A Cr (aq) solution is electrolyzed using a current of 13.5 A. What mass of Cr(s) is plated out after 3.00 days?
- hcbiochemLv 72 months agoFavorite Answer
You didn't indicate the oxidation state of the chromium solution, but I am going to assume that it is 3+. If it is different that, you will have to alter one calculation.
Coulomb = 13.5 A X (3.00 day) X (24 hr/day) X (60 min/hr) X (60 s/min) = 3.50X10^6 Coulomb
Moles of electrons = 3.50X10^6 C /96485 C/mole e- = 36.3 mol e-
Moles Cr = 36.3 mol e- / 3 mol e- / mol Cr = 12.1 mol Cr X 52.00 g/mol = 629 g Cr(s)