$2.644 \ g$ of metal $(M)$ was deposited when $8040 \ C$ of electricity was passed through molten $MF_2$ salt. What is the atomic mass of $M$ $(F = 96500 \ C \ mol^{-1})$ (in $u$)?

$A$ current of $2.0 \ A$ is passed for $5 \ hours$ through a molten metal salt,which deposits $22.2 \ g$ of metal (At. wt. $= 177$). The oxidation state of the metal in the metal salt is:

When an electric current is passed through a solution of $KCl$,$19.5 \ g$ of potassium (atomic mass $= 39$) is deposited. If the same amount of electric current is passed through a solution of $AlCl_3$,how many grams of aluminum will be liberated?

Silver is removed electrically from $200 \ mL$ of a $0.1 \ N$ solution of $AgNO_3$ by a current of $0.1 \ A$. How long will it take to remove half of the silver from the solution? $(F = 96500 \ C \ mol^{-1})$

Aluminium oxide may be electrolysed at $1000 \, ^\circ C$ to furnish aluminium metal (At. Mass $= 27 \, amu$; $1 \, F = 96,500 \, C$). The cathode reaction is $Al^{3+} + 3e^- \to Al^0$. To prepare $5.12 \, kg$ of aluminium metal by this method would require:

$0.592 \ g$ of copper is deposited in $60 \ minutes$ by passing $0.5 \ amperes$ current through a solution of copper$(II)$ sulphate. The electrochemical equivalent of copper$(II)$ (in $g \ C^{-1}$) is $\left(F=96500 \ C \ mol^{-1}\right)$