Zumdahl_chapt_17

Zumdahl_chapt_17 - Chapter 17 Electrochemistry 17.1 17.2 17.3 Energy 17.4 17.5 17.6 17.7 17.8 Galvanic Cells Standard Potentials Voltage Work and

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    Chapter 17 Electrochemistry 17.1 Galvanic Cells 17.2 Standard Potentials 17.3 Voltage, Work and Free Energy 17.4 Non-standard conditions 17.5 Batteries 17.6 Corrosion 17.7 Electrolysis 17.8 Commercial Processes
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    Which way is downhill?  Electrochemistry Chemical Energy  Electrical Energy Galvanic cell Spontaneous chemical reaction to produce electrical work
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    Nomenclature LEO the Lion says GER! Loss of Electrons means Oxidation. Gain of  Electrons means Reduction
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    Nomenclature Anode Negative Oxidation. D E Cathode Positive Reduction
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    Oxidation Half Reactions  H 2 (g) + 2OH -    2H 2 O(l) + 2e - NO(g) + 2H 2 O(l)    NO 3 - (aq) + 4H + + 3e - 2I - (aq)    I 2 (s) + ___e - Sn 2+  Sn 4+ + ___e - Fe(s)   Fe 2+ (aq) + ___e -
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    Reduction Half Reactions Fe 3+ + e -    Fe 2+ Ag + + e -  Ag(s) AgCl(s) + ___e -  Ag(s) + Cl - F 2 (g) + ___e -    2F - (aq)
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    More Nomenclature Line notation Anode salt bridge Cathode on the left on the right A single vertical line denotes a phase boundary solid liquid solid gas liquid gas
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    More Nomenclature Line notation A double vertical line   denotes a salt bridge anode  cathode site of oxidation  site of reduction negative electrode    positive electrode
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    Reading galvanic cell line notation Fe(s) Fe 2+ (aq)  Ag + (aq) Ag(s) Zn(s) Zn 2+ (aq)  H + (aq) H 2 (g) Pt(s) Electrodes need not be involved in the electrochemical reaction. Common passive electrodes include forms of graphite and platinum.
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    Reading galvanic cell line notation Pt(s) I 2 (s) I - (aq)  Ag + (aq)  Ag(s) C(s) H 2 (g) H + (aq)  OH - (aq) O 2 (g)  Pt(s) Pt(s) Sn 4+ (aq),Sn 2+ (aq)  Cl - (aq) Hg 2 Cl 2 (s) Hg (l)
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    Calculating cell potential   The overall cell reaction is the sum of the reduction half reaction and the oxidation half reaction
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  Calculating cell potential   We cannot measure the potential of a half reaction, why not? but we can measure the overall cell potential for a cell
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This note was uploaded on 10/26/2008 for the course CHEM 105BL taught by Professor Warshel during the Summer '07 term at USC.

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Zumdahl_chapt_17 - Chapter 17 Electrochemistry 17.1 17.2 17.3 Energy 17.4 17.5 17.6 17.7 17.8 Galvanic Cells Standard Potentials Voltage Work and

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