Faraday constant
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", i.e., 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, 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):
- F = e × NA
- = 1.602176634×10−19 C × 6.02214076×1023 mol−1
- = 9.64853321233100184×104 C⋅mol−1.
| Faraday constant | |
|---|---|
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 |
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