When a current of $X$ Faraday is passed through a solution of aluminium nitrate,$1 \ mol$ of $Al$ is deposited. Then,$X =$ . . . . . . ?

The weight of silver $(at. \ wt. = 108)$ displaced by a quantity of electricity which displaces $5600 \ mL$ of $O_2$ at $STP$ will be ............ $g.$

An acidic solution of dichromate is electrolyzed for $8 \ min$ using $2 \ A$ current. As per the following equation: $Cr_{2}O_{7}^{2-} + 14H^{+} + 6e^{-} \rightarrow 2Cr^{3+} + 7H_{2}O$. The amount of $Cr^{3+}$ obtained was $0.104 \ g$. The efficiency of the process (in $\%$) is (Take: $F = 96000 \ C$,At. mass of chromium $= 52$)

On passing $0.5 \ F$ of electricity through $NaCl$,the amount of $Cl_2$ gas deposited at the anode is .............. $g$.

$A$ solution of copper sulphate is electrolysed for $10 \text{ minutes}$ with a current of $1.5 \text{ amperes}$. The mass of copper deposited at the cathode is:
(Given: Molar mass of $Cu = 63 \text{ g mol}^{-1}$; $1F = 96487 \text{ C mol}^{-1}$)

$A$ current of $0.4 \ A$ is passed through excess of molten $MgCl_2$ for $9.65 \times 10^4 \ sec$. The mass of $Mg$ deposited at the cathode is .............. $gm$