Final answer:
To electrolyze Au+ to produce 2.20 mol of Au, you would require 212,300 coulombs, which is calculated using the Faraday's constant of 96,500 C/mol for the charge of electrons needed to reduce the gold ions.
Step-by-step explanation:
The number of coulombs required to electrolyze Au+(aq) to produce 2.20 mol Au is calculated by considering the charge required to reduce gold ions to gold metal. Since each gold ion requires one electron to be reduced to gold metal, and 1 mol of electrons carries a charge of 96,500 C (1 Faraday), we can determine the total charge required for 2.20 mol of gold.
Number of coulombs = moles of Au × moles of electrons per mole of Au × Faraday's constant.
Number of coulombs = 2.20 mol × 1 mol e-/mol Au × 96,500 C/mol e-.
Number of coulombs = 212,300 C.