What is the number of moles of electrons passed when a current of $5 \ A$ is passed through a solution of $FeCl_3$ for $20 \ minutes$?

The mass of silver (Molar mass of $Ag: 108 \ g \ mol^{-1}$) displaced by a quantity of electricity which displaces $5600 \ mL$ of $O_2$ at $S.T.P.$ will be . . . . . . $g$.

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 $Ca=40$]

$A$ current of $0.01 \ A$ is passed through a solution of a metal bromide $(MBr_x)$. The only reaction at the cathode is the deposition of metal $(M)$. After $3 \ hours$,$0.072 \ g$ of metal $(M)$ is deposited. The value of '$x$' is approximately (Given: Atomic weight of $M = 192$)

How many moles of electrons (how many Faradays of electricity) are required to reduce $1 \ mol$ of $MnO_4^-$ to $MnO_2$?

During electrolysis,the amount of ions discharged is $NOT$ proportional to which of the following?