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 $9.65 \ A$ is passed for $10 \ \text{minutes}$,$3.0 \ g$ of metal is deposited. What is the equivalent weight of the metal?

Copper is to be electrodeposited on a nickel block of $(20 \times 5) \ cm^2$ area by using $CuSO_4$ as electrolyte. How much quantity of electricity is needed to deposit a $3.6 \ \mu m$ layer of copper (in $C$)? [Atomic weight of $Cu = 63.5 \ g \ mol^{-1}$,Density of $Cu = 8.9 \ g/cm^3$]

One Faraday of electricity when passed through a solution of copper sulphate deposits:

$4.5 \ g$ of aluminium (atomic mass $27 \ amu$) is deposited at the cathode from an $Al^{3+}$ solution by a certain quantity of electric charge. The volume of hydrogen produced at $STP$ from $H^{+}$ ions in the solution by the same quantity of electric charge will be .............. $L$.

How many grams of chlorine gas will be produced as a product when a current of $2 \ A$ is passed through a concentrated aqueous solution of $NaCl$ for $30 \ \text{minutes}$?