Activation energy

In chemistry, activation energy, also called threshold energy, is a term introduced in 1889 by Svante Arrhenius that is defined as the energy that must be overcome in order for a chemical reaction to occur.

Activation energy The activation energy in chemistry is the energy needed by a system to initiate a particular process. Activation energy is often used to denote the minimum energy needed for a specific chemical reaction to occur.

activation energy The energy that must be possessed by atoms or molecules in order to react. active site ...

Activation Energy and Enzymes The amount of activation energy that is required is considerably less when enzyme is present. Conditions that Affect Enzymatic Reactions ...

A substance that promotes a chemical reaction by lowering the activation energy of a chemical reaction, but which itself remains unaltered at the end of the reaction. (See Catalytic antibody, Catalytic RNA.) Catalytic antibody (abzyme).

activation energy (DGo') The amount of energy (SI unit of joules) required to convert 1 mole of a reactant from the ground state to the transition state.

Overcoming this repulsion requires energy (activation energy), which is typically provided by the heat of the system; i.e. Full article ...

They achieve their effect by temporarily binding to the substrate and, in doing so, lowering the activation energy needed to convert it to a product. The rate at which an enzyme works is influenced by several factors, e.g., ...

enzymes - highly specific protein catalysts, they speed up the reactions by reducing the activation energy for a particular chemical change.

Many enzymes function by lowering the activation energy of reactions. By bringing the reactants closer together, chemical bonds may be weakened and reactions will proceed faster than without the catalyst.

See also: Enzyme, Action, Trans, Molecule, Proteins