1. Balance Redox Rxns: Fe(OH) 3 + [Cr(OH) 4 ] -1 Fe(OH) 2 + CrO 4 -2 in base

2. Electrochemistry

3. Metallic Conduction The flow of electrons through a metal

4. Ionic Conduction The movement of ions (electrolytes) through a solution Electrolytic Conduct.

5. Electrode The surface or point in which oxidation or reduction takes place

6. Anode The electrode where oxidation takes place An Ox (-)

7. Cathode The electrode where reduction takes place Red Cat (+)

8. Voltaic or Galvanic Cell Electrochemical Cell in which:

9. a spontaneous oxidation-reduction reaction produces electrical energy

10. Half-Cell A cell where only oxidation or only reduction takes place

11. An electrochemical cell must have two half-cells connected by a salt bridge

12. A half-cell will not work by itself Both half-cells are required

13. Salt Bridge 1) Allows electrical contact between the two half-cells

14. 2) Prevents mixing of the two half- cell solutions

15. 3) Allows ions to flow maintaining electrical neutrality

16. Determining the Redox Rxn & Voltage of an Electrochemical Cell

17. Identify all molecules & ions (reactants) that exist in the electrolytic cell

18. 1) Determine all possible half- reactions that could occur in the system

19. 2 ) Look up each half-rxn from the Std. Redox Tables

20. 3) Record each half-rxn & its standard voltage

21. 4) Save the oxidation half- rxn that has the highest voltage

22. 5) Save the reduction half- rxn that has the highest voltage

23. 6) Balance the electrons between the two half-rxns

24. 7) Add the two half-rxns to obtain the full electrochemical reaction

25. 7) Add the voltage of each half-rxn to obtain the std. voltage required

26. Voltaic Cell Problems

27. Determine all when a cell with a Cu electrode in CuCl 2(aq) is connected to a cell with a Zn electrode in ZnBr 2(aq)

28. Determine all when a cell with a Fe electrode in FeCl 3(aq) is connected to a cell with a Mn electrode in MnCl 2(aq)

29. Determine all when a cell with a Mg electrode in Mg(NO 3 ) 2(aq) is connected to a cell with a Au electrode in Au(NO 3 ) 3 (aq)

31. Electrolysis Using electricity to force a non- spontaneous electrochemical rxn

32. Electrolytic Cell Chemical cell where electrolysis is being performed

33. How to determine the Redox Rxn & voltage of an Electrolytic Cell

34. Identify all molecules & ions (reactants) that exist in the electrolytic cell

35. 1) Determine all possible half- reactions that could occur in the system

36. 2 ) Look up each half-rxn from the Std. Redox Tables

37. 3) Record each half-rxn & its standard voltage

38. 4) Save the oxidation half- rxn that has the highest voltage

39. 5) Save the reduction half- rxn that has the highest voltage

40. 6) Balance the electrons between the two half-rxns

41. 7) Add the two half-rxns to obtain the full electrochemical reaction

42. 7) Add the voltage of each half-rxn to obtain the std. voltage required

43. Determine the rxn that takes place when 1.5 V is passed through two Pt electrodes in a solution containing MgI 2(aq) & ZnCl 2(aq)

44. Determine the rxn that takes place when 2.5 V is passed through two Pt electrode in a solution of NaCl (aq) 0

45. Determine the rxn that takes place when 2.0 V& 9.65 A is passed for 2.5 Hrs through two Pt electrodes in a solution containing MnBr 2(aq) & AlF 3(aq)

46. Relating Equations  G o =  H o - T  S o  G o = -RTlnK eq  G o = -nF E o

47. Nernst Equation E = E o - (RT/nF)lnQ for non-standard conditions

48. Determine the voltage of a cell with a silver electrode in 1.0 M AgNO 3 & an iron electrode in 0.10 M Fe(NO 3 ) 2 at 27 o C

49. Determine the voltage of a cell with a silver electrode in 1.0 M AgNO 3 & a zinc electrode in 0.010 M Zn(NO 3 ) 2 at 27 o C

50. Determine the voltage of a cell with a copper electrode in 0.10 M CuNO 3 & a zinc electrode in 1.0 M Zn(NO 3 ) 2 at 27 o C

51. Electroplating & Electro-purifying

52. Electrolysis During electrolysis, oxidation & degradation would occur at the anode while reduction & electroplating would occur at the cathode

53. Current Formula Current = charge/unit time Amps = coul/sec Amount (mass, volume, moles, etc) can be determined from the charge

54. Calculate the mass of copper plated onto the cathode when a 9.65 mAmp current is applied to a solution of CuSO 4 for 5.0 minutes.

55. Calculate the years required to plate 216 kg onto the cathode when a 96.5 mAmp current is applied to a solution of AgNO 3

56. Calculate the current required to purify 510 kg of aluminum oxide in 5.0 hours

57. Calculate the time required to electroplate 19.7 mg of gold onto a plate by passing 965 mA current through a solution of Au(NO 3 ) 3

58. Calculate the time required to gold plate a 2.0 mm layer onto a 250 cm 2 by passing 965 mA current through a solution of Au(NO 3 ) 3 (D Au = 20 g/cm 3 )

59. Calculate the time required to purify a 204 kg of ore that is 60.0 % Al 2 O 3 by applying a 965 kA current through molten ore sample:

60. Calculate the time required to purify a 32 kg of ore that is 75.0 % Fe 2 O 3 by applying a 9.65 kA current through molten ore sample:

61. Determine the voltage of a cell with a silver electrode in 5.0 M AgNO 3 & an zinc electrode in 0.25 M Zn(NO 3 ) 2 at 27 o C