A current of 0.50 ampere is passed for 30 minutes through a voltameter containing copper sulphate solution. Calculate the mass of Cu deposited at the cathode. Given that atomic mass of Cu is 63.0amu.

A solution of CuSO_4 is electolysed for 10 minutes with a current of 1.5 amperes. What is the mass of copper deposited at the cathode?

A current of 1.50A was passed through an electrolytic cell containing AgNO_3 solution with inert electrodes. The mass of silver deposited to cathode was 1.50g. How long did the current flow? (atomic mass of Ag = 108u, 1F = 96500C).

A solution of Ni(NO_3)_2 is electrolysed between platinum electrodes using a current of 5 amperes for 20 minutes. What mass of Ni is deposited at the cathode?

Three electolytic cells A,B,C containing solutions of ZnSO_4 , AgNO_3 and CuSO_4 respectively are connected in series. A steady current of 1.5 amperes was passed throught them until 1.45 g of silver deposited at the cathode of cell B. How long did the current flow? What mass of copper and zinc were deposited?

Three electrolytic cells A, B and C containing electrolytes ZnSO_4 , AgNO_3 and CuSO_4 respectively were connected in series. A steady current of 1.5A was passed through them. 1.45g Ag were deposited at the cathode of cell B.What mass of copper and zinc were deposited? (Atomic mass of Cu = 63.5u, Zn = 65.3u, Ag = 108u.)

Three electrolytic cells A, B and C containing electrolytes ZnSO_4 , AgNO_3 and CuSO_4 respectively were connected in series. A steady current of 1.5A was passed through them. 1.45g Ag were deposited at the cathode of cell B. How long did the current flow?(Atomic mass of Cu = 63.5u, Zn = 65.3u, Ag = 108u.)

Aluminium crystallises as face-centered cubic lattice and it has a density of 2.7xx10^3kgm^(-3) . Calculate edge length of the unit cell. Given atomic mass of aluminium equal to 27.0 amu.

Calculate the electrode potential at a copper electrode dipped in 0.1 M solution of copper sulphate at 25^@C . Given, the standard emf of Cu^(2+) system is +0.34V at 298K.