Calculate the time required in seconds to deposit $6.35 \ g$ of copper from its salt solution by passing a $5 \ A$ current. [Molar mass of $Cu = 63.5 \ g \ mol^{-1}$]

$A$ current of $0.4 \ A$ is passed through excess of molten $MgCl_2$ for $9.65 \times 10^4 \ sec$. The mass of $Mg$ deposited at the cathode is .............. $gm$

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

The quantity of charge required to obtain $1 \, mole$ of aluminium from $Al_2O_3$ is ............ $F$.

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

Mass in grams of copper deposited by passing $9.6487 \ A$ current through a voltmeter containing copper sulphate solution for $100 \ s$ is (Given : Molar mass of $Cu: 63 \ g \ mol^{-1}, 1 \ F=96487 \ C$ ) (in $g$)