1. Kinetics Lesson 3 Collision Theory

2. The Collision Theory Link to Simulation of Molecular Motion 1.Matter consists of moving particles. 2.As the temperature increases the particles move faster and collide more often and with more energy. 3.In chemical reactions bonds must be broken and new ones formed. 4.The energy for this comes from particle collisions. 5.The collisions have a variety of energy, as some are harder than others. 6.A collision energy diagram is a graph of the number of the collisions versus the energy of each collision.

3. Low Collision energy High 100 % Percent of Collisions With Energy 0 % Collision Energy Diagram SimulationSimulation

4. Low Collision energy High Collision Energy Diagram Activation Energy Ea- minimum energy required for a successful collision- to break the bonds! 100 % Percent of Collisions With Energy 0 %

5. Low Collision energy High Collision Energy Diagram Activation Energy Ea- minimum energy required for a successful collision- too break the bonds! 100 % Percent of Collisions With Energy 0 %

6. Low Collision energy High Collision Energy Diagram Activation Energy Ea- minimum energy required for a successful collision- too break the bonds! 100 % Percent of Collisions With Energy 0 % This area represents the fraction of collisions that do not have the Ea- not successful.

7. Low Collision energy High Collision Energy Diagram Activation Energy Ea- minimum energy required for a successful collision- too break the bonds! 100 % Percent of Collisions With Energy 0 % This area represents the fraction of collisions with the Ea -successful.

8. What happens to the number of successful collisions if we add a catalyst, which lowers the activation energy Ea? Watch!

9. Low Collision energy High Collision Energy Diagram Activation Energy Ea- minimum energy required for a successful collision- too break the bonds! 100 % Percent of Collisions With Energy 0 % This area represents the fraction of collisions with the Ea -successful.

10. Low Collision energy High Collision Energy Diagram Activation Energy Ea- minimum energy required for a successful collision- too break the bonds! 100 % Percent of Collisions With Energy 0 % Lowering the Ea increases successful collisions!

11. What happens to the number of successful collisions if we increase the temperature- so that the average collision energy is greater? Watch!

12. Low Collision energy High Collision Energy Diagram Activation Energy Ea- minimum energy required for a successful collision- too break the bonds! 100 % Percent of Collisions With Energy 0 %

13. Low Collision energy High Collision Energy Diagram Activation Energy Ea- minimum energy required for a successful collision- too break the bonds! 100 % Percent of Collisions With Energy 0 % Increasing the temperature increases successful collisions- increases rate! Push the graph down and right!

14. Collision Theory You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires:

15. Collision Theory Collision Theory You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires:

16. Collision Theory You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 1.Favourable Geometry

17. Collision Theory You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 1.Favourable Geometry products

18. Collision Theory You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 1.Favourable Geometry versus Poor Geometry products

19. Collision Theory You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 1.Favourable Geometry versus Poor Geometry products

20. Collision Theory You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 1.Favourable Geometry versus Poor Geometry products

21. Collision Theory You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 1.Favourable Geometry versus Poor Geometry products

22. Collision Theory You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 1.Favourable Geometry versus Poor Geometry no products products

23. Collision Theory You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 1.Favourable Geometry versus Poor Geometry products no products

24. Collision Theory You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 2.Sufficient Energy to break the chemical bonds

25. Collision Theory You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 2.Sufficient Energy to break the chemical bonds

26. Collision Theory You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 2.Sufficient Energy to break the chemical bonds

27. Collision Theory You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 2.Sufficient Energy to break the chemical bonds Activation energy is the minimum amount of energy required for a successful collision.

28. The Collision Theory can be used to explain how the rate of a reaction can be changed. Reaction rates can increase due to 1.More collisions 2.Harder collisions- greater collision energy 3.Lower activation energy or Ea, which allows low energy collisions to be more effective. And that’s it!

29. The Collision Theory can be used to explain how the rate of a reaction can be changed. 1.Increasing the temperature increases the rate because there are:

30. The Collision Theory can be used to explain how the rate of a reaction can be changed. 1.Increasing the temperature increases the rate because there are: More frequent collisions

31. The Collision Theory can be used to explain how the rate of a reaction can be changed. 1.Increasing the temperature increases the rate because there are: More frequent collisions Harder collisions

32. The Collision Theory can be used to explain how the rate of a reaction can be changed. 2.Increasing the reactant concentration increases the rate because there are:

33. The Collision Theory can be used to explain how the rate of a reaction can be changed. 2.Increasing the reactant concentration increases the rate because there are: More frequent collisions

34. The Collision Theory can be used to explain how the rate of a reaction can be changed. 3.Adding a catalyst increases the rate because:

35. The Collision Theory can be used to explain how the rate of a reaction can be changed. 3.Adding a catalyst increases the rate because Lower activation energy or Ea, which allows low energy collisions to be successful Movie-Movie- The catalyst KI is added to H 2 O 2, food colouring, and dishwashing detergent. The O 2 produced makes foam.

36. The Collision Theory can be used to explain how the rate of a reaction can be changed. 4.Changing the nature of the reactant for a more reactive chemical changes the rate because

37. The Collision Theory can be used to explain how the rate of a reaction can be changed. 4.Changing the nature of the reactant for a more reactive chemical changes the rate because Lower activation energy or Ea, which allows low energy collisions to be more effective

38. The Collision Theory can be used to explain how the rate of a reaction can be changed. 5.Increasing the surface area of a solid reactant increases the rate because:

39. The Collision Theory can be used to explain how the rate of a reaction can be changed. 5.Increasing the surface area of a solid reactant increases the rate because: More frequent collisions

40. Explain each Scenario Using the Collision Theory 1.A balloon full of H 2 and O 2 do not react at room temperature. A small spark ignites causes an explosion.

41. Explain each Scenario Using the Collision Theory 1.A balloon full of H 2 and O 2 do not react at room temperature. Ea is too high for the room temperature collisions A small spark ignites causes an explosion.

42. Explain each Scenario Using the Collision Theory 1.A balloon full of H 2 and O 2 do not react at room temperature. Ea is too high for the room temperature collisions A small spark ignites causes an explosion. The spark provides the Ea and it explodes because it is exothermic

43. Explain each Scenario Using the Collision Theory 2.A candle does not burn at room temperature A match causes the candle to burn. The candle continues to burn

44. Explain each Scenario Using the Collision Theory 2.A candle does not burn at room temperature Ea is too high for the room temperature collisions A match causes the candle to burn. The candle continues to burn

45. Explain each Scenario Using the Collision Theory 2.A candle does not burn at room temperature Ea is too high for the room temperature collisions A match causes the candle to burn. The match provides the Ea The candle continues to burn

46. Explain each Scenario Using the Collision Theory 2.A candle does not burn at room temperature Ea is too high for the room temperature collisions A match causes the candle to burn. The match provides the Ea The candle continues to burn It burns because it is exothermic

47. Explain each Scenario Using the Collision Theory 3.H 2 O 2 decomposes very slowly at room temperature. 2H 2 O 2(aq) → O 2(g) + 2H 2 O (l) KI increases the reaction rate dramatically.

48. Explain each Scenario Using the Collision Theory 3.H 2 O 2 decomposes very slowly at room temperature. 2H 2 O 2(aq) → O 2(g) + 2H 2 O (l) KI increases the reaction rate dramatically.

49. Explain each Scenario Using the Collision Theory 3.H 2 O 2 decomposes very slowly at room temperature. 2H 2 O 2(aq) → O 2(g) + 2H 2 O (l) KI increases the reaction rate dramatically. KI is a catalyst as it is not a reactant and it speeds up the rate.

50. Explain each Scenario Using the Collision Theory 3.H 2 O 2 decomposes very slowly at room temperature. 2H 2 O 2(aq) → O 2(g) + 2H 2 O (l) KI increases the reaction rate dramatically. KI is a catalyst as it is not a reactant and it speeds up the rate. Lowers the activation energy or Ea, which allows low energy collisions to be more effective

51. Describe and Graph the Relationship between the Following Ea and the rate Ea Rate

52. Describe and Graph the Relationship between the Following Ea and the rate Decreasing the Ea increases the rate- inverse. Ea Rate

53. Describe and Graph the Relationship between the Following Ea and the rate Decreasing the Ea increases the rate- inverse. Ea Rate

54. Describe and Graph the Relationship between the Following Temperature and the rate Temp Rate

55. Describe and Graph the Relationship between the Following Temperature and the rate Increasing the temperature increases the rate- direct. Temp Rate

56. Describe and Graph the Relationship between the Following Temperature and the rate Increasing the temperature increases the rate- direct. Temp Rate

57. Describe and Graph the Relationship between the Following Concentration and the rate Conc Rate

58. Describe and Graph the Relationship between the Following Concentration and the rate Increasing the concentration increases the rate- direct. Conc Rate

59. Describe and Graph the Relationship between the Following Concentration and the rate Increasing the concentration increases the rate- direct. Conc Rate

60. Describe and Graph the Relationship between the Following Ea and the temperature Ea Temp

61. Describe and Graph the Relationship between the Following Ea and the temperature The only way to change the Ea is by adding a catalyst! No relationship! Ea Temp

62. Describe and Graph the Relationship between the Following Ea and the temperature The only way to change the Ea is by adding a catalyst! No relationship! Ea Temp