To deposit $0.6354 \ g$ of copper by electrolysis of aqueous cupric sulphate solution,the amount of electricity required (in coulombs) is

In acidic medium,$MnO_4^-$ is converted to $Mn^{2+}$ when it acts as an oxidant. The quantity of electricity required to reduce $0.06 \ mol$ of $MnO_4^-$ would be ........... $F$.

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:

Charge required for reduction of $0.01 \ mol$ of $MnO_4^-$ in neutral medium is ............ $C$.

The number of electrons involved in redox reactions when $1$ Faraday of electricity is passed through an electrolyte in solution is

One Faraday of electricity liberates $x \times 10^{-1}$ gram atom of copper from copper sulphate,$x$ is . . . . . . .