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

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

When $9650 \ C$ of charge is passed through an $AgNO_3$ solution during the electrolysis process in an electroplating bath,what is the weight of silver deposited at the cathode in $g$?

$9.65 \ C$ 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

$A$ certain current liberated $0.504 \ g$ of hydrogen in $2 \ hours$. How many grams of copper can be liberated by the same current flowing for the same time in a copper sulphate solution?

$CuSO_4$ solution is electrolysed for $15 \ minutes$ to deposit $0.4725 \ g$ of copper at the cathode. The current in amperes required is (Faraday $= 96,500 \ C \ mol^{-1}$,atomic weight of copper $= 63$)