A current of 10.0 amps over a period of 3.00 hr is passed through a solution of molten KCl. What weight of K metal is produced?

Question

Quizplus · Accepted Answer

The weight of K metal produced can be calculated using Faraday's laws of electrolysis. The charge passed is 10.0 A * 3.00 hr * 3600 s/hr = 108,000 C. The molar mass of K is 39.1 g/mol, and it requires 1 mole of electrons (96,485 C) to produce 1 mole of K. Therefore, the weight of K produced is (108,000 C / 96,485 C/mol) * 39.1 g/mol = 43.8 g.

A Current of 10