2. Unit 1 Kinetics Reaction Rates Read Hebdon Chapter 1

3. Introduction Chemical Kinetics

4. Introduction Chemical Kinetics is the study of the rates of chemical reactions.

5. Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate =

6. Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product

7. Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product Δ in Time

8. Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product Δ in Time Δ means change State of Reactant or ProductAmountUnit

9. Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product Δ in Time Δ means change State of ReactantAmountUnit (s)

10. Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product Δ in Time Δ means change State of ReactantAmountUnit (s)mass

11. Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product Δ in Time Δ means change State of ReactantAmountUnit (s)massg

12. Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product Δ in Time Δ means change State of ReactantAmountUnit (s)massg (g)

13. Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product Δ in Time Δ means change State of ReactantAmountUnit (s)massg (g)volume

14. Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product Δ in Time Δ means change State of ReactantAmountUnit (s)massg (g)volumemL, or L

15. Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product Δ in Time Δ means change State of ReactantAmountUnit (s)massg (g)volumemL, or L (aq)

16. Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product Δ in Time Δ means change State of ReactantAmountUnit (s)massg (g)volumemL, or L (aq) concentration

17. Introduction Chemical Kinetics is the study of the rates of chemical reactions. Reaction Rate = Δ in Amount of Reactant or Product Δ in Time Δ means change State of ReactantAmountUnit (s)massg (g)volumemL, or L (aq) concentrationM

18. Time Units

19. Time Unitssecondsminuteshours

20. Time Unitssecondsminuteshours Rate Units

21. Time Unitssecondsminuteshours Rate Unitsg/minmL/hmoles/s

22. Measuring Reaction Rates Reactants→Products

23. Measuring Reaction Rates Reactants→Products Decrease.

24. Measuring Reaction Rates Reactants→Products Decrease Increase as you measure them.

25. CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change

26. CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change

27. CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change

28. CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massof CaCO 3(s)

29. CaCO 3(s) +HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massg

30. CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease

31. CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease

32. CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease Concentration

33. CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationM

34. CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease

35. CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease

36. CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease

37. CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease Volume

38. CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease VolumemL

39. CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease VolumemLincrease

40. CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease VolumemLincrease

41. CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease VolumemLincrease Concentration

42. CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease VolumemLincrease ConcentrationM

43. CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease VolumemLincrease ConcentrationMincrease

44. CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease VolumemLincrease ConcentrationMincrease

45. CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease VolumemLincrease ConcentrationMincrease

46. CaCO 3(s) +2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Property MeasuredUnits Change Massgdecrease ConcentrationMdecrease VolumemLincrease ConcentrationMincrease The water concentration does not change enough to measure. It increases as does a drop in a bucket.

47. 1.Volume of H 2 Zn (s) + 2HCl (aq) → H 2(g) + ZnCl 2(aq) Diagram Volume (mL) Time (s) 01530456075

48. 1.Volume of H 2 Zn (s) + 2HCl (aq) → H 2(g) + ZnCl 2(aq) Diagram Volume (mL) 4.05.15.96.87.68.3 Time (s) 01530456075

49. Calculations Rate in mL H 2 /s=8.3 - 4.0 mL = 75 s

50. Calculations Rate in mL H 2 /s=8.3 - 4.0 mL =0.057 mL/s 75 s Rate in mole H 2 /min @ STP 0.057 mL s

51. Calculations Rate in mL H 2 /s=8.3 - 4.0 mL =0.057 ml/s 75 s Rate in mole H 2 /min @ STP 0.057 mL x 1 L x s 1000 mL

52. Calculations Rate in mL H 2 /s=8.3 - 4.0 mL =0.057 ml/s 75 s Rate in mole H 2 /min @ STP 0.057 mL x 1 L x 1 mole s 1000 mL 22.4 L

53. Calculations Rate in mL H 2 /s=8.3 - 4.0 mL =0.057 ml/s 75 s Rate in mole H 2 /min @ STP 0.057 mL x 1 L x 1 mole x 60 s= s 1000 mL 22.4 L 1 min

54. Calculations Rate in mL H 2 /s=8.3 - 4.0 mL =0.057 ml/s 75 s Rate in mole H 2 /min @ STP 0.057 mL x 1 L x 1 mole x 60 s= 1.5 x 10 -4 mole/min s 1000 mL 22.4 L 1 min

55. Calculations Rate in mL H 2 /s=8.3 - 4.0 mL =0.057 ml/s 75 s Rate in mole H 2 /min @ STP 0.057 mL x 1 L x 1 mole x 60 s= 1.5 x 10 -4 mole/min s 1000 mL 22.4 L 1 min Rate in g HCl/h

56. Calculations Rate in mL H 2 /s=8.3 - 4.0 mL =0.057 ml/s 75 s Rate in mole H 2 /min @ STP 0.057 mL x 1 L x 1 mole x 60 s= 1.5 x 10 -4 mole/min s 1000 mL 22.4 L 1 min Rate in g HCl/h 1.5 x 10 -4 mole H 2 min

57. Calculations Rate in mL H 2 /s=8.3 - 4.0 mL =0.057 ml/s 75 s Rate in mole H 2 /min @ STP 0.057 mL x 1 L x 1 mole x 60 s= 1.5 x 10 -4 mole/min s 1000 mL 22.4 L 1 min Rate in g HCl/h 1.5 x 10 -4 mole H 2 x 2 moles HCl min 1 mole H 2

58. Calculations Rate in mL H 2 /s=8.3 - 4.0 mL =0.057 ml/s 75 s Rate in mole H 2 /min @ STP 0.057 mL x 1 L x 1 mole x 60 s= 1.5 x 10 -4 mole/min s 1000 mL 22.4 L 1 min Rate in g HCl/h 1.5 x 10 -4 mole H 2 x 2 moles HCl x 36.5 g min 1 mole H 2 1 mole

59. Calculations Rate in mL H 2 /s=8.3 - 4.0 mL =0.057 ml/s 75 s Rate in mole H 2 /min @ STP 0.057 mL x 1 L x 1 mole x 60 s= 1.5 x 10 -4 mole/min s 1000 mL 22.4 L 1 min Rate in g HCl/h 1.5 x 10 -4 mole H 2 x 2 moles HCl x 36.5 g x 60 min min 1 mole H 2 1 mole1 h

60. Calculations Rate in mL H 2 /s=8.3 - 4.0 mL =0.057 ml/s 75 s Rate in mole H 2 /min @ STP 0.057 mL x 1 L x 1 mole x 60 s= 1.5 x 10 -4 mole/min s 1000 mL 22.4 L 1 min Rate in g HCl/h 1.5 x 10 -4 mole H 2 x 2 moles HCl x 36.5 g x 60 min = 0.67 g/h min 1 mole H 2 1 mole1 h

61. 2.Mass of an open container CaCO 3(s) + 2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Diagram Mass (g) 82.0781.8481.7181.6681.6481.63 Time (s) 01530456075

62. 2.Mass of an open container CaCO 3(s) + 2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Diagram 1. Calculate the rate in units of grams CO 2 /s.

63. 2.Mass of an open container CaCO 3(s) + 2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Diagram 1. Calculate the rate in units of grams CO 2 /s. Rate=(82.07 - 81.63) g =0.0059 g/s 75 s

64. 2.Mass of an open container CaCO 3(s) + 2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Diagram 1. Calculate the rate in units of grams CO 2 /s. Rate=(82.07 - 81.63) g =0.0059 g/s 75 s 2.Calculate the rate in grams CaCO 3 /h

65. 2.Mass of an open container CaCO 3(s) + 2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Diagram 1. Calculate the rate in units of grams CO 2 /s. Rate=(82.07 - 81.63) g =0.0059 g/s 75 s 2.Calculate the rate in grams CaCO 3 /h 0.0059 g CO 2 s

66. 2.Mass of an open container CaCO 3(s) + 2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Diagram 1. Calculate the rate in units of grams CO 2 /s. Rate=(82.07 - 81.63) g =0.0059 g/s 75 s 2.Calculate the rate in grams CaCO 3 /h 0.0059 g CO 2 x 1 mole s 44.0 g

67. 2.Mass of an open container CaCO 3(s) + 2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Diagram 1. Calculate the rate in units of grams CO 2 /s. Rate=(82.07 - 81.63) g =0.0059 g/s 75 s 2.Calculate the rate in grams CaCO 3 /h 0.0059 g CO 2 x 1 mole x 1 mole CaCO 3 s 44.0 g 1 mole CO 2

68. 2.Mass of an open container CaCO 3(s) + 2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Diagram 1. Calculate the rate in units of grams CO 2 /s. Rate=(82.07 - 81.63) g =0.0059 g/s 75 s 2.Calculate the rate in grams CaCO 3 /h 0.0059 g CO 2 x 1 mole x 1 mole CaCO 3 x 100.1 g s 44.0 g 1 mole CO 2 1 mole

69. 2.Mass of an open container CaCO 3(s) + 2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Diagram 1. Calculate the rate in units of grams CO 2 /s. Rate=(82.07 - 81.63) g =0.0059 g/s 75 s 2.Calculate the rate in grams CaCO 3 /h 0.0059 g CO 2 x 1 mole x 1 mole CaCO 3 x 100.1 g x 3600 s s 44.0 g 1 mole CO 2 1 mole 1 h

70. 2.Mass of an open container CaCO 3(s) + 2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Diagram 1. Calculate the rate in units of grams CO 2 /s. Rate=(82.07 - 81.63) g =0.0059 g/s 75 s 2.Calculate the rate in grams CaCO 3 /h 0.0059 g CO 2 x 1 mole x 1 mole CaCO 3 x 100.1 g x 3600 s = 48 g/h s 44.0 g 1 mole CO 2 1 mole 1 h

71. 3.Pressure in a closed container Ca (s) +2HOH (l) → Ca(OH) 2(aq) + H 2(g) Diagram

72. 4.Colour of Solution Cu (s) +2AgNO 3(aq) →2Ag (s) +Cu(NO 3 ) 2(aq) clear blue

73. 5. If 0.895 g of H 2 SO 4 is neutralized with 0.50 M NaOH in 30.0 seconds, what is the reaction rate in moles NaOH /min. H 2 SO 4 + 2NaOH →

74. 5. If 0.895 g of H 2 SO 4 is neutralized with 0.50 M NaOH in 30.0 seconds, what is the reaction rate in moles NaOH /min. H 2 SO 4 + 2NaOH → The wording of the question tells you that all 0.895 g is used up and some portion of the 0.50 M is consumed. Rate=

75. 5. If 0.895 g of H 2 SO 4 is neutralized with 0.50 M NaOH in 30.0 seconds, what is the reaction rate in moles NaOH /min. H 2 SO 4 + 2NaOH → The wording of the question tells you that all 0.895 g is used up and some portion of the 0.50 M is consumed. Rate=0.895 g H 2 SO 4

76. 5. If 0.895 g of H 2 SO 4 is neutralized with 0.50 M NaOH in 30.0 seconds, what is the reaction rate in moles NaOH /min. H 2 SO 4 + 2NaOH → The wording of the question tells you that all 0.895 g is used up and some portion of the 0.50 M is consumed. Rate=0.895 g H 2 SO 4 x 1 mole 98.1 g

77. 5. If 0.895 g of H 2 SO 4 is neutralized with 0.50 M NaOH in 30.0 seconds, what is the reaction rate in moles NaOH /min. H 2 SO 4 + 2NaOH → The wording of the question tells you that all 0.895 g is used up and some portion of the 0.50 M is consumed. Rate=0.895 g H 2 SO 4 x 1 mole x 2 moles NaOH 98.1 g 1 mole H 2 SO 4

78. 5. If 0.895 g of H 2 SO 4 is neutralized with 0.50 M NaOH in 30.0 seconds, what is the reaction rate in moles NaOH /min. H 2 SO 4 + 2NaOH → The wording of the question tells you that all 0.895 g is used up and some portion of the 0.50 M is consumed. Rate=0.895 g H 2 SO 4 x 1 mole x 2 moles NaOH 98.1 g 1 mole H 2 SO 4 0.500 min

79. 5. If 0.895 g of H 2 SO 4 is neutralized with 0.50 M NaOH in 30.0 seconds, what is the reaction rate in moles NaOH /min. H 2 SO 4 + 2NaOH → The wording of the question tells you that all 0.895 g is used up and some portion of the 0.50 M is consumed. Rate=0.895 g H 2 SO 4 x 1 mole x 2 moles NaOH 98.1 g 1 mole H 2 SO 4 0.500 min =0.036 moles NaOH/min