A metal object is to be gold-plated by an electrolytic procedure using aqueous AuCl₃ electrolyte. Calculate the number of moles of gold deposited in 3.0 min by a constant current of 10.A.

Question

Quizplus · Accepted Answer

The amount of charge transferred during the electrolysis can be calculated using Faraday's Law:

Q = It

Where Q is the charge transferred (in Coulombs), I is the current (in Amperes), and t is the time (in seconds).

We can convert Coulombs to moles of gold using the equation:

1 mole of gold = 1 Faraday = 96,485 Coulombs

Therefore, the number of moles of gold deposited can be calculated as:

n = Q / (1 Faraday)

n = (It) / (1 Faraday)

n = (10 A)(3.0 min × 60 s/min) / (96,485 C/mol)

n = 6.2 × 10^-3 mol

Therefore, the best choice is A, with a value of 6.2 × 10^-3 mol.

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