$A$ 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 ............. $g$ $(At. \, weight \, of \, Cu = 63.6)$.

If the electrochemical equivalent of a substance is $0.0006735 \ g/C$,what is its equivalent weight?

Calculate the quantity of electricity required to liberate $0.1 \ mole$ of chlorine gas during electrolysis of molten sodium chloride. (in $C$)

$9.65 \ C$ of electric current is passed through fused anhydrous $MgCl_2$. The magnesium metal thus obtained is completely converted into a Grignard reagent. The number of moles of Grignard reagent obtained is

The density of $Cu$ is $8.94 \, g \, cm^{-3}$. The quantity of electricity needed to plate an area $10 \, cm \times 10 \, cm$ to a thickness of $10^{-2} \, cm$ using $CuSO_4$ solution would be,if atomic mass of $Cu$ is $63.5$ .................. $C$

In $CuSO_4$ solution,when an electric current equal to $2.5 \ F$ (faraday) is passed,the number of $gm$ equivalents deposited on the cathode is: