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15 cards from this deck
Theory explaining reaction rates based on particle collisions
Particles collide, sufficient energy, correct orientation
Collision with enough energy & orientation forming products
Particles must collide in correct orientation for reaction to occur
Spread of kinetic energies among gas molecules
Minimum energy colliding particles need for reaction
Few molecules have sufficient energy; slow reaction rate
More molecules have enough energy; faster reaction rate
Highest energy point where bonds break & form (transition state)
Products lower energy than reactants; heat released
Products higher energy than reactants; heat absorbed
More particles have energy above activation energy threshold
More particles, closer together; more frequent collisions
Greater surface area; more frequent effective collisions
Provides alternative pathway with lower activation energy
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