Activation Energy

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Activation energy	Is the energy which must be available to a chemical system with potential reactants to result in a chemical reaction. Activation energy may also be defined as the minimum energy required to start a chemical reaction or ignite a combustible vapor, gas or dust cloud.
Image: Activation Energy (binary/octet-stream)	The activation energy (Ea) of a reaction is measured in joules (J) and or kilojoules per mole (kJ/mol) or rarely kilocalories per mole (kcal/mol).
Activation energy can be thought of as the height of the potential barrier (sometimes called the energy barrier) separating two minima of potential energy (of the reactants and products of a reaction). For a chemical reaction to proceed at a reasonable rate, there should exist an appreciable number of molecules with translational energy equal to or greater than the activation energy. The term was introduced in 1889 by the Swedish scientist Svante Arrhenius.	To see: https://goo.gl/1EhjbK

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	Created by Alvaro Vargas Calero about 6 years ago