$3.17 \ g$ of a substance is deposited by a current of $0.1 \ mol$ of electrons. What is the equivalent weight of the substance?

Faraday's $2^{nd}$ law of electrolysis states that the mass of a substance deposited at an electrode is directly proportional to its:

Copper is to be electrodeposited on a nickel block of $(20 \times 5) \ cm^2$ area by using $CuSO_4$ as electrolyte. How much quantity of electricity is needed to deposit a $3.6 \ \mu m$ layer of copper (in $C$)? [Atomic weight of $Cu = 63.5 \ g \ mol^{-1}$,Density of $Cu = 8.9 \ g/cm^3$]

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:

An electrolytic cell contains a solution of $Ag_{2}SO_{4}$ and has platinum electrodes. $A$ current is passed until $1.6 \ g$ of $O_{2}$ is liberated at the anode. The amount of silver deposited at the cathode would be ............ $g$.

When the same quantity of electricity is passed through electrolytic cells containing different electrolytes connected in series,the amount of products obtained at the various electrodes is proportional to their: