Three faradays of electricity were passed through an aqueous solution of iron $(II)$ bromide. The weight of iron metal (atomic weight $= 56$) deposited at the cathode (in $g$) is

In two separate experiments,the same quantity of electricity was passed through silver and gold solutions. The amounts of $Ag$ and $Au$ deposited are $2.15 \ g$ and $1.31 \ g$,respectively. The valency of gold is [Atomic mass of $Ag = 107.9$; $Au = 197$].

$A$ current is passed for $2 \, \text{hours}$ through an acidic solution,liberating $11.2 \, L$ of oxygen at $NTP$ at the anode. What will be the amount of copper deposited at the cathode by the same current when passed through a solution of copper sulphate for the same duration? .......... $g$

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

The approximate time duration in hours to electroplate $30 \ g$ of calcium from molten calcium chloride using a current of $5 \ A$ is [At. mass of $Ca=40$]