To deposit $0.6354 \ g$ of copper by electrolysis of aqueous cupric sulphate solution,the amount of electricity required (in coulombs) is

To gain $1 \ mole$ $Mg$ from $Mg^{2+}$ and $1 \ mole$ $Al$ from $Al^{3+}$,how many Coulombs of electricity are required respectively?

When the same quantity of electricity is passed through solutions of $Ag^{+}$,$Cu^{2+}$,and $Fe^{3+}$ ions,what is the ratio of the number of moles of each metal deposited?

The density and equivalent weight of a metal are $10.5\, g\, cm^{-3}$ and $100$,respectively. The time required for a current of $3\, A$ to deposit a $0.005\, mm$ thick layer of the same metal on an area of $80\, cm^2$ is closest to $....\, s$

The mass of ions deposited during a given interval of time in the process of electrolysis depends on

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: