A steady current of 5 amps is maintained for 45 mins . During this time it deposits `4.572` gms of zinc at the cathode of a voltameter. E.C.E. of zinc is

If a steady current of 4 amp maintained for 40 minutes, deposits 4.5 gm of zinc at the cathode and then the electro chemical equivalent will be

A steady current of 10.0 A is maintained in a copper voltmeter . Calculate the time required to deposit 2.5 g of copper . Relative atomic mass of copper = 63.5 g .

A current of 5.00 A flowing for 30.00 min deposits 3.048 g of zinc at the cathode. Hence, equilvalent mass of zinc is:

A current of 5.00 A flowing for 30.00 min deposits 3.048 g of zinc at the cathode. Hence, equilvalent mass of zinc is:

A steady current of 10.0 A is maintained in a copper voltameter . Calculate the time required to deposit 2.5 g of copper . Relative atomic mass of copper = 63.5 g .

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)

If a current strength of 1 amp. is passed for 10 minutes in AgNO3 solution 4 gm Ag metal is deposited find the ECE of Ag.

A 5A current in passed through a solution of zinc sulphate for 40 min . The amount of zinc deposited at the cathode is

A 5A current in passed through a solution of zinc sulphate for 40 min . These amount of zinc deposited at the cathode is

Three electrolytic 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 through 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?