In 10 minutes, 508 ml / g of bivalent metal was released in the electrolytic

In 10 minutes, 508 ml / g of bivalent metal was released in the electrolytic bath. Find out which metal it is if the current strength during electrolysis was 2.5

According to Faraday’s law, the mass of the released metal during electrolysis can be calculated by the formula:
m = k * I * ∆t, where m is the mass of the released metal (m = 508 mg = 508 * 10 ^ -6 kg), k is the electrochemical equivalent, I is the current strength (I = 2.5 A), ∆t – duration of electrolysis (∆t = 10 min = 10 * 60 = 600 s).
Let us express and calculate the electrochemical equivalent:
k = m / (I * ∆t) = 508 * 10 ^ -6 / (2.5 * 600) = 3.39 * 10 ^ -7 kg / C (the desired metal is copper or zinc).
Answer: The desired metal is copper (zinc).