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

*F*= 96,485.3365(21) C/mol.

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

where:

*e*≈ 1.6021766×10−19 C;*N*_{A}≈ 6.022141×1023 mol−1.

*N*_{A} 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. Research is continuing into more accurate ways of determining the interrelated constants *F*, *N*_{A}, and *e*.

Read more about Faraday Constant: Other Common Units of Faraday's Constant, Faraday Unit of Charge

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