$96.5$ amperes current is passed through the molten $AlCl_3$ for $100$ seconds. The mass of aluminium deposited at the cathode is (atomic weight of $Al = 27$ $u$). (in $g$)

The quantity of electricity in Faraday needed to reduce $1 \ mol$ of $Cr_{2}O_{7}^{2-}$ to $Cr^{3+}$ is ....

When $10 \,A$ current is passed for $80 \,min$, the volume of hydrogen gas liberated at $STP$ is: (in $\,L$)

If nearly $10^5 \ C$ liberate $1 \ gm$ equivalent of aluminium,then the amount of aluminium (equivalent weight $9$) deposited through electrolysis in $20 \ minutes$ by a current of $50 \ A$ will be .............. $gm$.

How many electrons are involved in the reaction when $0.40 \ F$ of electricity is passed through an electrolytic solution?

Faraday's $2^{nd}$ law of electrolysis states that the mass of a substance deposited at an electrode is directly proportional to its: