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  1. Collision Theory and Rates of Reaction
  2. Collision Theory! In order for a reaction to occur: • Two reactants must collide • The collision must have enough energy
  3. What is the rate of a reaction? • The rate of reaction is the speed at which a reaction occurs or how fast it occurs. • There are certain things that can impact this rate.
  4. Factors that affect the rate of reaction Think! • What are some ways we can increase the speed of a reaction? • And how do these reasons relate to collision theory?
  5. Factors that Affect Rate of Reaction Chemical nature of Reactants Temperature Concentration of Reactants Presence of Catalyst Surface Area Pressure
  6. Chemical nature of Reactants  some reactants are more/less reactive then others Gold is much less reactive then zinc In HCl (aq) Families of elements tend to undergo the same types of reactions, but at different rates
  7. Concentration of Reactants  Higher Concentration = faster reaction • particles more likely to collide
  8. Surface Area of Reactants  Higher Surface Area = greater rate of reaction • Particles more likely to collide
  9. Temperature  Higher Temperature= greater rate of reaction Particles move faster, so more likely to collide
  10. Presence of a Catalyst  A substance that speeds up a reaction without being a reactant or being used up
  11. Pressure  A higher pressure forces the particles closer together. • More chance of particles colliding and reacting.