1 / 10

ELECTROCHEMISTRY Chap 20

ELECTROCHEMISTRY Chap 20. Nernst Equation for a Complete Reaction. E cell = E + − E − = E cathode − E anode. Only valid when both ½-rxns written as reductions. Given: Cd ( s ) │ Cd(NO 3 ) 2 ( aq ); M A ║ FeCl 2 (aq); M C │ Fe ( s)

osmond
Download Presentation

ELECTROCHEMISTRY Chap 20

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. ELECTROCHEMISTRY Chap 20

  2. Nernst Equation for a Complete Reaction Ecell = E+ − E− = Ecathode − Eanode • Only valid when both ½-rxns written as reductions • Given: • Cd (s) │ Cd(NO3)2 (aq); MA ║ FeCl2 (aq); MC │ Fe (s) • [Cd2+] = 0.50 M; [Fe2+] = 0.10 M Ans = −0.058 V • (b) [Cd2+] = 0.010 M; [Fe2+] = 1.0 M; Ans = +0.021 V

  3. In Class Exercise: Calculate the cell potential for: Cu │ CuCl2 (0.0200 M) ║ AgNO3 (0.0200 M) │ Ag Ans = +0.410 V Calculate the cell potential for: Pt │ UO22+ (0.0150 M); U4+ (0.200 M); H+ (0.0300 M ║ Fe2+ (0.0100 M); Fe3+ (0.0250 M) │ Pt Ans = +0.638 V UO22+ + 4H+ + 2e−→ U4+ + 2H2O;Eo= +0.334 V

  4. Applications of Oxidation-Reduction Reactions • Batteries and Fuel Cells • Corrosion • Electrolysis

  5. Batteries Fig 20.19 A 12 V automobile lead-acid battery Fig 20.19 Combining cells

  6. Fig 20.21 Cutaway view of a miniature alkaline cell

  7. Fig 20.24 Corrosion of iron in contact with water

  8. Fig 20.25 Cathodic protection of iron in contact with zinc

  9. Fig 20.26 Cathodic protection of an iron water pipe

  10. Fig 20.27 Electrolysis of molten sodium chloride

More Related