Two electrolytic cells containing silver nitrate solution and dilute sulphuric acid solution were connected in series. A steady current of 2.5 amp was passed through them till 1.078 g of silver was deposited?
`[Ag=107.8g mol^-1, 1f=96500C]`
How much electricity was consumed?

Two electrolytic cells containing silver nitrate solution and dilute sulphuric acid solution were connected in series. A steady current of 2.5 amp was passed through them till 1.078 g of silver was deposited? [Ag=107.8g mol^-1, 1f=96500C] What was the weight of oxygen gas liberated?

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?

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 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.

Aquesous copper sulphate solution and aqueous silver nitrate solution are electroolysed by 1 Ampere current for 10 minutes in separate electrolytic cells. Will the mass of copper and silver deposited on the cathode be same or different? Explain your answer.

How many grams of silver could be plated out on a serving tray by elelctolysis of a solution containing silver in +1 oxidation state for a period of 8.0 hours at a current of 8.46 amperes? What is the area of the tray if the thickness of the silver plating is 0.0025 cm? density of silver is 10.5 g/cm^3 .

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

Calculate how long it will take to deposit 1.0 g of chromium when a current of 1.25A flows through a solution of chromium sulphate.

Same amount of electric current is passed thorugh solution of AgNO_3 and HCl . If 1.08 g of silver is obtained in the first case, the amount of hydrogen liberated at S.T.P in the second case is:

A solution containing 2.675 g of CoCl_3 .6NH_3 (molar mass = 267.5 g mol^-1 ) is passed through a cation exchanger. The chloride ions obtained in solution were treated with excess of AgNO_3 to give 4.78 g of AgCl (molar mass = 143.5 g mol^-1 ). The formula of the complex is : (At. mass of Ag = 108 u)