When $1 \ C$ of charge is passed through an electrolyte solution,the mass deposited is equal to:

The electrolytic cells,one containing acidified ferrous chloride and another acidified ferric chloride,are connected in series. The ratio of iron deposited at the cathodes in the two cells when electricity is passed through the cells will be:

When $9.65 \ C$ of electricity is passed through a solution of silver nitrate (atomic weight of $Ag = 108$),the amount of silver deposited is $............ \ mg$.

How many atoms of calcium will be deposited from molten $CaCl_2$ by a current of $25 \, mA$ flowing for $60 \, s$?

The amount of copper metal deposited at the cathode on passing an electric current of $500 \, mA$ for $20 \, minutes$ in a cupric chloride solution is ............ $g$.

How many total Faraday currents will be required to obtain $1 \ mole$ of $Ag$,$Mg$,and $Al$ respectively?