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Understanding Collision Theory in Kinetics: Simulation and Diagram

Learn the principles of Collision Theory in chemistry: how temperature affects particle collisions, energy diagrams, activation energy, and successful reactions. Explore simulations and diagrams to grasp the concept effectively.

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Understanding Collision Theory in Kinetics: Simulation and Diagram

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  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 collidemore often and with more energy. 3. In chemical reactionsbonds 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. Collision Energy Diagram Simulation 100 % Percent of Collisions With Energy 0 % Low Collision energy High

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

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

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

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

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

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

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

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

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

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

  14. 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:

  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 products no 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 Hardercollisions

  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- The catalyst KI is added to H2O2, food colouring, and dishwashing detergent. The O2 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 H2 and O2do 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 H2 and O2do not react at room temperature. Ea is too highfor the room temperature collisions A small spark ignites causes an explosion.

  42. Explain each Scenario Using the Collision Theory 1. A balloon full of H2 and O2do not react at room temperature. Ea is too highfor 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 highfor 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 highfor 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 highfor 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. H2O2 decomposes very slowly at room temperature. 2H2O2(aq) → O2(g) + 2H2O(l) KI increases the reaction rate dramatically.

  48. Explain each Scenario Using the Collision Theory 3. H2O2 decomposes very slowly at room temperature. 2H2O2(aq) → O2(g) + 2H2O(l) KI increases the reaction rate dramatically.

  49. Explain each Scenario Using the Collision Theory 3. H2O2 decomposes very slowly at room temperature. 2H2O2(aq) → O2(g) + 2H2O(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. H2O2 decomposes very slowly at room temperature. 2H2O2(aq) → O2(g) + 2H2O(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

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