One Faraday equals how many coulombs?

• A. 86000 C
• B. 96500 C
• C. 100000 C
• D. 76500 C

Answer: (B)

One Faraday is the charge carried by one mole of electrons. This constant, called the Faraday constant, is F = N_A × e, where N_A is Avogadro’s number and e is the elementary charge. Calculating gives F ≈ (6.022×10^23 mol⁻¹) × (1.602×10⁻¹⁹ C) ≈ 9.6485×10^4 C/mol, i.e., about 96485 C per mole of electrons. So one Faraday is roughly 9.6485×10^4 coulombs. The closest value among the options is 96500 C. This is the quantity you use to convert moles of electrons transferred in a redox reaction or electrolysis into coulombs of charge; for example, transferring 0.5 moles of electrons corresponds to about 4.82×10^4 C.