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 0.110A is passed through an electroplating cell with an aqueous solution of AgNO3 in the cathode compartment for 84.0 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.

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Asked Nov 22, 2019
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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 0.110A is passed through an electroplating cell with an aqueous solution of AgNO3 in the cathode compartment for 84.0 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.

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Expert Answer

Step 1

The electrolysis equation is given as,

Ag
Agte
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Ag Agte

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Step 2

Now, 1 mol of silver requires 1 electron and 1 mol of electron consists of 96485 C. It is given that a current of 0.110 A is passed for a duration of 84 sec and hence the charge can be calculated as,

Q Ixt
Q 0.11 x 84
Q 9.24 C
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Q Ixt Q 0.11 x 84 Q 9.24 C

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Step 3

Since 96485 C are contained in 1 mol of electron. Hence the ...

1
x 9.24
No. of moles in 9.24 C =
96485
No. of moles in 9.24 C 9.57 x 10-5 mols
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1 x 9.24 No. of moles in 9.24 C = 96485 No. of moles in 9.24 C 9.57 x 10-5 mols

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