To deposit $0.6354 \ g$ of copper by electrolysis of aqueous cupric sulphate solution,the amount of electricity required (in coulombs) is

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 $Al = 27$)

What is the number of moles of electrons passed when a current of $2 \text{ A}$ flows through an electrolyte solution for $10 \text{ minutes}$?

The time required to remove electrolytically one fourth of $Ag^+$ from $0.2 \ L$ of $0.1 \ M \ AgCl$ solution by a current of $0.1 \ A$ is approximately $.......... \ min$.

Match the following and select the correct option for the quantity of electricity,in $C \ mol^{-1}$,required to deposit various metals at the cathode:

List-$I$	List-$II$
$a. \ Ag^{+}$	$i. \ 386000 \ C \ mol^{-1}$
$b. \ Mg^{2+}$	$ii. \ 289500 \ C \ mol^{-1}$
$c. \ Al^{3+}$	$iii. \ 96500 \ C \ mol^{-1}$
$d. \ Ti^{4+}$	$iv. \ 193000 \ C \ mol^{-1}$

The mass of carbon anode consumed (giving only carbon dioxide) in the production of $270 \ kg$ of aluminium metal from bauxite by the Hall process is ............... $kg$.