When $1 \ F$ (Faraday) of electricity is passed through an aqueous solution of $CuSO_4$,the amount of $Cu$ deposited is:

Passage of a current for $548 \, s$ through a silver coulometer results in the deposition of $0.746 \, g$ of silver. What is the current (in $A$)?

The value of one Faraday is .............. $C \ mol^{-1}$.

On electrolysis of aqueous $CuSO_4$ solution using $Cu$ electrodes,if $2.5 \ g$ of $Cu$ is deposited at the cathode,then at the anode:

The amount of metal deposited at the cathode on passing an electric current of $0.75 \ A$ in an aqueous ferric sulphate solution for $30 \ min$ will be - ........... $g$ (atomic weight of $Fe = 56$).

What mass of silver (Atomic mass = $108 \text{ g/mol}$) is deposited by a quantity of electricity that displaces $5600 \text{ mL}$ of $O_2$ gas at $STP$ (in $\text{ g}$)?