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.
Answer:
0.0103g of Ag
Explanation:
First we put down the reduction equation at the cathode showing the exact number of electrons transferred. In this case, only one electron was transferred.
But 1 mole of electrons =96500C of charge.
And Q=It that is current ×time
Substituting the values stated in the question, we obtain our answer as shown in the image attached.
