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activation energy. activation energy, in chemistry, minimum energy needed to cause a chemical reaction. A chemical reaction between two substances occurs only when an atom, ion, or molecule of one collides with an atom, ion, or molecule of the other.
The activation energy [Activation energy: The minimum energy required for a collision between particles, in order for a reaction to occur.] (E a) for the forward reaction is shown by (A): E a (forward) = H (activated complex) - H (reactants) = 200 - 150 = 50 kJ mol-1. The activation energy (E a) for the reverse reaction is shown by (B): E a (reverse) = H (activated complex) - H (products) = 200 - 50 = 150 kJ mol-1. The enthalpy change for the forward reaction is shown by (C):