Faraday was a British scientist who greatly contributed to the field of electrochemistry.
The mass of a substance liberated at an electrode during electrolysis is directly proportional to the quantity of electricity transferred at that electrode.
W∝ A🞩t
W = ZAt
Where.,
W=amount of deposited or liberated substance. (Grams or g)
Z= constant [Electrochemical equivalent (gram per coulomb or g.C-1)].
A= current (Amperes or A).
T= time (Seconds or sec.)
The weight of the substance collected at the electrodes when one coulomb of electric charge is passed through the electrolyte
The number of different substances deposited or liberated due to the passage of the same quantity of current through different electrolytes is proportional to their chemical equivalent masses.
Equivalent mass or weight = 𝑎𝑡𝑜𝑚𝑖𝑐 𝑤𝑒𝑖𝑔ℎ𝑡/𝑣𝑎𝑙𝑒𝑛𝑐𝑦
The basic unit of electric charge is Faraday.
It is defined as the charge on one mole of an electron.
F=Avogadro’s number 🞩 charge on an electron in coulombs F=6.02🞩1023 mol-1 🞩 1.602192 C
F= 96,484 C.mol-1
Approximately; 1F = 96500 C
