, the Faraday constant
(named after Michael Faraday
) is the magnitude of electric charge
. 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
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.
- Mohr, Peter J.; Taylor, Barry N. (2005). "CODATA recommended values of the fundamental physical constants: 2002". Rev. Mod. Phys. 77 (1): 1–107.