On passing $96500 \ C$ of charge through a $CuSO_4$ solution,the amount of copper liberated is:

Electrolytic cells containing $Zn$ and $Al$ salt solutions are connected in series. If $6.5 \ g$ of $Zn$ is deposited in one cell,calculate the mass of $Al$ deposited in the second cell (molar mass: $Zn=65 \ g \ mol^{-1}$,$Al=27 \ g \ mol^{-1}$) by passing a definite quantity of electricity. (in $g$)

In the electrolysis of a fused salt,the weight of the deposit on an electrode will not depend on:

How many seconds of current at $9.65 \ A$ must be passed through a solution of $Al^{3+}$ to obtain $1 \ \text{millimole}$ of $Al$ metal?

Faraday's laws of electrolysis state that the mass deposited on an electrode is proportional to:

$5 \, A$ current is passed through an electrolytic cell filled with $AgNO_3$ solution for $2.7$ hours. If $1$ spoon requires $0.01 \, g$ of silver to get coated,calculate how many spoons can be coated by the silver obtained at the cathode? $[Ag = 108 \, u]$