In electrochemistry, one Faraday represents the charge of one mole of electrons. It is determined by multiplying the charge of a single electron by Avogadro's number.
The charge of a single electron is approximately \(1.602 \times 10^{-19}\) Coulombs. Avogadro's number, representing the quantity of atoms or molecules in one mole, is approximately \(6.022 \times 10^{23}\).
The value of one Faraday is computed as follows:
Faraday = Charge of one electron × Avogadro's number
Faraday = \(1.602 \times 10^{-19} \) C × \(6.022 \times 10^{23}\)
This calculation results in approximately 96587 Coulombs.
Thus, the value is 96587.