Question

A current of 19296C is passed through an aqueous solution of copper sulphate using copper electrodes . what is the mass in g of copper deposited at the cathode ( molar mass of cu =63.5g mol-1)​

Answer 1

Answer:

The electrode reaction are:

1 mole

Cu

2+

+

2×96500 C

2e

−

→Cu(Cathode)

Cu×Cu

2+

+2e

−

(Anode)

Thus, cathode increases in mass as copper is deposited on it and the anode decreases in mass as copper from it dissolves.

Charge passed through cell =2.68×60×60 coulomb

Copper deposited or dissolved =

2×96500

63.5

×2.68×60×60=3.174 g

Increase in mass of cathode = Decrease in mass of anode =3.174 g.