Current: In a certain electroplating process gold is deposited by using a current of 14.0 A for 19 minutes. A gold ion, Au⁺, has a mass of approximately 3.3 × 10^-22 g. How many grams of gold are deposited by this process?

Question

Quizplus · Accepted Answer

To calculate the mass of gold deposited, we use Faraday's laws of electrolysis. The charge (Q) passed is Q = It = 14.0 A * 1140 s (19 minutes = 19 * 60 = 1140 seconds). The amount of substance deposited (n) can be calculated using Q = nF, where F is Faraday's constant (approximately 96485 C/mol). Since the charge of a gold ion is +1, each ion requires 1 mole of electrons to be deposited. The mass (m) deposited is then m = n * M, where M is the molar mass of gold (approximately 197 g/mol). By calculating n from Q and then m, we find that the mass of gold deposited is closest to 33 g, making option A correct.

Current: in a Certain Electroplating Process Gold Is Deposited by Using