1. Rates Of Reaction Flow Of Learning

4. Concentration

5. Temperature

6. Catalyst -The meaning of Collision Theory. -To explain how each factor increases

8. Experiment On Effect Of Concentration

9. Experiment On Effect Of Temperature

10. Experiment On Effect Of CatalystIs proven by

11. How KFC can cook Fried chicken in quickly?

12. Application of The Rate Of reaction In daily Activities

13. Observable changes in quantity that use to determine rate of reaction Meaning rate of reaction Unit for rate of reaction Avarage rate of reaction Measurement Rate Of Reaction Rate Of reaction at specific time Factors that affect rate of reaction Rate Of Reaction

14. Rate Speed = total Distance/Total time K.L J.B

15. Speed= Speed= = = = 100km/h = 300km/h

16. Reaction Types 2 1 Chemical Bonds are made / broken Change in oxidation states Plasma Li +1 P+1 P+1

17. Chemical properties/ changes/ reactions (i.e., reactivity, combustibility). development of a gas, formation of precipitate, and change in color). Reactivity Combustibility Gas formation Precipitate Color change

18. Hydrogen-VERY reactive. Helium-Non-reactive.

20. The weathering of rocks is an extremely very slow reaction. weathering of rocks

21. The fermentation of sugar to alcohol is quite slow but you can see the carbon dioxide bubbles forming in the 'froth' in a laboratory experiment or beer making in industry! Bubble gas

24. evidence of Chemical Change: development of a gas formation of precipitate change in color

25. Meaning Of Rate Of Reactions The rate of reaction is a measurement of the change in the quantity of reactant or product against time: Rate Of Reaction= Change in quantity of reactant / product Time taken Student ans: Changes of reactant or product against time (0 Mark)

26. Meaning Of Rate Of Reaction A rate of reaction is high if the reaction occurs fast within a short period of time.. A rate of reaction is low if the reaction occurs slowly within a long period of time.. A rate of reaction is inversely proportional to time: Rate of reaction α 1 time taken

27. Meaning Of Rate Of Reactions The Higher rate of reaction the shorter time taken to complete the reaction The lower rate of reaction the longer time taken to complete reaction granule powder 5 minute 1 minute Which is the higher rate of reaction?

28. CaCO3 (s) + 2HCl (aq) -> CaCl2 (aq) + H2O + CO2 (g)

29. CaCO3 (s) + 2HCl (aq) -> CaCl2 (aq) + H2O + CO2 (g)

31. Increase in total amount of mass / concentration of the product of reaction per unit of time

32. Total volume of the gas released.

34. Increase in total amount of mass / concentration of the product of reaction per unit of time

35. Total volume of the gas released. CaCO3 (s) + 2HCl (aq) -> CaCl2 (aq) + H2O + CO2 (g) Deliverytube Conical flask burette water Must shade!

36. Formation of precipitate. Na2SO3+2HCl->NaCl+S+SO2+H20 PERCIPITATE stopwatch

37. Precipitatethe formation of insoluble ionic compounds. Does NOT dissolve in water.

38. Example:Study the reaction: Between calcium carbonate and excess 1 mol dm-3 hydrochloride acid.CaCO3 (s) + 2HCl (aq) -> CaCl2 (aq) + H2O + CO2 (g)

39. CaCO3 (s) + 2HCl (aq) -> CaCl2 (aq) + H2O + CO2 (g)

40. Observable changes CaCO3 (s) + 2HCl (aq) -> CaCl2 (aq) + H2O + CO2 (g) stopwatch

41. Observable changes CaCO3 (s) + 2HCl (aq) -> CaCl2 (aq) + H2O + CO2 (g) Hydrometer

42. Observable changes CaCO3 (s) + 2HCl (aq) -> CaCl2 (aq) + H2O + CO2 (g) Hydrometer

43. Observable changes CaCO3 (s) + 2HCl (aq) -> CaCl2(aq) + H2O + CO2 (g) Displacement Of water

46. Introduction to the Rate of Reaction A reaction between small pieces of excess calcium carbonate with 80 cm3 hydrochloric acid 0.05M is conducted a laboratory to study the rate of reaction at interval time. The volume of gas released is recorded in the table below.

47. 40 40 30 30 27.00cm3 37.00cm3 Volume : 37-27=10 cm3

48. (a) Draw an apparatus to shows how this experiment can be conducted at laboratory. Must label the diagram!

49. x x

50. √ √

51. √ √

52. (b) Write a balance chemical equation for this reaction. CaCO3 (s) + 2HCl (aq) -> CaCl2(aq) + H2O + CO2 (g)

53. (c) CaCO3 + 2HCl -> CaCl2 + H2O + CO2 CaCO3 + 2H++2Cl- -> Ca2++2Cl- + H2O + CO2 CaCO3 + 2H++ -> Ca2++ H2O + CO2 Remember !!! Only separate soluble salt Don’t separate covalentand insoluble salt

54. (d) Carbon dioxide gas

55. (e) A reaction between small pieces of excess calcium carbonate with 80 cm3hydrochloric acid 0.05M is conducted a laboratory to study the rate of reaction at interval time. Number of mole in the solution will use : MV Mol, n = 1000 0.05(80) = 1000 = 0.004 mol

56. (f) CaCO3 + 2HCl -> CaCl2 + H2O + CO2 From the chemical equation : Mole Ratios: 2 mol HCl : 1 mol CO2 0.004 mol HCl : 0.004 mol HCl × 1 mol CO2 2 mol HCl = 0.002 mol CO2 Volume of gas Co2 at room condition = 0.002×24 0.048 dm3 =

57. (g) Because some of carbon dioxide gas can escape to surrounding during the experiment.

58. (h)

59. Volume of CO2, cm3 Connect the point without using ruler! Not all the point is connected Time , s

60. Volume of CO2 cm3 Cannot like this graph Straight line It’s must be smooth graph Time s

61. (i) Average Rate Of reaction The average rate of reaction in the first 90 seconds. = The total volume of gas released in the first 90 seconds Time taken 33.5÷90=0.372 cm3s-1 unit = Not cm3 per second

62. i(ii) The average rate of reaction in the whole experiment. = The total volume of gas released in the whole experiment Time taken 47.5÷180= 0.264cm3s-1 =

63. (h) Volume of gas against time y x α How to fit your scale in graph? For y: use ratio 5: 10 Check it’s enough by 5÷10=0.5 Maximum volume 47.5÷0.5=95 small boxes How about x:? 30÷10=3 Maximum 240÷3=80small boxes

64. Analysis of Data Rate of reaction at t second = gradient AB = p/q cm3 s-1 Total volume of Hydrogen gas/cm3 Tangent is a line that touch just 1 point of graph in order to calculate gradient B Tangent p A q Cannot take directly at x t Time (second)

65. Tangent Cannot touch more than 2 point because each of point have different gradient Only touch 1 point of curve

66. tangent α

67. Analysis of data Total Volume of CO2(cm3) F D E Rate of reaction at t1 = gradient AB B Rate of reaction at t2 = gradient CD C Rate of reaction at t3 = gradient EF Each of point have different gradient! A t1 t3 t2 Time (second)

68. Two method to calculate tangent: Total volume of Hydrogen gas/cm3 number of small boxes ×value of 1 small unit box B Tangent Y A X Time (second)

69. First Method Gradient of graph: Total volume of Hydrogen gas/cm3 m = ΔY ΔX B m = Y2-y1 y2 X2-x1 Tangent A y1 Time (second) x1 x2

70. Analysis of Data Rate of reaction at t second = gradient AB = p/q cm3 s-1 Total volume of Hydrogen gas/cm3 B Tangent p A q t Time (second)

71. Analysis of data Total Volume of CO2(cm3) F D E Rate of reaction at t1 = gradient AB B Rate of reaction at t2 = gradient CD C Rate of reaction at t3 = gradient EF A t1 t3 t2 Time (second)

72. From the answer of question (i) (iii) and (i) (iv), make a conclusion from the calculation of this experiment. (j) Ans : Rate of reaction will decreases

73. (k) Explain why does there is a difference of the rate of reaction at 30 second and 120 second. Ans: Rate of reaction at 30 second is higher because number of particles of reactant is higher than 120 second

76. The temperature of acid is increased.

77. A bigger conical flask is used.

78. The conical flask containing acid is shaken.