Faraday Constant
The Faraday constant F = Nₐ × e connects the Avogadro number to the elementary charge. It is the central quantity of electrochemistry and describes how much charge is needed to deposit one mole of a substance.
physics.constants
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Exact Value (F)
Exact since 2019 (SI redefinition), since both Nₐ and e are exactly defined.
Formula
Nₐ = 6.022 140 76 × 10²³ mol⁻¹, e = 1.602 176 634 × 10⁻¹⁹ C.
Discovered
Michael Faraday formulated his electrolysis laws in 1832–1833 at the Royal Institution in London.
Application
E = E₀ − (RT/zF) ln Q. Central to battery design, corrosion, and membrane biophysics.
Relations
The Faraday constant and the Planck constant are both exactly defined in the SI system since 2019.
Explanations
The Faraday constant (F = 96.485 C/mol) connects two important numbers from physics: Avogadro's number and the elementary charge. It tells you how much electrical charge is needed to deposit exactly one mole of a substance – for example when charging batteries or electrolyzing water. This constant has been known since 1832–1833 and is the heart of all electrochemical calculations.
Sources
CODATA-Referenzwert der Faraday-Konstante.
Überblick über Faradays Elektrolyse-Gesetze und historischen Kontext.
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Provenance
Status
seed
Review
none
Last Updated
2026-02-17