How many grams of chromium metal are plated out

Question

How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through an aqueous solution containing Cr+3 ions for 320 minutes?(at .wt. Cr = 52 g/mol)

Answer 1

Cr³⁺ + 3e- ==> Cr(s)

8.00 A = 8.00 C/sec

320 min x 60 sec/min x 8.00 C/sec = 153,600 C

153,600 C x 1 e-/96,500 C x 1 mol Cr/3 mol e- = 0.531 moles Cr

0.531 moles Cr x 52 g/mole = 28.1 g Cr