How long should aqueous $NaCl$ be electrolysed by passing $100 \ A$ current,so that $0.5 \ mol$ chlorine is released at anode?

Calculate the quantity of electricity required to produce $0.42 \ g$ of $Ag$ at the cathode during the electrolysis of an $AgNO_3$ solution. (Molar mass of $Ag = 108 \ g \ mol^{-1}$) (in $C$)

$5 \, A$ current is passed through an electrolytic cell filled with $AgNO_3$ solution for $2.7$ hours. If $1$ spoon requires $0.01 \, g$ of silver to get coated,calculate how many spoons can be coated by the silver obtained at the cathode? $[Ag = 108 \, u]$

If solutions of silver nitrate and cupric salt are connected in series and the same current is passed,what will be the weight of copper deposited in $gm$ when $1.08 \ g$ of silver is deposited?

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