ELECTROLYSIS: Decomposition of an ionic substance by passing an electric current through it
sELECTROLYSIS OF LEAD (II) BROMIDE:
sELECTROLYSIS OF LEAD (II) BROMIDE | ||
Diagram showing the Electrolysis of Lead (II) Bromide | ||
METHOD:
| ||
REACTION AT ELECTRODES: | ||
SOLUTION | PRODUCT AT POSITIVE ELECTRODE | PRODUCT AT NEGATIVE ELECTRODE |
LEAD (II) BROMIDE ( PbBr2 ) | Bromine - Br2 2Br - - 2e- → Br2 | Lead - Pb Pb2+ + 2e- → Pb |
s
ELECTROLYSIS OF AQUEOUS SOLUTIONS:
ssRULES:
s- Aqueous Solutions will Always have Water ( H2O )
Positive Electrode
s- Either Oxygen or Non-Metal will be produced E.g Chlorine, Bromine, Nitrogen
s
Negative Electrode
s- Either Hydrogen or Metal will be produced
- If Metal is above Hydrogen in Reactivity Series, Hydrogen will be produced
- If Metal is below Hydrogen in Reactivity Series, Metal will be produced
ELECTROLYSIS OF AQUEOUS SOLUTIONS | ||
Diagram showing the Electrolysis of Aqueous Solutions | ||
METHOD:
| ||
REACTION AT ELECTRODES: | ||
AQUEOUS SOLUTION | PRODUCT AT POSITIVE ELECTRODE | PRODUCT AT NEGATIVE ELECTRODE |
SODIUM CHLORIDE ( NaCl ) | Chlorine - Cl 2Cl- - 2e- → Cl2 | Hydrogen - H2 2H2O + 2e- → H2 + 2OH- |
DILUTE SULFURIC ACID ( H2SO4 ) | Oxygen - O2 2H2O - 4e- → O2 + 4H+ | Hydrogen - H2 2H+ + 2e- → H2 |
COPPER (II) SULFATE ( CuSO4 ) | Oxygen - O2 2H2O - 4e- → O2 + 4H+ | Copper - Cu Cu2+ + 2e- → Cu |
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