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Electrochemistry review

Electrochemistry review. 6. Electrode- definitions on pages 613-614 Anode- Cathode-. 13. Mg is +2, Cl is -1. 16. K  e - + K + oxidation, occurs at anode Cu 2+ +e -  Cu + reduction, occurs at cathode Br 2 +2e - 2Br - reduction, occurs at cathode. 17.

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Electrochemistry review

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  1. Electrochemistry review

  2. 6 • Electrode- definitions on pages 613-614 • Anode- • Cathode-

  3. 13 Mg is +2, Cl is -1

  4. 16 • K  e- + K+ oxidation, occurs at anode • Cu2+ +e-  Cu+ reduction, occurs at cathode • Br2 +2e- 2Br- reduction, occurs at cathode

  5. 17 • Ca  Ca2+ • Cl2 2Cl- • Redox • Ca (oxidation #0) + Cl2 (oxidation #0)  CaCl2

  6. 22 • Cathode: absorbs electrons • Anode: releases electrons • Cd  Cd2+ + 2e- • Ag+ + e-  Ag • Balancing: Cd + 2Ag+ + 2e-  Cd2+ +2Ag +2e-

  7. 25

  8. 33

  9. 58 • AgCl(s) + e- -> Ag(s) + Cl-(aq) 0.222V (Cath) • 2H3O+(aq) + 2e- -> H2(g) 0V (An) • Cath-An

  10. 85 • Ag: 400g/20hrs • Au: 200g/17hrs • Divide total produced by time it took to produce

  11. 86 • Ag: 400g/20hrs ×1mole/107.9g=0.19 mole/hr • Au: 200g/17hrs ×1mole/197g = 0.06 mole/hr

  12. 87/88 • Ag+ + e- Ag 0.19mole/hr; 5.3hrs for 1 mole • Au3+ + 3e-  Au .06mole/hr × 3; 5.6hrs for 1mole

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