At what amperage does the electrolysis of silver occur if 12 g of silver is released at the cathode in 5 minutes?

According to Faraday’s law, the mass of silver released during electrolysis can be calculated by the formula:
m = k * I * ∆t, where m is the mass of silver released at the cathode (m = 12 g = 0.012 kg), k is the electrochemical equivalent for silver (k = 1.118 * 10 ^ -6 kg / C), I is the force current, ∆t is the duration of electrolysis (∆t = 5 min = 5 * 60 s = 300 s).
Let us express and calculate the current strength:
I = m / (k * ∆t) = 0.012 / (1.118 * 10 ^ -6 * 300) ≈ 36 A.
Answer: Electrolysis occurs at a current strength of 36 A.