The laws of electrolysis were proposed by

When two electrolytic cells containing $NiSO_4$ and $CuSO_4$ solutions are connected in series and an electric current is passed,$1.6 \ g$ of $Cu$ is deposited on the electrode. How much $Ni$ metal is produced? If a cell containing $AgNO_3$ solution is connected instead of $NiSO_4$,how many grams of silver will be obtained? [Atomic mass: $Cu = 63.5 \ g/mol$,$Ni = 58.7 \ g/mol$,$Ag = 108 \ g/mol$]

What is the nature of the Faraday constant?

The amount of charge required to liberate $9 \ g$ of aluminium (atomic weight = $27$ and valency = $3$) in the process of electrolysis is ......... $coulombs$ (Faraday's constant $= 96500 \ C \ mol^{-1}$)

Oxidation of succinate ion produces ethylene and carbon dioxide gases. On passing $0.2 \ F$ electricity through an aqueous solution of potassium succinate,the total volume of gases (at both cathode and anode) at $STP$ ($1 \ atm$ and $273 \ K$) is .............. $L$

Match List $I$ with List $II$.

List $I$ (Conversion)	List $II$ (Number of Faraday required)
$A$. $1 \text{ mole of } H_2O \text{ to } O_2$	$I$. $3F$
$B$. $1 \text{ mol of } MnO_4^- \text{ to } Mn^{2+}$	$II$. $2F$
$C$. $1.5 \text{ mol of } Ca \text{ from molten } CaCl_2$	$III$. $1F$
$D$. $1 \text{ mol of } FeO \text{ to } Fe_2O_3$	$IV$. $5F$

Choose the correct answer from the options given below: