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Ch17 z5e electrochem

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Electrochemistry pp Applications of Redox
17.1 Galvanic Cells ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Applications ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
[object Object],[object Object],H + MnO 4 - Fe +2
Galvanic Cell H + MnO 4 - Fe +2 Salt Bridge allows current to flow
Galvanic Cell H + MnO 4 - Fe +2 Electrons flow in the wire, ions flow through the salt bridge
[object Object],[object Object],H + MnO 4 - Fe +2 e -
H + MnO 4 - Fe +2 Porous Disk
Reducing Agent Oxidizing Agent e - e - e - e - e - e - Oxidation at Anode Reduction at Cathode
Cell Potential ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
17.2 Standard Reduction Potentials ,[object Object],[object Object],[object Object],[object Object],[object Object]
Zn +2 SO 4 -2 1 M HCl Anode 0.76 1 M ZnSO 4 H + Cl - H 2 in Cathode
Standard Hydrogen Electrode ,[object Object],[object Object],[object Object],1 M HCl H + Cl - H 2 in
Z5e 841 Figure 17.5: Zn/H Galvanic Cell. Notice the electron flow also.
Cell Potential ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Z5e 842 Fig 17.6 Zn/Cu Galvanic Cell
Cell Potential pp ,[object Object],[object Object],[object Object],[object Object],[object Object]
Cell Potential pp ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Cell Potential pp ,[object Object],[object Object],[object Object],[object Object]
Cell Potential ,[object Object],[object Object],[object Object]
Cell Potential ,[object Object],[object Object],[object Object],[object Object],[object Object]
Line Notation pp ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Complete Galvanic Cell Description (AP Test) pp ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Practice pp ,[object Object],[object Object]
Practice - Item 1 pp ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Practice - Item 2 pp ,[object Object],[object Object],[object Object]
Practice - Item 3 pp ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Practice - Item 4 pp ,[object Object],[object Object],[object Object],[object Object],[object Object]
pp Figure 17.7: A Schematic of the previous Galvanic Cell Eº = 1.95 v Be able to draw this as well as write the line notation for the AP exam.
17.3 Cell Potential, Work &  G ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Potential, Work and  G pp ,[object Object],[object Object],[object Object],[object Object]
Potential, Work and  G ,[object Object],[object Object],[object Object],[object Object]
Putting It Together pp ,[object Object],[object Object],[object Object],[object Object],[object Object]
Putting It Together pp ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
17.4 Cell Potential and Concentration pp ,[object Object],[object Object],[object Object],[object Object]
17.4 Cell Potential and Concentration pp ,[object Object],[object Object],[object Object]
Cell Potential pp ,[object Object],[object Object],[object Object]
Cell Potential pp ,[object Object],[object Object],[object Object]
Cell Potential pp ,[object Object],[object Object],[object Object],[object Object]
Le Chatelier, ∆G, & Concentration Cells ,[object Object],[object Object],[object Object]
Le Chatelier, ∆G, & Concentration Cells pp ,[object Object],[object Object],[object Object]
The Nernst Equation ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
The Nernst Equation continued ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
The Nernst Equation pp ,[object Object],[object Object],[object Object]
We’ll do “a,” “b,” & “c”. pp
E cell when [Ag 1+ ] on the right = 1.0 M pp ,[object Object],[object Object],[object Object],[object Object]
E cell when [Ag 1+ ] on the right = 2.0 M pp ,[object Object],[object Object],[object Object],[object Object],[object Object]
E cell when [Ag 1+ ] on the right = 0.10 M pp ,[object Object],[object Object],[object Object],[object Object],You will have a test question on this and it is NOT on the pre-test, so . . . Do p. 832 #53!!
E cell when [Ag 1+ ] on the right = 0.10 M pp ,[object Object],[object Object],[object Object],[object Object],[object Object],You will have a test question on this and it is NOT on the pre-test, so . . . Do p. 832 #53!!
The Nernst Equation ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Nernst Equation & K pp ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Nernst Equation & K pp ,[object Object],[object Object],[object Object]
17.5 Batteries are Galvanic Cells ,[object Object],[object Object],[object Object]
Figure 17.13 One of the Six Cells in Storage Battery a 12-V Lead Storage Battery
Batteries are Galvanic Cells ,[object Object],[object Object],[object Object],[object Object]
Figure 17.14 A Common Dry Cell Battery
17.6 Corrosion ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Water Rust Iron Dissolves - Fe  Fe +2 e - Salt speeds up process by increasing conductivity
Figure 17.17 The Electrochemical Corrosion of Iron
Preventing Corrosion ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Preventing Corrosion ,[object Object],[object Object]
Figure 17.18 Cathodic Protection
[object Object],[object Object],[object Object],[object Object],[object Object],17.7 Electrolysis
1.0 M Zn +2 e - e - Anode Cathode 1.10 Zn Cu 1.0 M Cu +2 Galvanic Cell - spontaneous
1.0 M Zn +2 e - e - Anode Cathode A battery >1.10V Zn Cu 1.0 M Cu +2 Electrolytic Cell Forces the opposite reaction.
Figure 17.19 (a) A Standard Galvanic Cell (b) A Standard Electrolytic Cell
Calculating plating ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Calculating plating pp ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Calculating plating pp ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Calculating plating pp ,[object Object],[object Object],[object Object]
Calculating plating pp ,[object Object],[object Object],[object Object],[object Object]
Calculating plating pp ,[object Object],[object Object]
Calculating plating pp ,[object Object],***** ,[object Object]
Calculating plating pp ,[object Object],[object Object],[object Object],[object Object]
Calculating plating pp ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Calculating plating pp ,[object Object],[object Object],[object Object],[object Object]
Calculating plating ,[object Object],[object Object],[object Object],[object Object]
Calculating plating ,[object Object],[object Object]
Other uses pp ,[object Object],[object Object],[object Object],[object Object]
Relative Oxidizing Abilities pp ,[object Object],[object Object],[object Object],[object Object],[object Object]

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Ch17 z5e electrochem

  • 1. Electrochemistry pp Applications of Redox
  • 2.
  • 3.
  • 4.
  • 5. Galvanic Cell H + MnO 4 - Fe +2 Salt Bridge allows current to flow
  • 6. Galvanic Cell H + MnO 4 - Fe +2 Electrons flow in the wire, ions flow through the salt bridge
  • 7.
  • 8. H + MnO 4 - Fe +2 Porous Disk
  • 9. Reducing Agent Oxidizing Agent e - e - e - e - e - e - Oxidation at Anode Reduction at Cathode
  • 10.
  • 11.
  • 12. Zn +2 SO 4 -2 1 M HCl Anode 0.76 1 M ZnSO 4 H + Cl - H 2 in Cathode
  • 13.
  • 14. Z5e 841 Figure 17.5: Zn/H Galvanic Cell. Notice the electron flow also.
  • 15.
  • 16. Z5e 842 Fig 17.6 Zn/Cu Galvanic Cell
  • 17.
  • 18.
  • 19.
  • 20.
  • 21.
  • 22.
  • 23.
  • 24.
  • 25.
  • 26.
  • 27.
  • 28.
  • 29. pp Figure 17.7: A Schematic of the previous Galvanic Cell Eº = 1.95 v Be able to draw this as well as write the line notation for the AP exam.
  • 30.
  • 31.
  • 32.
  • 33.
  • 34.
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  • 36.
  • 37.
  • 38.
  • 39.
  • 40.
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  • 42.
  • 43.
  • 44.
  • 45. We’ll do “a,” “b,” & “c”. pp
  • 46.
  • 47.
  • 48.
  • 49.
  • 50.
  • 51.
  • 52.
  • 53.
  • 54. Figure 17.13 One of the Six Cells in Storage Battery a 12-V Lead Storage Battery
  • 55.
  • 56. Figure 17.14 A Common Dry Cell Battery
  • 57.
  • 58. Water Rust Iron Dissolves - Fe  Fe +2 e - Salt speeds up process by increasing conductivity
  • 59. Figure 17.17 The Electrochemical Corrosion of Iron
  • 60.
  • 61.
  • 62. Figure 17.18 Cathodic Protection
  • 63.
  • 64. 1.0 M Zn +2 e - e - Anode Cathode 1.10 Zn Cu 1.0 M Cu +2 Galvanic Cell - spontaneous
  • 65. 1.0 M Zn +2 e - e - Anode Cathode A battery >1.10V Zn Cu 1.0 M Cu +2 Electrolytic Cell Forces the opposite reaction.
  • 66. Figure 17.19 (a) A Standard Galvanic Cell (b) A Standard Electrolytic Cell
  • 67.
  • 68.
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