On passing $0.1 \ F$ of electricity through aluminium chloride,the amount of aluminium metal deposited on the cathode is $(Al = 27)$ ............ $g$.

The quantity of electricity needed to liberate $0.5 \ g$ equivalent of an element is

Aluminum oxide is electrolyzed at $1000^\circ C$ to produce aluminum metal. The cathode reaction is $Al^{3+} + 3e^- \rightarrow Al$. What quantity of electricity is required to produce $5.12 \ kg$ of aluminum metal? (Given: $1 \ Faraday = 96500 \ C$)

On passing $3 \ A$ of electricity for $50 \ minutes$,$1.8 \ g$ of metal deposits. The equivalent mass of the metal is:

Find the number of faradays of electricity required to produce $45 \ g$ of $Al$ from molten $Al_2O_3$. (in $F$)

The value of current required to deposit $0.972 \ g$ of chromium in $3 \ hours$ if the $E.C.E.$ of chromium is $0.00018 \ g \ C^{-1}$,is ............ $A$.