In physics and chemistry, the Faraday constant (named after Michael Faraday) is the magnitude of electric charge per mole of electrons.[1] It has the currently accepted value

9.64853399(24) x 104 C mol-1.

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

$F\,=\,eN_{A}$

where

e ≈ 1.6021766×10−19 C;[2]
NA ≈ 6.022141×1023 mol−1.[3]

NA is the Avogadro constant (the ratio of the number of particles N to the amount of substance n - a unit mole), and e is the elementary charge or the magnitude of the charge of an electron. 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.

One common use of the faraday constant is electrolysis. One can divide the amount of charge in coulombs by the Faraday constant in order to find the amount (in moles) of the element that has been oxidized.

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.[4] Research is continuing into more accurate ways of determining the interrelated constants F, NA, and e.

## Other Common Units of Faraday's Constant

• 96,485 J (96.485 kJ) per volt gram equivalent
• 23.061 kcal per volt gram equivalent
• 26.801 A·h/mol

Related to Faraday's constant is the "faraday", a unit of electrical charge. It is much less common than the coulomb, but sometimes used in electrochemistry.[5] One faraday of charge is the magnitude of the charge of one mole of electrons, i.e. 96485.3365(21) C.[6]