1. Kaupapa / Learning Outcomes I can explain what ‘reaction rate’ means andhow to measure the rate of reaction I can explain how reactions happen due to collisions between particles I can explain how surface area, concentration and temperature affect the reaction rate using collision theory

3. Rate of Reaction the speed at which a chemical reaction occurs. Some reactions are quick Some are not The rate of a reaction can be altered

4. Measuring rate of reaction Two common ways: 1)Measure how fast the products are formed Colour change Gas formation 2)Measure how fast the reactants are used up

5. Rate of reaction graph Amount of product formed Time Reaction begins rapidly Slows down as time passes as reactants are used up Stops after a certain time – graph levels out as one (or both) reactants have been used up.

6. Collision Theory “For a reaction between two particles to occur, the particles must collide and the collision must be effective”

7. Effective Collisions When the particles collide with enough kinetic energy and the correct orientation to break the bonds between particles so new bonds can form. Collisions can occur and yet result in no reaction if there is insufficient energy or incorrect orientation.

8. How do reactions occur? Reactions take place when particles collide with a certain amount of energy. Not enough energy – no reaction

9. How do reactions occur? Reactions take place when particles collide with a certain amount of energy. Incorrect orientation – no reaction

10. How do reactions occur? Reactions take place when particles collide with a certain amount of energy. Enough energy and correct orientation – reaction!

11. Activation Energy The minimum amount of energy needed for the particles to react is called the activation energy, and is different for each reaction. If particles collide with less energy than the activation energy, they will not react. Kick-starting Reactions - Activation Energy

12. Collisions and Rate The more frequently effective collisions occur the faster the rate of reaction. Change the concentration of reactants Change the temperature of the reaction Change the surface area of reactants Use a catalyst To change the rate of reaction we can: How to speed up chemical reactions (and get a date).

13. Concentration Increasing the concentration of a reactant increases the number of particles per volume. This increases the frequency of collisions. Which increases the rate of the reaction

14. Surface Area Increasing the surface area of a reactant increases the number of particles available to react. This increases the frequency of collisions which increases the rate of the reaction.

15. Temperature Increasing the temperature of a reaction increases the kinetic energy of the particles. The particles collide more often and with more energy this increases the frequency of effective collisions which increases the rate of reaction

16. In Summary SLOW REACTIONSFAST REACTIONS