The number of $Faradays$ needed to reduce $4 \ g$ equivalents of $Cu^{++}$ to $Cu$ metal will be:

The number of moles of electrons required to deposit $36 \ g$ of $Al$ from an aqueous solution of $Al(NO_3)_3$ is (At. wt. of $Al = 27$)

How much current should be passed through acidified water for $100 \ s$ to liberate $0.224 \ L$ of $H_2$ gas at $STP$ (in $A$)?

If a current of $5 \ A$ is passed through a zinc sulfate solution for $40 \ \text{minutes}$,what is the mass of zinc deposited at the cathode (in $g$)?

The number of electrons required to deposit $1 \ g$ atom of aluminium (at. wt. $= 27$) from a solution of aluminium chloride will be ............ $N$ (where $N$ is Avogadro's number).

When $3 \ F$ of electricity is passed through an aqueous solution of iron $(II)$ bromide,what is the mass of iron metal deposited at the cathode in $g$?