In an industrial electrolytic cell with current efficiency of 75% it is desired to produce 48 g of Mg metal per hour. Calculate the charge required:

Calculate the current in amperes required to liberate 10g of iodine electrolytically in one hour from KI solution .

Calculate the quantity of electricity that would be required to reduce 12.3g of nitrobenzene to aniline, if the current efficiency for the process is 50% . If the potential drop across the cell is 3.0V , how much energy will be consumed?

Current efficiency is defined as the extent of a desired electrochemical reaction, divided by the theoretical extent of the reaction times 100%. What is the current efficiency of an electrodeposition of Cu metal in which 9.8g Cu is deposited by passage of 3A current for 10000 seconds.

Hg_(2)CI_(2) is produced by the electrolytic reduction of Hg^(2+) ion in presence of CI^(-) ion is 2Hg^(2+) +2CI^(-) +2e^(Theta) rarr Hg_(2)CI_(2) . Calculate the current required to have a rate production of 44g per hour of Hg_(2)CI_(2) . [Atomic weight of Hg = 200.6] :-

State Faraday's first law of electrolysis . How much charge in terms of Faraday is required for the reduction of 1mol of Cu^(2+) to Cu. (b) Calculate emf of the following cell at 298 K : Mg(s) | Mg ^(2+)(0.1 M)||Cu^(2+) (0.01)|Cu(s) [Given E_(cell)^(@)=+ 2.71V, 1 F = 96500C mol^(-1)]

An aqueous solution of NaCl on electrolysis gives H_(2)(g), Cl_(2)(g), and NaOH accroding to the reaction : 2Cl^(c-)(aq)+2H_(2)Orarr2overset(c-)(O)H(aq)+H_(2)(g)+Cl_(2)(g) A direct current of 25A with a current efficiency of 62% is passed through 20L of NaCl solution (20% by weight ) . Write down the reactions taking place at the anode and cathode. How long will it take to produce 1 kg of Cl_(2) ? ( Assume no loss due to evaporation . )

An aqueous solution of NaCl on electrolysis gives H_(2)(g), Cl_(2)(g), and NaOH accroding to the reaction : 2Cl^(-)(aq)+2H_(2)Orarr2overset(-)(O)H(aq)+H_(2)(g)+Cl_(2)(g) A direct current of 25A with a current efficiency of 62% is passed through 20L of NaCl solution (20% by weight ) . Write down the reactions taking place at the anode and cathode. How long will it take to produce 1 kg of Cl_(2) ? What will be the molarity of the solution with respect to hydroxide ion ? ( Assume no loss due to evaporation . )

When molten lithium chloride (LiCl) is electrolysed, lithium metal is formed at the cathode. If current efficiency is 75% then how many grams of lithium are liberated when 1930 C charge pass through the cell? (Atomic mass of Li=7)

3g of metal ions were discharged at cathode using a current of 3 amperes for 2 hours from aqueous cupric sulphate solution. Calculate the current efficiency. At wt . of Cu is 63.5 .

A current of 10A is employed to plate nickel in NiSO_(4) bath. The current efficiency with respect to Ni plating is 60% . a. How many grams of Ni is plated on the cathode per hour ? b. What is the thickness of the plating if the cathode consists of a sheet of metal 4.0 cm^(2) which is coated on both faces ? c. What is the volume of H_(2)(STP) evolved during above electrolysis ?