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ELECTROCHEMISTRY Chap 20
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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+] = M; [Fe2+] = M Ans = −0.058 V (b) [Cd2+] = M; [Fe2+] = 1.0 M; Ans = V
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Calculate the cell potential for:
In Class Exercise: Calculate the cell potential for: Cu │ CuCl2 ( M) ║ AgNO3 ( M) │ Ag Ans = V Calculate the cell potential for: Pt │ UO22+ ( M); U4+ (0.200 M); H+ ( M ║ Fe2+ ( M); Fe3+ ( M) │ Pt Ans = V UO H+ + 2e− → U4+ + 2H2O; Eo = V
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Applications of Oxidation-Reduction Reactions
Batteries and Fuel Cells Corrosion Electrolysis
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Batteries Fig 20.19 A 12 V automobile Fig 20.19 Combining cells
lead-acid battery Fig Combining cells
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Fig 20.21 Cutaway view of a miniature alkaline cell
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Fig 20.24 Corrosion of iron in contact with water
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Fig 20.25 Cathodic protection of iron in contact with zinc
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Fig 20.26 Cathodic protection of an iron water pipe
Figure 20-26 Title: Cathodic protection of an iron water pipe. Caption: A mixture of gypsum, sodium sulfate, and clay surrounds the magnesium anode to promote conductivity of ions. The pipe, in effect, is the cathode of a voltaic cell. Notes: Keywords:
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Fig 20.27 Electrolysis of molten sodium chloride
Figure 20-27 Title: Electrolysis of molten sodium chloride. Caption: Cl– ions are oxidized to Cl2(g) at the anode, and Na+ ions are reduced to Na(l) at the cathode. Notes: Keywords:
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