Faraday’s Laws of
Electrolysis
Electrolysis

In the production of elements or refining of
metals or electroplating, it is the amount of
electricity (electric charge) that determined
the masses of substances that react or are
produced at the electrodes.
The Coulomb


The Coulomb (C) measures the amount of
electric charge flowing.
It is the number of electrons passing a given
point.
Ampere





Current is the rate at which charges flow.
It is the number of electrons passing a given
point in a certain amount of time.
Symbol: I
Unit: Ampere (A)
I=q
q = charge (C)
t
t = time (s)
I = current (A)
Ampere

A=C
s
Faraday’s Constant




Faraday discovered the relationship between
Electricity and electrochemical changes.
Faraday’s Constant represents the electric charge
carried on one mole of electrons.
It is equal to 9.648 × 104 coulombs per mole.
The constant is used to calculate the electric charge
needed to discharge a particular quantity of ions
during electrolysis.
Faraday’s Constant




1 mol electrons = 1.0 Faraday
1 mol electrons = 96500 C
∴ 96 500 C = 1.0 Faraday
1 F = 9.65 * 104 C/mol