Faraday constant

The Faraday constant is a scientific value that represents the amount of electric charge carried by one mole of electric charge-carrying particles, such as electrons. Numerically, it equals approximately 96,485 coulombs, meaning that one mole of electrons (about 6.022 x 10²³ electrons) transfers this amount of charge. It’s used in electrochemistry to relate the amount of electric current involved in chemical reactions to the number of particles reacting, helping scientists understand and calculate processes like battery operation and metal plating.