In $CuSO_4$ solution,when an electric current equal to $2.5 \ F$ (faraday) is passed,the number of $gm$ equivalents deposited on the cathode is:

On passing a current through molten $KCl$,$19.5 \ g$ of potassium is deposited. If the same quantity of electricity is passed through molten aluminium chloride,then the amount of aluminium deposited will be ............. $g$.

The current flowing in a copper voltameter is $1.6 \ A$. The number of $Cu^{2+}$ ions deposited at the cathode per minute are

On passing $3 \ A$ of electricity for $50 \ minutes$,$1.8 \ g$ of metal deposits. The equivalent mass of the metal is:

$250 \ mL$ of a waste solution obtained from the workshop of a goldsmith contains $0.1 \ M \ AgNO_3$ and $0.1 \ M \ AuCl$. The solution was electrolyzed at $2 \ V$ by passing a current of $1 \ A$ for $15 \ minutes$. The metal/metals deposited will be
$(E^0_{Ag^+/Ag} = 0.80 \ V, E^0_{Au^+/Au} = 1.69 \ V)$

How much charge in coulombs is required for the reduction of one mole of $Al^{3+}$ to $Al$?