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Molecularity in chemistry is the number of molecules that come together to react in an elementary reaction〔Atkins, P.; de Paula, J. Physical Chemistry. Oxford University Press, 2014〕 and is equal to the sum of stoicheometric coefficients of reactants in this elementary reaction.〔Temkin, O. N. State-of-the-Art in the Theory of Kinetics of Complex Reactions. In Homogeneous Catalysis with Metal Complexes: Kinetic Aspects and Mechanisms, John Wiley and Sons, ltd, 2012〕 Depending on how many molecules come together, a reaction can be unimolecular, bimolecular or termolecular. == Unimolecular Reactions == In a unimolecular reaction, a single molecule rearranges atoms forming different molecules.〔 This is illustrated by the equation ''A → P'' and is described by the first order rate law d()/dt = -kr (), where () is the concentration of species A, t is time, and kr is the reaction rate constant. As can be deduced from the rate law equation, the number of A molecules that decay is proportional to the number of A molecules available. An example of a unimolecular reaction, is the isomerization of cyclopropane to propene: Unimolecular reactions can be explained by the Lindemann-Hinshelwood mechanism. 抄文引用元・出典: フリー百科事典『 ウィキペディア（Wikipedia）』 ■ウィキペディアで「Molecularity」の詳細全文を読む スポンサード リンク
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