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Activation energy can be thought of as the magnitude of the potential barrier (sometimes called the energy barrier) separating minima of the potential energy surface pertaining to the initial and final thermodynamic state. For a chemical reaction to proceed at a reasonable rate, the temperature of the system should be high enough such that ...
Illustration of change in activation energy caused by a catalyst. Made by me in Inkscape by tracing the original image by Vinay.bhat, who holds the copyright but has released all rights. Description of original image: Activation energies Ea(X→Y) or 'Ea(Y→X)' need to be supplied to initiate the reactions X→Y or Y→X, respectively. When ...
Activation energy for catalysed and uncatalysed reactions. International version. Date: 26 March 2007: Source: Own work, adapted from Image:Activation2 updated.svg:
For any reaction to proceed, the starting material must have enough energy to cross over an energy barrier. This energy barrier is known as activation energy (∆G ≠) and the rate of reaction is dependent on the height of this barrier. A low energy barrier corresponds to a fast reaction and high energy barrier corresponds to a slow reaction.
Diagram of a catalytic reaction, showing the energy level as a function of the reaction coordinate. For a catalyzed reaction, the activation energy is lower.. In chemistry, a reaction coordinate [1] is an abstract one-dimensional coordinate chosen to represent progress along a reaction pathway.
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The activation energy is the minimum amount of energy to initiate a chemical reaction and form the activated complex. [6] The energy serves as a threshold that reactant molecules must surpass to overcome the energy barrier and transition into the activated complex.