The electrochemical equivalent of a metal is $x \ g \ C^{-1}$. The equivalent weight of the metal is:

The amount of charge in $F$ (Faraday) required to obtain one mole of iron from $Fe_{3}O_{4}$ is (Nearest Integer).

$96.5$ amperes current is passed through the molten $AlCl_3$ for $100$ seconds. The mass of aluminium deposited at the cathode is (atomic weight of $Al = 27$ $u$). (in $g$)

Faraday's laws of electrolysis state that the mass deposited on an electrode is proportional to:

$A$ constant current was passed through a solution of $AuCl_4^-$ ion between gold electrodes. After a period of $10.0 \ \text{minutes}$,the increase in mass of cathode was $1.314 \ \text{g}$. The total charge passed through the solution is . . . . . . $\times 10^{-2} \ \text{F}$. (Given atomic mass of $Au = 197$)

The mass of carbon anode consumed (giving only carbon dioxide) in the production of $270 \ kg$ of aluminium metal from bauxite by the Hall process is ............... $kg$.