When a current of 0.75A is passed through a `CuSO_4` solution for 25 min, 0.369g of copper is deposited. Calculate the atomic mass of copper.

A current of 4 amp was passed for 1.5 hours through a solution of copper sulphate when 3.2 g of copper was deposited. Calculate the current efficiency.

Two faraday of electricity is passed through a solution of CuSO 4 ​ . The mass of copper deposited at the cathode is : (at mass of Cu=63.5 u)

A solution of copper sulphate is electrolysed for 10 minutes with a current of 1.5 amperes. What is the mass of copper deposited at cathode ? The atomic mass of copper = 63.5 a.m.u.

Three conductivity cells A, B and C containing solutions of zinc sulphate, silver nitrate and copper sulphate respectively are connected in series. A steady current of 1.5 amperes is passed through them until 1.45 g of silver is deposited at the cathode of cell B. How long did the current flow ? What mass of copper and what mass of zinc got deposited in their respective cells ? (Atomic mass : Zn = 65.4 u, Ag = 108 u, Cu = 63.5 u)

A current of 3A was passed through a solution of AuCl_4^- ions using gold electrolyte and it caused deposition of 1.234g of Au. The time for which the current was passed is

when molten salt was elctrolysed for 5 min with9.65 A current , 0.18g of the metal was deposited. Calculate the Eq. mass of metal.

A current of 1.5A is passed through 500 mL of 0.25M solution of zinc sulphate for 1 hr with a current efficiency of 90%. Calculate the final molarity of Zn^(2+) assuming volume to be constant.

The same quantity of electrical charge that deposited 0.583g of silver was passed through solution of gold salt and 0.355g of gold was formed. What is the oxidation state of gold in this salt?

Three electrolytic cells A,B and C containing electrolyses of zinc sulphate, silver nitrate and copper sulphate respectively were connected in series. A steady current of 1.50 amp was passed through them until 1.45g of silver were deposited at the cathode of cell B. HOw long did the current flow?