$A$ current of $0.25 \, A$ is passed through $CuSO_4$ solution placed in a voltameter for $45 \, minutes$. The amount of $Cu$ deposited on the cathode is ............. $g$ $(At. \, weight \, of \, Cu = 63.6)$.

$1$ mole of electrons corresponds to how much Faraday,how much Coulomb,and how many electrons?

Two electrolytic cells containing molten solutions of nickel chloride and aluminium chloride are connected in series. If the same amount of electric current is passed through them,what will be the weight of nickel obtained when $18 \ g$ of aluminium is obtained (in $g$)? $[Al = 27 \ g/mol, Ni = 58.5 \ g/mol]$

The electrochemical equivalent $Z$ of any element can be obtained by multiplying the electrochemical equivalent of hydrogen with

$A$ current of $15.0 \ A$ is passed through a solution of $CrCl_2$ for $45 \ min$. The volume of $Cl_2$ (in $L$) obtained at the anode at $1 \ atm$ and $273 \ K$ is around ($1 \ F = 96500 \ C \ mol^{-1}$,At. wt. of $Cl=35.5$,$R=0.082 \ L \ atm \ K^{-1} \ mol^{-1}$) (in $.7$)

What is achieved by Faraday using the principles of electrolysis?