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?

4 ampere current was passed through an aqueous solution of an unknown salt of Pd for 1 hour, 3.977 g of P d^ n+ was deposited at cathode. Find n (mass of P d=106.4)

The following galvanic cell Zn|Zn(NO_3)_2(aq)||Cu(NO_3)_2(aq)|Cu Anode (100mL,1M)(100mL,1M) cathode was operated as an electrolysis cell as Cu as the anode and Zn as the cathode. A current of 0.48 ampere was passed for 10 hours and then the cell was allowed to function to galvanic cell.What would be the emf of the cell at 25^@C Assume that the only electrode reactions occurring were those involving Cu//Cu^(2+) and Zn//Zn^(2+) (E_(Cu^(2+),Cu)^@=+0.34V, E_(Zn^(2+),Zn)^@=-0.76V)

How much time would it take in minutes to deposit 1.18 g of metallic copper on a metal object when a current of 2.0 A is passed through the electrolytic cell containing Cu ^2 +ions? [ Molar mass of Cu =63.5 g /mol;IF=96,500 Cmol^-1]

A current of strength 2.5 amp was passed through CuSO4 solution for 6 minutes 26 seconds.The amount of copper deposited is (at. wt. of C u=63.5) cdot(F=96500 C) (a)0.3175g (b)3.175g (c)0.635g (d)6.35g

A current of 4 A is passed through a solution of silver nitrate to coat a metal surface of 80 cm^(2) with 0.005 mm thick layers of silver. If the density of silver (molar mass: 108 g "mol"^(-1) )is 10.8 g cm^(-3) , the time for which the current is passed is about