Electroplating is a way to coat a complex metal object with a very thin (and hen

Question

Electroplating is a way to coat a complex metal object with a very thin (and hence inexpensive) layer of a precious metal, such as silver or gold. In essence the metal object is made the cathode of an electrolytic cell in which the precious metal cations are dissolved in aqueous solution. Suppose a current of 0.830 A is passed through am electroplating cell with an aqueous solution of Ag_2SO_4 in the cathode compartment for 54.0 seconds. Calculate the mass of pure silver deposited on a metal object made into the cathode of the cell. Round your answer to 3 significant digits. Also, be sure your answer contains a unit symbol. [Ag^+(aq) + e^- rightarrow Ag(s)]

Explanation / Answer

Ans:

1. Current = charge(coloumbs)/time(seconds)

I = q/t

0.830A = q/54.0 seconds

q = 44.82 coloumbs

2. 1Faraday ie 96500Coloumbs charge is generated by 1 mol of electrons.

44.82 coloumbs generated by ? moles of electrons

44.82/96500 = x/1

x = 4.64 x 10-4 moles of electrons

3. 1 Ag takes 1 mole of electron ie

Ag atomic mass is 107.8682 g/mol

or 1 mole electron deposits 107.8682g Ag

ie 4.64 x 10-4 moles of electrons deposits ? g Ag

4.64 x 10-4 moles of electrons/1 mol electron = x g Ag/107.8626g

x = 4.64 x 10-4 x 107.8628 = 0.05 g Ag

ans: Amount of silver deposited at cathode is 0.05g

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