A piece of matal weighing 200 g is to be electroplated with 5% of its weight with gold. If the strength of the available current is 2 ampere, how long would it take to deposite the required amount of gold . ECE of H `=0.1044xx10^(-4)`, atomic mass of gold =197.1, atomic weight of hydrogen =1.008 .

A metal plate weighting 750g is to be electroplated wiwth 0.05% of its weight of silver. If a current of 0.8A is used. Find the time needed for depositing the required weight of silver. "E.C.E. of silver is" 11.18xx10^(-7)kgC^(-1) .

Calculate the strength of the current required to deposit 1.2 g magnesium from molten MgCl_(2) in hour . [1F= 96,500Cmol^(-1), ("atomic mass"): Mg =24.0 u]

0.02 equivalent of Ag was deposited in an electrolysis experiment. If same quantity of a electricity is passed through a gold solution, 1.314 g of gold is deposited. Find oxidation state of the gold. (Atomic mass of Au = 197)

A current of 5A is passed fir 5hours through three voltameters arranged in series, containing solution of copper sulphate. Silver nitrate and sulphuric acid. Calculate the masses of silver, copper and hydrogen liberated (E.C.E of silver =11.18xx10^(-7) kg C^(-1) m=, atomic weight of silver =107.88, atomic weight of copper =63.57 and atomic weight weight of hyrdrogen=1.008.)

An electric current of 0.4 A is passed through a silver voltameter for half an hour . Find the amount of silver deposited on the cathode. ECE of silver = 1.2 xx 10^(-3) g C^(-1) .

How long will a current of 1 ampere take for complete deposition of copper from 1 litre of 1NCuSO_(4).5H_(2)O solution ?

A brass plate having surface area 200 cm^2 on one side is electroplated with 0.10 mm thick silver layers on both sides using a 15 A current. Find the time taken to do the job. The specific gravity of silver is 10.5 and its atomic weight is 107.9 g mol^(-1)