What mass of copper can be deposited by the passage of 12.0 A for 25.0 min through a solution of copper(II) sulfate? [1 C = 1 A•s; F = 96,500 C]

Question

Quizplus · Accepted Answer

The mass of copper deposited can be calculated using Faraday's laws of electrolysis. First, convert the time to seconds: 25.0 min × 60 s/min = 1500 s. The total charge passed is current × time = 12.0 A × 1500 s = 18,000 C. The molar mass of copper (Cu) is 63.55 g/mol, and it has a valency of 2 in copper(II) sulfate, meaning it requires 2 moles of electrons (2 × 96,500 C = 193,000 C) to deposit 1 mole of Cu. The mass of Cu deposited is calculated as: (18,000 C / 193,000 C/mol) × 63.55 g/mol ≈ 5.93 g.

What Mass of Copper Can Be Deposited by the Passage