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Starter. Learning Objectives. Increasing the number of collisions between particles increases the rate of reaction How temperature, concentration and surface area affect the rate of reaction. Rates of Reaction & Collision Theory. ANIMATION. COOL PARTICLES. HOT PARTICLES.

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Starter

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  1. Starter 2007

  2. Learning Objectives • Increasing the number of collisions between particles increases the rate of reaction • How temperature, concentration and surface area affect the rate of reaction 2007

  3. Rates of Reaction &Collision Theory ANIMATION 2007

  4. COOL PARTICLES HOT PARTICLES Which reaction is faster? Why? 2007

  5. CONCENTRATED SOLUTION DILUTE SOLUTION Which reaction is faster? Why? 2007

  6. BIG PIECE (small surface area) SMALL PIECES (large surface area) Which reaction is faster? Why? 2007

  7. COUNTDOWN TIMER Your presentation should: • Explain that particle collisions are needed for a reaction • Explain how the number of collisions affects the rate of reaction • Explain how concentration OR temperature OR surface area affect the rate of reaction 2007

  8. Presentations & Feedback 2007

  9. TRUEORFALSE Collision theory helps us to explain rates of reaction 2007

  10. TRUEORFALSE Reaction rates depend on temperature 2007

  11. TRUEORFALSE Reactions will speed up if they are heated 2007

  12. TRUEORFALSE Dilute solutions of reactants will react faster than concentrated solutions of reactants 2007

  13. TRUEORFALSE Reactions slow down if they are diluted 2007

  14. TRUEORFALSE A powdered reactant will react slower than a solid lump of reactant 2007

  15. TRUEORFALSE A larger surface area decreases the number of useful collisions 2007

  16. TRUEORFALSE When particles collide they always react 2007

  17. Temperature Concentration Surface Area There are more particles to collide There is a bigger surface area for other particles to collide with Particles move faster and so there are more collisions and collisions have more energy “Match of the Day” 2007

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