Definitions

In physics and chemistry, the Faraday constant (named after Michael Faraday) is the magnitude of electric charge per mole of electrons. The Faraday constant, denoted F, is widely used in calculations in electrochemistry, and has the currently accepted value:

F = 96 485.3399(24) C/mol

The constant F has a simple relation to two other physical constants:

F = Ne
where NA is the Avogadro constant (approximately 6.02 mol−1) and e is the elementary charge, the magnitude of the charge on an electron (approximately 1.602 C). This relation is true because the amount of charge of a mole of electrons is equal to the amount of charge in one electron, multiplied by the number of electrons in a mole.

The value of F was first determined by weighing the amount of silver deposited in an electrochemical reaction in which a measured current was passed for a measured time, and using Faraday's law of electrolysis. Research is continuing into more accurate ways of determining the interrelated constants F, NA, and e.