The constant equivalent to 96,485 coulombs per mole of electrons is the Faraday constant.
The Faraday constant, represented by F, is the electric charge carried by one mole of elementary charges. Its value is approximately 96,485 coulombs per mole. In practical electrochemistry, it connects the amount of chemical substance involved in a reaction with the quantity of electricity passed through an electrolytic cell.
The constant combines two fundamental quantities: Avogadro’s constant and the elementary charge. In simplified form, F = Nₐe. Because one mole of electrons contains Avogadro’s number of electrons, multiplying that number by the charge of one electron gives the Faraday constant.
Michael Faraday’s work on electrolysis helped establish the relationship between electricity and chemical change, although the modern constant was defined later using precise physical constants. It is often confused with the farad, the SI unit of capacitance. The farad measures a capacitor’s ability to store charge; the Faraday constant measures charge per mole of particles.