Faraday's Second Law of Electrolysis describes the relationship between the quantities of different substances deposited at electrodes when the same amount of charge is passed through different electrolytic solutions.
Faraday's First Law states that the mass of a substance deposited is directly proportional to the charge passed. Faraday's Second Law compares different substances at the same charge.
"When the same quantity of electricity is passed through different electrolytes connected in series, the masses of substances deposited at the respective electrodes are directly proportional to their equivalent masses (chemical equivalents)."
Mathematically:
m₁/m₂ = E₁/E₂
Where:
The Equivalent Mass (or Chemical Equivalent) is calculated as:
Equivalent Mass = Molar Mass / Valency (n-factor)
Example: If you pass the same charge through aqueous CuSO₄ and AgNO₃:
For every 32 g of copper deposited, 108 g of silver will be deposited simultaneously.
It is used in **electroplating** industries to precisely calculate how much of a metal (like gold or silver) will be deposited on an object for a given amount of current and time.
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