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.

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