0.5 faraday of electricity was passed to deposit all the copper present in 500 ml of CuSO4 solution. What was the Molarity of this solution?

 

Related Questions:

(1) A current of 2.68 ampere is passed for one hour through an aqueous solution of copper sulphate using copper electrodes. Calculate the change in the mass cathode and that of anode. ( atomic mass of copper is 63.5 u).

(2) In the electrolysis of aqueous solution of NaOH , 2.8 litre of oxygen at NTP liberated at anode. How much Hydrogen was liberated at cathode ?

(3) On passing 3 faradays of electricity through three electrolytic cells connect in series containing Ag+ , Ca+2 and Al+3 ions respectively , the molar ratio in which three metals ions are liberated at the electrode is

(4) How many grams of silver could be plated out on a serving tray by electrolysis of solution containing silver in +1 oxidation state for a period of 8 hours. At a current of 8.46 ampere? What is the area of tray if the thickness of silver plating is 0.00254 cm. density of silver is 10.5 gm cc.

(5) A current of 3 ampere passed for 2 hours through a solution of CuSO4 3 gm of Cu2+ ions were discharged at cathode calculate the current efficiency.

(6) What current strength ampere will be require to liberate 10 gm chlorine from sodium chloride solution in one hour?

(7) Ag is electrodeposited on a vessel of total surface area 800 cm2 by passing current of 0.2 A for 3 hrs. Calculate thickness of Ag deposited. (Density Ag = 9.67 g/ml).