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(Set 1)

Electrolysis. (Set 1). I) Electrolytic cell. II) Electrolysis of some compounds. A) Solid / molten PbBr 2. B) Aqueous NaCl solution. I) Electrolytic cell. cathode. anode. electrolyte. anion. cation. The cathode is the electrode. negative.

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(Set 1)

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  1. Electrolysis (Set 1)

  2. I) Electrolytic cell II) Electrolysis of some compounds A) Solid / molten PbBr2 B) Aqueous NaCl solution

  3. I) Electrolytic cell cathode anode electrolyte anion cation The cathode is the electrode. negative move towards the cathode. Cations The anode is the electrode. positive move towards the anode. Anions

  4. II) Electrolysis of some compounds A) Electrolysis of solid/molten PbBr2

  5. Solid PbBr2 does not conduct electricity because the ions are not free to move. Molten PbBr2 conducts electricity because the ions are free to move.

  6. At the cathode: Half equation: Pb2+(l) + 2e- Pb(l) Pb2+ ions discharge by electrons gaining This is a reaction reduction

  7. At the anode: Half equation: 2Br-(l)  Br2(g) + 2e- Br- ions discharge by electrons losing This is an reaction oxidation

  8. I am ared cat. I am an ox. Reduction occurs at the cathode. Oxidation occurs at the anode.

  9. B) Electrolysis of aqueous NaCl Ions present: Na+, Cl-,H+, OH- At the cathode: 2H+(aq) + 2e- H2(g) At the anode: 2Cl-(aq)  Cl2(g) + 2e-

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