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 140.0 ma is passed through an electroplating cell with an aqueous solution of ag2s04 in the cathode compartment for 22.0 seconds. calculate the mass of pure silver deposited on a metal object made into the cathode of the cell. round your answer to significant digits. also, be sure your answer contains a unit symbol.

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AnnuG AnnuG · Answer 1 · 2022-11-24T17:11:04+01:00

The mass of pure silver deposited on a metal object made into the cathode of the cell is 1350g.

2Ag2S04(s) + 4H2O(l) ---> 4Ag(s) + 4HSO4-(aq) + O2(g)

4Ag(s) + 4e- ---> 4Ag(0)

Ecell = -0.800V

n = Q/F ( n = charge/ charge per mole of electrons)

n = It/F ( n = current(A) x time/ charge per mole of electrons)

n = (140.0mA) (22.0s) / (4e-)

n = 12.5mol

M = m/n

M = (12.5mol)(108g/mol)

M = 1350g

In above equation, 2 moles of Ag2SO4 is reacts with 4 moles of H2O and gives 4 moles of Ag, 4 moles of HSO4 and 1 mole of O2.

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