What mass of gold is produced when 23.0A of current are passed through a gold so

Question

What mass of gold is produced when 23.0A of current are passed through a gold solution for 42.0 minutes

Metal plating is done by passing current through a metal solution. For example, an item can become gold plated by attaching the item to a power source and submerging it into a Au3+ solution. The item itself serves as the cathode, at which the Au3+ ions are reduced to Au(s). A piece of solid gold is used as the anode and is also connected to the power source, thus completing the circuit What mass of gold is produced when 23.0A of current are passed through a gold solution for 42 0 min ? Express your answer with the appropriate units.

Explanation / Answer

23.0 A for 42.0 min is
23.0 Coulomb/s x 42.0 min x 60 sec/min = 57960 Coulombs
One Faraday is 96,500 Coulombs
57960 Coulombs / 96,500 Coulombs / Faraday = 0.600 Faraday
Au3+ + 3e- >> Au
For every 3 Faradays of electricity used up , one mole Au forms.
0.600 Faraday x 1 mole Au/ 3 Faradays = 0.200 mole Au
One mole Au is 196.967 g
196.967 g/mol x 0.200 = 39.43 g Au

Related Questions

Navigate

• Browse (All)
• Browse W
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.