The quality of electricity required to discharge 1 mole of univalent ion is

Analyze the question: It asks for the quantity of electricity (charge) needed to discharge 1 mole of a univalent ion (an ion with a charge of 1+ or 1−) during electrolysis.

Concept: Faraday's Laws of Electrolysis

• One Faraday (F) is the quantity of electricity needed to discharge 1 mole of a univalent ion.
• It equals the charge carried by 1 mole of electrons.

Solution:

Charge of one electron: e = 1.602 × 10⁻¹⁹ C Avogadro's number: L = 6.02 × 10²³ per mole

Charge on 1 mole of electrons:

F = e × L = (1.602 × 10⁻¹⁹) × (6.02 × 10²³) ≈ 96,500 C/mol

For a univalent ion (e.g., Na⁺ + e⁻ → Na, or Ag⁺ + e⁻ → Ag), 1 mole of ions needs 1 mole of electrons, so the charge needed is 96,500 C.

For comparison:

• 1 mole of a divalent ion (e.g., Cu²⁺) would need 2 × 96,500 = 193,000 C (option D).
• 48,250 C is half a Faraday, so it is not the answer.
• 9,600 C is not a standard value for this.

Answer: Option C, 96,500 C.

Tip: Remember "1 Faraday = 96,500 C = 1 mole of electrons." Then multiply by the charge on the ion: 1 mole of an ion with charge n needs n Faradays. For example, Al³⁺ needs 3 × 96,500 C per mole.