Activation Energy - In this video Paul Andersen explains how the activation energy is a measure of the amount of energy required for a chemical reaction to occur. Due to the collision theory the activation energy requires proper energy and orientation of the colliding molecules. The Maxwell-Boltzman distribution can be used to determine the number of particles above and below this point.
Activation energy - the molecules must collide with sufficient energy to break the existing bonds in the reactants and form new products via bond formation in the products (activation energy). Usually supplied via the addition of heat or a flame (temperature = kinetic energy). This energy is added and the bonds form by absorbing this energy (endothermic).
The Reaction Path: In this video Paul Andersen explains how the reaction path can be described in an energy profile. Enough energy must be added to reach the activation energy required and stress the bonds. Eventually the bonds break and new bonds are formed. The rate constant is temperature dependent. The Arrhenius equation can be used to calculate the activation energy when the temperature and rate constant are calculated.
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Two schematic plots are shown side by side, comparing the amount of activation energy required to support an un-catalyzed reaction (left) versus an enzyme-catalyzed reaction (right). Total energy is the label on the y-axis.
This high-energy state is often referred as transition state. These transition states have a relatively short life span, and once this highly unstable transition state is formed, it quickly disintegrates to form the products. For a reaction to reach this transition energy level, a certain amount of energy is required. This energy is called the activation energy or the energy of activation.