Three electrolytic 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 A was passed through them until 1.45g of silver deposited at the cathode of cell B. How long did the current flow? What mass of copper and zinc were deposited in the concerned cells? ( Atomic mass of Ag= 108, Zn = 65.4, Cu = 63.5)

Two electrolytic cells containing silver nitrate solution and dilute sulphuric acid were connected in a series. A steady current of 2.5 A was passed through them till 1.078 g of silver was deposited ( Ag = 107.8 g //" mol" ) (a) How much electricity was consumed? (b) What is the weight of oxygen gas liberated during the reaction?

When a current of 0.75 ampere is passed through CuSO_4 for 25 mins, 0.369 g of copper is deposited at the cathode. Calculate the atomic mass of copper.

Can copper sulphate solution be stored in zinc vessel ?

Copper sulphate solution can be stored in a zinc vessel.

A current of 0.5 amperes was passed through a solution of silver nitrate for six min. Find the mass of silver deposited. (Atomic mass of Ag = 108 )

Electric current is passed through two cells A and B in series. Cell A contains aqueous solution of Ag_(2) SO_(4) and platinum electrodes. Cell B contains aqueous solution of CuSO_(4) and copper electrodes. The current is passed till 1.6g of oxygen is liberated at the anode in cell A. Calculate the quantities of copper and silver deposited at the cathode of the two cells. [ Atomic mass, O = 16, Cu 63.5, Ag = 108]

Two electrolytic cells, one containing acidified ferrous chloride and another acidified ferric chloride are connected in series. The ratio of iron deposited at cathodes in the two cells when electricity is passed through the cell will be: