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 ........... $F$.

$A$ current of $3 \ A$ is passed through a molten calcium salt for $1 \ hr \ 47 \ min \ 13 \ s$. The mass of calcium deposited is $(Molar \ mass \ of \ Ca = 40 \ g \ mol^{-1})$ (in $g$)

When the same quantity of electricity is passed through aqueous $AgNO_3$ and $H_2SO_4$ solutions connected in series,$5.04 \times 10^{-2} \ g$ of $H_2$ is liberated. What is the mass of silver (in grams) deposited? (Eq. wts. of hydrogen $= 1.008$,silver $= 108$)

The electrochemical equivalent of a metal is $x \ g \ C^{-1}$. The equivalent weight of the metal is:

$A$ current of strength $2.5 \ A$ was passed through $CuSO_4$ solution for $6 \ \text{minutes} \ 26 \ \text{seconds}$. The amount of copper deposited is .............. $g$ (Atomic weight of $Cu = 63.5$) $(1 \ F = 96500 \ C)$

$0.066 \ g$ of metal was deposited when a current of $2 \ A$ is passed through a metal ion solution for $100 \ s$. What is the electrochemical equivalent (in $g \ C^{-1}$) of the metal?