ELECTROLYSIS
CONTENT
- Faraday’s Laws of Electrolysis
- Calculations
- Uses of Electrolysis and Corrosion of Metals: Corrosion Treated as a Redox Process
- Rusting of Iron and its Economic Costs
- Prevention of Rusting of Iron
Faraday’s Laws of Electrolysis
Faraday’s First Law of Electrolysis
1. Faraday’s first law of electrolysis states that the mass (m) of a substance librated or deposited at an electrode during electrolysis is directly proportional to the quantity (q) of electricity passing through the electrolyte.
Mathematically;
M α Q ————– (1)
The unit of quantity is coulombs (c). It is the product of current in Amperes and time in seconds
Q = It ——————— (2)
M α It
.: M = k It ——————— (3)
Where k = proportionality constant
I = current in ampere (A)
T = time in seconds (S)
It can be shown that the reciprocal of k, which is called charge-to-mass ratio, is Cf/M.
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