Theory
Catalysts are chemical compounds that increase the rate of a reaction by lowering the activation energy required to reach the transition state. Unlike reactants, a catalyst is not consumed as part of the reaction process. The process of speeding up a reaction by using a catalyst is known as catalysis.
Catalysts can be divided into two types, homogeneous or heterogeneous, depending on the reaction phase that they occupy.
Homogeneous catalysts are those that occupy the same phase as the reaction mixture (typically liquid or gas), while heterogeneous catalysts occupy a different phase. Heterogeneous catalysts are solid compounds that are added to liquid or gas reaction mixtures. Examples of homogeneous catalysts are acid catalysis, organometallic catalysis, and enzymatic catalysis.
