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A reaction that takes a long time to complete has a high rate of reaction.
If the frequency of collisions between particles increases, the rate of reaction increases.
A collision must have enough energy to break chemical bonds for it to be effective.
A chemical reaction with a high activation energy will generally be faster than one with a low activation energy.
Activation energy is the minimum amount of energy required for a reaction to occur.
All collisions that overcome the activation energy result in a chemical reaction.
Lowering the activation energy of a reaction will generally slow down the reaction.
The rate of a chemical reaction is independent of the energy of the collisions between reacting particles.