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?

According to Faraday's Law,

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

Moles = 0.01