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 0.490 A is passed through an electroplating cell with an aqueous solution of AgNO_3, In the cathode compartment for 90.0 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.

Answer 1

0.049 g of Ag

Step-by-step explanation:

From the question;

Ag^+ (aq) + e ----->Ag(s)

1 e = 96500 C

Note that Q= It

Where;

I = current and t= time taken

108 g of silver is deposited by 96500 C of electricity

x g is deposited by (0.49 * 90) C

x = 108 * (0.49 * 90) /96500

x= 0.049 g of Ag