How much electricity in terms of Faraday is required for the reduction of $2 \ mol$ of $Cr_2O_7^{2-}$ into $Cr^{3+}$ in an acidic medium (in $F$)?

Calculate the amount of electricity required to convert $1.1 \ mol$ of $Cr_2O_7^{2-}$ to $Cr^{3+}$ in acidic medium.

Calculate the quantity of electricity required to produce $0.42 \ g$ of $Ag$ at the cathode during the electrolysis of an $AgNO_3$ solution. (Molar mass of $Ag = 108 \ g \ mol^{-1}$) (in $C$)

On passing $C$ ampere of current for time $t$ seconds through $1 \ L$ of $2 \ M$ $CuSO_4$ solution (atomic weight of $Cu = 63.5$), the amount $m$ of $Cu$ (in grams) deposited on the cathode will be:

The amount of metal deposited at the cathode on passing an electric current of $0.75 \ A$ in an aqueous ferric sulphate solution for $30 \ min$ will be - ........... $g$ (atomic weight of $Fe = 56$).

The chemical equivalent of silver is $108$. If the current in a silver voltameter is $2 \ A$,the time required to deposit $27 \ g$ of silver will be ............ $hrs$.