Faraday constant | |
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![]() Michael Faraday, the constant's namesake | |
Common symbols | F |
SI unit | coulomb per mole (C/mol) |
In SI base units | s⋅A⋅mol−1 |
Derivations from other quantities | F = eNA |
Value | 9.64853321233100184×104 C⋅mol−1 |
In physical chemistry, the Faraday constant (symbol F, sometimes stylized as ℱ) is a physical constant defined as the quotient of the total electric charge (q) by the amount (n) of elementary charge carriers in any given sample of matter: F = q/n; it is expressed in units of coulombs per mole (C/mol). As such, it represents the "molar elementary charge",[1] that is, the electric charge of one mole of elementary carriers (e.g., protons). It is named after the English scientist Michael Faraday. Since the 2019 redefinition of SI base units,[1] the Faraday constant has an exactly defined value, the product of the elementary charge (e, in coulombs) and the Avogadro constant (NA, in reciprocal moles):
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