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.

 

Related Questions:

(1) The conductivity of 0.0011028 mol per liter acetic acid is 4.95 × 10–5 S per cm. Calculate its dissociation constant if ^°m for acetic acid is 390.5 S cm2 per mol–1 .

(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 to determine anode and cathode of concentration cell instead of both electrodes are same ?

(5) Write correct Nernst equation for the given galvanic cell containing both the electrodes are M/M (insoluble) salt at 25°c.: Ag(s)|AgCl(s)| KCl(M) || KBr (M)|AgBr(s)|Ag(s): [Given Ksp(AgCl) and Ksp(AgCl)]

(6) A silver electrode is immersed in saturated solution of Ag2SO4(aq). The potential difference between the silver and standard electrode is found to be 0.711 V. determined Ksp(Ag2SO4) given E0Ag+/Ag= 0.799 V

(7) 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.

(8) Calculate the emf of the cell: Pt H2(1atm)ICH3COOH(0.1M) II NH4OH(0.01M)IH2(1 atm)Pt and Ka for CH3COOH= 1.8x10^-5 and Kb for NH4OH = 1.8x10^-5