1. What is ? Collision theory? Rate of reaction Activation energy?
Factors affecting?
Collision theory?
Rate of reaction
Activation energy?
Energy level diagram?
Effective collision?

2. Quiz
Using collision theory, explain how these factors affect the rate of reaction
Size of reactant
Temperature
Concentration
Catalyst
2) Draw activation energy with and without catalyst

3. What is the rate of a reaction
The rate of reaction is how quickly a reaction happens.
Slow reaction
Fast reaction

4. Iron rusting - a CHEMICAL REACTION with a slow reaction rate.
Wood burning - a chemical reaction with a fast reaction rate.

5. What is ? Collision theory? Rate of reaction Activation energy?
Factors affecting?
Collision theory?
Rate of reaction
Activation energy?
Energy level diagram?
Effective collision?

6. "You can’t react if you don’t collide."
collision theory
"You can’t react if you don’t collide."

7. 3 necessary requirements in order for a reaction to take place:
the particles must collide to react.
2. Collision of particles must produce enough energy (to overcome energy of activation)
3. Collisions of particles must be correctly oriented

8. What is ? Collision theory? Rate of reaction Activation energy?
Factors affecting?
Collision theory?
Rate of reaction
Activation energy?
Energy level diagram?
Effective collision?

9. Prevent Effective collision
Camera to detect fast moving traffic

12. Effective collision

13. What is ? Collision theory? Rate of reaction Activation energy?
Factors affecting?
Collision theory?
Rate of reaction
Activation energy?
Energy level diagram?
Effective collision?

14. Activation energy
The energy that must be overcome in order for a chemical reaction to occur
Activation energy is the minimum energy necessary for a specific chemical reaction to occur

15. Activation energy
The sparks generated by striking steel against a flint provide the activation energy to initiate combustion in this Bunsen burner.

16. A little activation energy is added with the aid of a weed burner...
What is activation energy
A little activation energy is added with the aid of a weed burner...

17. Not enough kinetic energy for reactants to leap over reaction barrier.
What is activation energy
A "hot" reaction in progress showing reactants leaping over the activation energy barrier
Not enough kinetic energy for reactants to leap over reaction barrier.

18. Activation energy

19. Activation energy

20. What is activation energy
Only collisions with enough energy react to form products.
The critical amount of energy to make the reaction proceed

21. A B  C + D
reactants
products

22. What is activation energy

23. What is ? Collision theory? Rate of reaction Activation energy?
Factors affecting?
Collision theory?
Rate of reaction
Activation energy?
Energy level diagram?
Effective collision?

24. What affects the rate of a reaction?
Size of reactant
Temperature of reaction mixture
Concentration of reactants
/pressure
catalyst

25. What affects the rate of a reaction?
1. The effect of size of reactant

26. 1. The effect of size of reactant

27. THE EFFECT OF SIZE OF REACTANT
a reaction between magnesium metal and a dilute acid like hydrochloric acid.
Increasing the number of collisions per second increases the rate of reaction.

28. THE EFFECT OF SIZE OF REACTANT
Magnesium metal

29. THE EFFECT OF SIZE OF REACTANT
Magnesium metal

30. 1. The effect of size of reactant
Reducing the size of reactant
increases the Total Surface Area
increases the frequency of collisions
between particles
Increase the frequency effective
collisions between particles
Increase the rate of reaction.

31. Increasing temperature will increase kinetic energy in the particles

32. 1. The effect of temperature
Increase the temperature of solution
increase the kinetic energy of particles
increase the frequency of collisions
between particles
Increase the frequency effective
collisions between particles
Increase the rate of reaction.

33. 3. Concentration and Pressure
Increasing concentration or pressure increases the number of particles per unit volume

35. 1. The effect of concentration
Increase the concentration of solution
increase the number of particles per unit volume
increase the frequency of collisions
between particles
Increase the frequency effective
collisions between particles
Increase the rate of reaction.

36. Properties of Catalysts
A catalyst will change the rate of a reaction. - The catalyst itself does not take part in the reaction - It is not changed by the reaction
it is not used up during the reaction. - A catalyst is usually a transition metal, a transition metal oxide

37. How does a catalyst work?
Provides a surface on which the reaction can take place.
This increases the number of collisions between the particles of the substances that are reacting.

38. 4. Catalyst
Often a catalyst is there to provide a favourable surface for a reaction to take place
The black object represents the catalyst

39. Decomposition of hydrogen peroxide manganese(IV) oxide, MnO2
Examples CATALYSTS
reaction
catalyst
Decomposition of hydrogen peroxide
manganese(IV) oxide, MnO2
Manufacture of ammonia by the Haber Process
iron
Contact Process to make sulphuric acid
vanadium(V) oxide, V2O5

40. A catalyst provides an alternative route for the reaction with a a lower activation energy.

41. Activation energy with no catalyst

42. Activation energy with catalyst

43. 4. The effect of catalyst Catalyst provides alternative route
That has a lower activation energy
So more particles have energy equal or
greater than activation energy.
Number of effective collisions increase.
Increase the rate of reaction.

44. What is ? Collision theory? Rate of reaction Activation energy?
Factors affecting?
Collision theory?
Rate of reaction
Activation energy?
Energy level diagram?
Effective collision?

47. End of slides