1. 2C

2. Copy the title Task C1Equations

3. P7 Match the word symbol and balanced equations For each reaction identify the reactants and products Explain what s l g mean Identify the number and types of atoms in balanced chemical equations

5. In a chemical reaction, reactants usually react to form products products reactants

6. In a reversible reaction, the products of the reactant can react to produce the original reactants products reactants

7. The symbol below represents a reversible reaction products reactants

8. Heating copper sulphate - What happened? • Hydrated copper sulphate is blue. • When it is heated it turns into anhydrous copper sulphate (white) • When this is left to coolit turns back into hydrated copper sulphate. • The reverse reaction is used as a test for water. When water is added • to anhydrous copper sulphate2 things happen: • 1.) White solid turns blue2.) Reaction gives out heat. (Takes in) Heat Endothermic Anhydrous Copper Sulphate (White Solid) Hydrated Copper Sulphate (Blue Solid) (Cool + Steam) Exothermic

9. P7 Explain what irreversible and reversible reactions are Types of reactions- reversible or irreversible • What is a reversible reaction? • Draw the symbol that represents reversible reactions: • What happens to blue hydrated copper sulphate when it is heated? • What happens to anhydrous copper sulphate when it is left to cool and a little water is added? • What type of reaction is this?

10. P7 Explain what a neutralisation reaction is Give an example Write the word and symbol equation Types of reactions- neutralisation • Draw a diagram and explain what a neutralisation reaction is • Explain if it is reversible or irreversible • Write down the word equation • Copy the symbol equation below and explain everything that it tells us • H2SO4 (aq) + 2NaOH (aq)  Na2SO4 (aq) + 2H20 (l)

11. P7 Explain what the reactivity series is Types of reactions- displacement • Draw the diagram above • Explain which is the most reactive and which is the least reactive

12. P7 Explain what displacement is using your knowledge of the reactivity series Types of reactions- displacement • Draw a before and after diagram • Explain what happens in this displacement reaction • Explain if it is reversible or irreversible • Copy down the word and symbol equation below • Fe(s) + CuSO4(aq) --> FeSO4(aq) + Cu(s)

13. P7 Explain what displacement is using your knowledge of the reactivity series Types of reactions- displacement • Draw a before and after diagram • Explain what happens in this displacement reaction • Explain if it is reversible or irreversible

14. Displacement experiment

15. Copy the title Task C2Equations

17. P6 Using the following slides fill in the summary sheet Factors affecting the rate of a reaction

19. Temperature

20. Changing temperature

21. high temp Low temp • Less energy • Particles move slowly • Less collisions • Slow rate of reaction • More energy • Particles move faster • More frequent successful collisions • faster rate of reaction

22. Changing temperature Graphs Increasing the temperature increases the speed of the reacting particles so that they collide more frequently and more energetically. This increases the rate of reaction

23. Changing temperature Summary

24. Concentration

25. Magnesium and hydrochloric acid

26. Changing concentration Increasing the concentration of reactants in solutions increases the frequency of collisions and so increases the rate of reaction.

27. High conc Low conc • Less frequent collisions • Slower rate of reaction • More frequent successful collisions • Faster rate of reaction

28. Changing concentration

29. Pressure

30. Effect of pressure on rate of reaction lower pressure higher pressure As the pressure increases, the space in which the gas particles are moving becomes smaller. The gas particles become closer together, increasing the frequency of collisions. This means that the particles are more likely to react.

31. Surface area

32. Changing surface area Increasing the surface area of solid reactants increases the frequency of collisions and so increases the rate of reaction.

33. Changing surface area

34. Catalysts

35. What are catalysts? Ea withoutcatalyst energy (kJ) Ea withcatalyst reaction (time) Catalysts are substances that change the rate of a reaction without being used up in the reaction. Catalysts never produce more product – they just produce the same amount more quickly. Different catalysts work in different ways, but most lower the reaction’s activation energy (Ea).

36. P6 Copy the graph and explain what it shows A rate of reaction graph

37. P6 Explain why the rat graph curves A rate of reaction graph

38. Copy the title Task C3Industrial processes

39. M5 Answer the questions in full sentences Rates and industry- Margarine • Margarine is made in food factories from vegetable oils. Hydrogen gas is bubbled through the liquid oil. When the hydrogen reacts with the liquid vegetable oil it hardens to form a solid fat. This process is hydrogenation. • At room temperature there is no reaction and hydrogenation doesn’t happen. • But the rate of reaction can be increased by using: • A nickel catalyst (lowers activation energy and speeds up the reaction) • A temperature of 175-190C (which increased the number of successful collisions) • A high pressure (which increases the number of successful collisions) • The higher the temperature, pressure and catalyst increase the rate of reaction What raw product is used to make margarine? What happens when hydrogen is bubbled through he liquid oil? What 3 factors can increase the rate of reaction? Explain how each of these factors increases the rate of reaction

40. M5 Answer the questions in full sentences Rates and industry- Making smells • The chemical Methanol CH3OH is used to make a compound that smells like apple and pineapple. • The way that Methanol is made is below • Carbon monoxide + Hydrogen  methanol • CO (g) + 2H2 (g)  CH3OH (l) • The rate of reaction can be increased by • Increasing the temperature to 250 C (this increases the chance of successful collisions) • A pressure of 50-100 atmospheres (this forces the reactants to collide more often as they are pushed closer together) • Using a catalyst made from copper zinc oxide and aluminium oxide (this lowers the activation energy and increases the rate of reaction) Why is methanol useful? Write down the word and symbol equations. And explain which one are reactants and products What happens when hydrogen is bubbled through he liquid oil? What 3 factors can increase the rate of reaction? Explain how each of these factors increases the rate of reaction

41. H H H H H N N N M5 Answer the questions in full sentences Rates and industry- The HABER PROCESS for producing AMMONIA • The production of ammonia is a very important process as it is used to make fertilizers to grow more food crops. • Ammoniais made from: • nitrogen, which is removed from the air • hydrogen, made from methane (natural gas) • To give the best yeild of ammonia a temperature of 450°C and a pressure of 200 atmospheres is used. The Haber Process is a reversible reaction where both reactants and the product are GASES. What is the formula for ammonia? Why is ammonia important? What are the 2 reactants for making ammonia? What are the 2 conditions to make the most amount of ammonia?

42. hydrogen + nitrogen ammonia HYDROGEN NITROGEN AMMONIA % YIELD = % AMMONIA in main reaction vessel HYDROGEN & NITROGEN IN TEMPERATURE and PRESSURE of the reaction vessel can be controlled UNUSED HYDROGEN & NITROGEN RECYCLED Mixture cooled here. AMMONIAcondenses M5 Copy the diagram LIQUID AMMONIA REMOVED

43. M6 Copy the 2 key words down Key definitions Yield – • The amount of product made in the reaction Atom economy – • A way of measuring the amount of atoms in the reactants that become useful products