How many moles of solid chromium can be deposited from a crcl3 solution when a steel wrench is electroplated with a current of 3.0 amps for 965 seconds? do this without a calculator?
W = I t e / F Where, W = Amount deposited = ? I = Current = 3 A t = Time = 965 s e = Chemical equivalence = 52/3 = 17.33 F = Faraday's Constant = 96500 Putting Values, W = (3 × 965 × 17.33) ÷ 96500 W = (50170.35) ÷ 96500 W = 0.52 g As we know, Moles = mass ÷ M.mass Putting values, Moles = 0.52 ÷ 52
