How this energy compares to the kinetic energy provided by colliding reactant molecules is a primary factor affecting the rate of a chemical reaction. If the activation energy is much larger than the average kinetic energy of the molecules, the reaction will occur slowly since only a few fast-moving molecules will have enough energy to react. If the activation energy is much smaller than the average kinetic energy of the molecules, a large fraction of molecules will be adequately energetic and the reaction will proceed rapidly.
Activation energy (Ea)
The minimum energy necessary to form a product during a collision between reactants is called the activation energy (Ea).
Source & attribution
Chemistry 2e — Collision Theory
OpenStax contributors · OpenStax, Rice University
CC BY 4.0. Text excerpted; whitespace normalised and empty cross-references removed; learning prompts added. No illustrations reproduced.
Source edition: 2024-12-20T01:30:25Z
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