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 0.140A is passed through an electroplating cell with an aqueous solution of Ag2SO4 in the cathode compartment for 64.0 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.

0.01g of silver will be deposited on the metal object

Explanation:

Electroplating is an an application of electrolytic reaction. The equation for the reaction at the cathode where silver is deposited is:

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

Showing that 1 faraday (96500C) is required for the deposition.

But quantity of electricity passed (Q) = I×t

Where I is the current= 0.14A

And t is the time= 64seconds

Q= 0.14 ×64 = 8.96 Coulomb

From the cathodic equation for the reaction, 96500C deposited 108g og silver, therefore 8.96C will deposit

8.96 × 108÷96500

0.01g of silver.

water at room temperature is flowing through a pipe with pressure taps located 10 ft apart along one section of the pipe, which are connected to a mercury (s=13.6) manometer.