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

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Presentation on theme: "What is ? Effective collision? Collision theory? Factors affecting? Activation energy? Energy level diagram? Rate of reaction."— Presentation transcript:

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

2 Quiz 1)Using collision theory, explain how these factors affect the rate of reaction a)Size of reactant b)Temperature c)Concentration d)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. Fast reaction Slow reaction

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

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

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

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

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

9 Prevent Effective collision Camera to detect fast moving traffic

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12 Effective collision

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

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

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

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

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

18 Activation energy

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

21 A + B  C + D reactants products

22 What is activation energy activation energy

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

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

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

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 Magnesium metal THE EFFECT OF SIZE OF REACTANT

29 Magnesium metal THE EFFECT OF SIZE OF REACTANT

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 rate of reaction. Increase the frequency effective collisions between particles

31 2. Temperature 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 rate of reaction. Increase the frequency effective collisions between particles

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

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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 rate of reaction. Increase the frequency effective collisions between particles

36 - 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 Properties of Catalysts

37 4. Catalyst How does a catalyst work? 1)Provides a surface on which the reaction can take place. 2)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 Examples CATALYSTS reaction catalyst Decomposition of hydrogen peroxide manganese(IV) oxide, MnO 2 Manufacture of ammonia by the Haber Process iron Contact Process to make sulphuric acid vanadium(V) oxide, V 2 O 5

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 Increase the rate of reaction. So more particles have energy equal or greater than activation energy. Number of effective collisions increase.

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

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