How many Faraday of electricity is required to produce $5 \ g$ of magnesium from magnesium chloride (in $F$)? (Molar mass $Mg = 24 \ g \ mol^{-1}$)

When the same quantity of electricity is passed through aqueous $AgNO_3$ and $H_2SO_4$ solutions connected in series,$5.04 \times 10^{-2} \ g$ of $H_2$ is liberated. What is the mass of silver (in grams) deposited? (Eq. wts. of hydrogen $= 1.008$,silver $= 108$)

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 $63.5$ .................. $C$

The time required to remove electrolytically one fourth of $Ag^+$ from $0.2 \ L$ of $0.1 \ M \ AgCl$ solution by a current of $0.1 \ A$ is approximately $.......... \ min$.

When electricity is passed through the solution of $AlCl_3$,$13.5 \ g$ of $Al$ are deposited. The number of Faraday required is:

$A$ 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 $Au = 197$)