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 is passed through an electroplating cell with an aqueous solution of in the cathode compartment for seconds. Calculate the mass of pure silver deposited on a metal object made into the cathode of the cell. Be sure your answer has a unit symbol and the correct number of significant digits.

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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 0.270 A is passed through an electroplating cell with an aqueous solution of in the cathode compartment for 72 seconds. Calculate the mass of pure silver deposited on a metal object made into the cathode of the cell. Be sure your answer has a unit symbol and the correct number of significant digits.

0.219 g

Explanation:

According to mole concept:

1 mole of an atom contains number of particles.

We know that:

Charge on 1 electron =

To calculate the charge passed, we use the equation:

where,

I = current passed = 0.272 A

q = total charge = ?

t = time required = 72.0 s

Putting values in above equation, we get:

108 g of silver is deposited by 1 mole of electrons

96500 C deposits = 108 g of dilver

Thus 19.6 C deposits =

Thus the mass of pure silver deposited on a metal object made into the cathode of the cell is 0.0219 g

right

explanation:

there are no statements provided but here is why:

sulfur belongs to group 16 because it can be found in nature whether it is in a free or combined state.

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