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10 cards from this deck
How and why reactions occur at different rates
Energy barrier reactants must overcome to form products
Collision, sufficient energy, correct orientation
Collision unsuccessful, no reaction occurs
Particles bounce apart, remain as unreacted reactants
Increases collisions per unit volume per unit time
Average KE directly proportional to absolute temperature (K)
Spread of kinetic energies among gas molecules
Larger fraction of molecules has energy exceeding EaE_aEa
Determines if bonds can break and new bonds form
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