The number of moles of electrons required to deposit $1 \, g$ equivalent of aluminium $(At. \, wt. = 27)$ from a solution of aluminium chloride will be

Calculate the mass of a divalent metal produced at the cathode by passing $5 \ A$ current through its salt solution for $100 \ minutes$. (Molar mass of metal $= x \ g/mol$)

The number of electrons required to deposit $1 \ g$ atom of aluminium (at. wt. $= 27$) from a solution of aluminium chloride will be ............ $N$ (where $N$ is Avogadro's number).

$0.50 \, L$ of a $0.60 \, M$ $CuSO_4$ solution is electrolyzed for a period of $30.0 \, min$ using a current of $4.60 \, A$. If inert electrodes are used,what is the final concentration of $Cu^{2+}$ remaining in the solution? $M$

How much charge in Coulombs is required for the oxidation of $1 \ mol$ of $H_2O$ to $O_2$?

If a current of $0.5 \ A$ is passed through a solution of $AgNO_3$ for $193 \ s$,$0.108 \ g$ of $Ag$ is deposited. What is the equivalent weight of $Ag$?