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Activation energy, by definition, is the minimum amount of energy required for reactants to form products.

Which of the following is NOT true of activation energy?


The value of activation energy varies from reaction to reaction.


If molecules are moving fast enough, the collisions will result in kinetic energy that can be used to bend, stretch, and eventually break the bonds of the reactants, releasing the potential energy in a usable form.


All reactions eventually form an intermediate that lowers the overall energy requirements of the reaction, resulting in a relatively reasonable activation energy.


Reactants only form products if the activation energy barrier has been exceeded with usable kinetic energy from the system and/or surroundings.

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