research in the field of catalysis focuses on developing new catalysts, improving the efficiency of existing ones, and understanding the mechanisms by which they operate. This research has significant implications for energy production, environmental protection, and the synthesis of new materials and pharmaceuticals.

[[Category:Chemistry]]
[[Category:Catalysis]]

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Catalysis - Revision history

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