A mole of electrons is given a special name: 1 Faraday. The charge of 1 mole of electrons is called the Faraday Constant, F.
It is calculated by multiplying the charge of one electron by the Avogadro constant.
1 Faraday = 9.648 70 x 104, coulombs/faraday (C mol-1).
In electrolysis, Michael Faraday in 1832 - 1833 discovered the relationship between the charge and the quantity of matter liberated in an electrode reaction. He did not know about partial reactions at electrodes, electrons, or a unit (to be) named after him. He did know something about atomic and molecular masses. His results are summarised in two laws, now famous as Faraday's laws.
2 faradays produce 1 mol of H2:
2H+ + 2e- ® H2
1 faraday produces 1 mol of Ag:
Ag+ + e- ® Ag
3 faradays produce 1 mol of Al:
Al3+ + 3e- ® Al
That one mole of atoms or molecules always requires an integral number of faradays suggests a once novel but now familiar idea: the existence of a natural unit of charge, the charge of an electron.
See also Avogadro Constant | The Mole