Threshold and activation energy
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Re: Threshold and activation energy
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.
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Re: Threshold and activation energy
So a molecule uses activation energy to start making collisions but runs out of energy and thus uses threshold energy?
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Re: Threshold and activation energy
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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