How many faraday of electricity are required to deposit $10 \ g$ of calcium from molten calcium chloride using inert electrodes (in $F$)? (Molar mass of calcium $= 40 \ g \ mol^{-1}$)

$A$ certain quantity of electricity is passed through an aqueous solution of $AgNO_3$ and a cupric salt solution connected in series. The amount of $Ag$ deposited is $1.08 \ g$. The amount of copper deposited is ............. $g$ (atomic weight of $Cu = 63.5$; $Ag = 108$).

How much electricity in terms of Faraday is required to reduce $2 \ mol$ of $MnO_4^{-}$ into $Mn^{2+}$?

$A$ steady current of $5 \, A$ is maintained for $45 \, min$. During this time,it deposits $4.572 \, g$ of zinc at the cathode of a voltameter. The $E.C.E.$ of zinc is:

$A$ solution of $Ni(NO_{3})_{2}$ is electrolysed between platinum electrodes using a current of $5 \, A$ for $20 \, minutes$. What mass of $Ni$ is deposited at the cathode (in $, g$)?

When the same quantity of electricity is passed through aqueous $H_2SO_4$ and molten $MgSO_4$,what is the ratio of the weights of hydrogen and magnesium deposited?