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18.8 Electrolysis

18.8 Electrolysis. 2 Types of electrochemistry Battery or Voltaic Cell – Purpose? Electrolysis - forces a current through a cell to produce a chemical change that would not otherwise occur. Battery – voltaic cell. Pb + H 2 SO 4  PbSO 4 + 2H + + 2e - Anode

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18.8 Electrolysis

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  1. 18.8 Electrolysis 2 Types of electrochemistry • Battery or Voltaic Cell – Purpose? • Electrolysis - forces a current through a cell to produce a chemical change that would not otherwise occur.

  2. Battery – voltaic cell Pb + H2SO4 PbSO4 + 2H+ + 2e- Anode PbO2 + H2SO4 + 2e- + 2H +  PbSO4 + 2H2O Cathode

  3. Possible oxidation reactions. 2Cl- Cl2 + 2e- 2H2O  O2 + 4H+ + 4e- Possible reduction reactions Na+ + e- Na 2e- + 2H2O  H2 + 2OH- Electrolysis of salt waterNa+, Cl-, and H20 are present

  4. Electrolysis • A process where electrical energy is used to produce a chemical change. • Involves forcing a current through a cell to produce a change that would otherwise not occur. • Electrolysis of water produces hydrogen gas and oxygen gas. • Electrolysis is used to recharge lead storage batteries.

  5. Cu Fe + - Cu2+ Electroplating • A thin layer of one metal is deposited onto another. There is normally only one solution that supplies the metal needed. Cu  Cu2+ + 2e- Cu2+ + 2e-  Cu

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