Faraday's first law: It states that, “The mass of any substance deposited or liberated at any electrode is directly proportional to the quantity of electricity passed.”i.e., m ∝ Q
Where, m = Mass of ions liberated in gm,
Q = Quantity of electricity passed in Coulombs
= Current in Amperes (I) × Time in second (t)
∴ m ∝ I × t or m = Z × I × t
Faraday's second law: It states that, “When the same quantity of electricity is passed through different electrolytes, the masses of different ions liberated at the electrodes are directly proportional to their chemical equivalents (Equivalent weights).” i.e.
W1/W2 = E1/E2 or Z1It/Z2It or Z1/Z2 = E1/E2 (∴ W = ZIt)
Thus the electrochemical equivalent (Z) of an element is directly proportional to its equivalent weight (E), i.e., E ∝ Z or E = FZ or E = 96500 × Z
where, F = Faraday constant = 96500 C mol–1
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