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Threshold energy is the energy needed to make effective collisions while activation energy is the energy needed to make these collisions even occur. A molecule normally doesn't have enough threshold energy to make this occur so it needs activation energy to start these collisions.
Activation energy is the energy difference between reactants and products in a chemical reaction (energy needed to make the reaction occur), while threshold energy is the energy required for reactants to undergo successful collisions (existing kinetic energy + activation energy). Thus, threshold energy is greater than activation energy.
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