Faraday Law of Electrolysis: According to Faraday's Law, the mass of a substance deposited during electrolysis is directly proportional to the quantity of electricity passed through the solution.
Faraday stated that 96500 Coulombs (1 Faraday) of electricity is required to deposit 1 mole of any metal. For the reaction: Mg2+ + 2e- ⶠMg, 19300 Coulombs (2 Faraday) of electricity is required to deposit 1 mole of Magnesium metal (1 mole of Mg = 24g).
This implies that 19300 Coulombs will liberate 24g and x Coulombs will liberate 0.110g of magnesium. We can calculate the value of x as follows:
x = (19300 Ã 0.110) / 24
x = 884.6 Coulombs
Using the formula Q = It, where Q is the quantity of electricity, I is the current, and t is the time taken, we can determine the time required to deposit 0.110 grams of magnesium:
884.6 = 0.998 Ã t
t = 884.6 / 0.998
t â 886.3 seconds
Therefore, the time required to deposit 0.110 grams of magnesium metal from the given solution with a current of 0.998 A applied is approximately 886.3 seconds.