How many moles of electrons (how many Faradays of electricity) are required to reduce $1 \ mol$ of $MnO_4^-$ to $MnO_2$?

When a current of $0.5 \ A$ is passed for $2 \ hours$ through a molten metal salt,$3.88 \ g$ of the metal was deposited. If the atomic mass of the metal is $208 \ units$,the oxidation state of the metal in the salt is:

How much Faraday of electricity is required to reduce $1.5 \ mole$ of $KMnO_4$ into $MnO_2$ in a basic medium (in $F$)?

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

How long would it take to reduce completely $80 \ mL$ of $0.1 \ M$ $Fe_2(SO_4)_3$ to $FeSO_4$ by passing a current of $2 \ A$?

What is the $SI$ unit for electrochemical equivalent?