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

Faraday's laws of electrolysis are related to the

During the electrolysis of molten sodium chloride,the time required to produce $0.10 \ mol$ of chlorine gas using a current of $3 \ A$ is .......... $\min.$

$A$ dilute solution of sulphuric acid is electrolysed using a current of $0.10 \ A$ for $2 \ hours$ to produce hydrogen and oxygen gas. The total volume of gases produced at $STP$ is $...... \ cm^3$. (Nearest integer) $[$ Given : Faraday constant $F = 96500 \ C \ mol^{-1}$ at $STP$,molar volume of an ideal gas is $22.7 \ L \ mol^{-1} ]$

Calculate the mass of $Ca$ deposited at the cathode by passing $0.8 \ A$ current through molten $CaCl_2$ for $60 \ minutes$. [Molar mass of $Ca = 40 \ g \ mol^{-1}$] (in $g$)

$18.4 \, A$ current is passed for $1$ hour and $42$ minutes through $CuSO_4$ solution using graphite electrodes at $298 \, K$ temperature and $1 \, bar$ pressure. If the cell efficiency is $75 \%$,calculate the mass of $Cu$ deposited and the volume of $O_2$ gas evolved at $STP$. $[Cu = 63.5 \, u, O = 16 \, u, R = 0.08314 \, L \, bar \, K^{-1} \, mol^{-1}]$