The amount of current in Faraday required for the reduction of $1 \ mol$ of $Cr_{2}O_{7}^{2-}$ ions to $Cr^{3+}$ is, (in $F$)

What will be the weight of $Al$ deposited at the cathode when $0.5 \ F$ of electricity is passed through an aqueous solution of $AlCl_3$ (in $g$)? (Atomic mass of $Al = 27$)

$A$ solution of $CuSO_4$ is electrolysed for $10$ minutes with a current of $1.5$ amperes. What is the mass of copper deposited at the cathode (in $g$)?

To deposit one litre of hydrogen at $22.4 \text{ atmosphere}$ from acidulated water,the quantity of electricity that must pass through is ............. $coulomb$.

The electrochemical equivalent of a metal is $x \ g \ C^{-1}$. The equivalent weight of the metal is:

$1 \ F$ current means $...$ Coulomb electricity. (in $C$)