Activation energy = (Threshold energy) - (Average energy of the reactants)
= ET - ER
The concept of activation can be easily visualized from the figure.
Activation energy is low for fast reactions.
Activation energy is high for slow reactions.
Consider expression of rate constant according to collision theory.
k = Zfp
where Z is the collision frequency
f is the fraction of collisions having energy greater than the threshold energy and p is the fraction of the collisions that occurs with the reactant molecules properly oriented.
Rate= PZ e-Ea/RT
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