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

How much charge is required for the following reductions:
$(i)$ $1 \, mol$ of $Al^{3+}$ to $Al$.
$(ii)$ $1 \, mol$ of $Cu^{2+}$ to $Cu$.
$(iii)$ $1 \, mol$ of $MnO_{4}^{-}$ to $Mn^{2+}$.

$A$ solution of $CuSO_4$ is electrolysed using a current of $1.5 \ A$ for $10 \ minutes$. What mass of $Cu$ is deposited at the cathode (in $g$)? (Atomic mass of $Cu = 63.7$)

When a current of $9.65 \ A$ is passed for $10 \ \text{minutes}$,$3.0 \ g$ of metal is deposited. What is the equivalent weight of the metal?

What is the number of moles of electrons passed when a current of $2 \text{ A}$ flows through an electrolyte solution for $10 \text{ minutes}$?

During the electrolysis of an electrolyte,the number of ions produced is directly proportional to the