How many coulombs would be required to electroplate 35.0 grams of chromium by passing an electrical current through a solution containing CrCl₃?

Question

Quizplus · Accepted Answer

To electroplate chromium, we need to calculate the moles of chromium and then the charge required. The molar mass of Cr is 51.996 g/mol, so 35.0 g is 0.673 moles. CrCl3 provides 3 electrons per Cr atom, so 0.673 moles of Cr require 0.673 × 3 = 2.019 moles of electrons. Since 1 mole of electrons is 96485 C, the total charge is 2.019 × 96485 = 1.95 × 10^5 C.

How Many Coulombs Would Be Required to Electroplate 35