The Faraday constant, denoted by the symbol F and sometimes stylized as ℱ, is named after Michael Faraday. In chemistry and physics, this constant represents the magnitude of electric charge per mole of electrons. It has the currently accepted value

F = 96485.33212... C·mol−1.

Since 1 mol electrons = 6.02214076×1023 electrons (Avogadro's number), the Faraday constant is equal to the elementary charge e, the magnitude of the charge of an electron multiplied by 1 mole:

F = 96485.3... C/(1 mol) = 96485.3... C/(6.022...×1023) = 1.60217663410×10−19 C = e

One common use of the Faraday constant is in electrolysis calculations. One can divide the amount of charge in coulombs by the Faraday constant in order to find the chemical amount (in moles) of the element that has been oxidized.

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.

## 2019 redefinition

Since the 2019 redefinition of SI base units, which introduced exactly defined values for the elementary charge and the mole, the Faraday constant is exactly

e × (1 mol) mol−1 = 1.602176634×10−19 C × 6.02214076×1023 mol−1 = 96485.3321233100184 C·mol−1.

## Other common units

• 96.485 kJ per volt–gram-equivalent
• 23.061 kcal per volt–gram-equivalent
• 26.801 A·h/mol