Point 1 of 12 — Lesson 3: Electrolysis, Faraday’s Laws and Industrial ApplicationsQuestion bank: 1 questions (1 with pictures)
01The electrolytic cell
Anelectrolytic cellis a cell in whichelectrical energy from an external source is converted into chemical energyby driving anon-spontaneousredox reaction.
It consists of a container with an electrolyte (a solution of a salt, acid or base, or a molten salt) and two electrodes (of the same material such as graphite or platinum, or of different materials such as carbon, copper, zinc).
The electrode joined to thepositive pole of the external source is the anode — it attracts anions andoxidationoccurs there.
The electrode joined to thenegativepole is thecathode — it attracts cations andreductionoccurs there.
Electrolytes conduct by movement ofions (ionic conductors), unlike metals, which conduct by movement of electrons (electronic conductors).
Liquid electrolytes are of two kinds: solutions of acids, bases or salts, and molten salts.
In this course we study the electrolysis of molten salts and of solutions of salts of metals that come after hydrogen in the series.
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