Electrolysis

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15 Terms

1
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what happens at anode - Electrolysis of molten Lead Bromide

  • 2Br → Br 2 + 2e-

  • oxidation

  • bromide ions have been reduced

2
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what happens at cathode - Electrolysis of molten Lead Bromide

(negative)

  • Pb2+ + 2e- → Pb

  • reduction

3
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what is given off at anode - Electrolysis of molten Lead Bromide

Bromine gas (orange)

4
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what accumulates at cathode

molten Bromine

5
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what is electrolyte?

ionic substance (melted/in solution split by electrolysis

6
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what are electrodes made out of, why?

  • made of graphite

  • inert so doesn’t interact with reaction

7
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what are the two rules - electrolysis of solutions

Now we have H2O → splits to give H+ (cathode) and OH- (anode) ions

  1. CATHODE

    • competition between metal hydrogen ion + hydrogen ion

    • MOST reactive STAYS in solution

  2. ANODE

    • is there a halide/group 7 ion

    • yes → that halogen is formed

    • no → oxygen is formed

8
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half equation for formation of oxygen at anode

4OH- → O2 + 2H2O + 4e-

9
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CuSO4 electrolysis anode/cathode

Anode - bubbles of gas, oxygen formed

cathode - pink/brown solid coating, copper formed

10
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H2SO4 electrolysis anode/cathode

anode - bubbles of gas, oxygen formed

cathode - bubbles of gas, hydrogen formed

11
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NaCl

anode - bubbles of gas, chlorine formed

cathode - bubbles of gas, hydrogen formed

12
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electrolysis - why should circuit not be connected for more than a few minutes

they may produce toxic gas e.g. chlorine

13
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why is there a light in the electrolysis circuit

to ensure it is working

14
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why are copper, sodium and hydrogen ions attracted to the cathode?

they are positive ions and the cathode is negative - opposite charges attract

15
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where does the H+ and the OH- come from in the experiment

the solution that is being tested - water splits into the ions