Which is the weight of $Al$ deposited at cathode when $1 \ A$ current is passed through molten $AlCl_3$ for $9650 \ s$ (in $g$)?
(Atomic mass of $Al = 27$)

Cells $A$ and $B$ contain aqueous solutions of ferrous chloride $(FeCl_2)$ and ferric chloride $(FeCl_3)$ respectively. If the same quantity of electricity is passed through both cells, what is the ratio of the mass of iron deposited in cell $A$ to that in cell $B$?

How many electrons flow when a current of $5 \ A$ is passed through a cell for $200 \ s$?

In an electroplating experiment,$m \ g$ of silver is deposited when $4 \ A$ of current flows for $2 \ min$. The amount (in $g$) of silver deposited by $6 \ A$ of current flowing for $40 \ s$ will be:

How many moles of electrons (how many Faradays of electricity) are required to reduce $1 \ mol$ of $MnO_4^-$ to $MnO_2$?

Which of the following aqueous solutions will result in the maximum number of moles of metal deposited on passing the same amount of charge?