A metal object is to be gold-plated by an electrolytic procedure using aqueous AuCl₃electrolyte. How much gold may be deposited in 3.0 min by a constant current of 10. A?

Question

Quizplus · Accepted Answer

The amount of gold deposited can be calculated using Faraday's laws of electrolysis. The charge (Q) passed through the electrolyte is given by Q = It, where I is the current (10 A) and t is the time in seconds (3.0 min = 180 s). Thus, Q = 10 A × 180 s = 1800 C. The molar mass of gold (Au) is approximately 197 g/mol, and it has a valency of 3 in AuCl3. The charge required to deposit 1 mole of Au is 3 × 96500 C (Faraday's constant). Therefore, the moles of gold deposited are given by (1800 C) / (3 × 96500 C/mol) = 6.2 × 10^-3 mol.

A Metal Object Is to Be Gold-Plated by an Electrolytic