How many Coulombs of electricity are required for the oxidation of one mol of water to dioxygen?

What is the charge on tin if $7.375 \ g$ of metallic tin is deposited by the passage of $24125 \ C$ through a solution containing the ion? [Atomic weight of $Sn = 118 \ g/mol$]

When a current of $0.5 \ A$ is passed for $2 \ hours$ through a molten metal salt,$3.88 \ g$ of the metal was deposited. If the atomic mass of the metal is $208 \ units$,the oxidation state of the metal in the salt is:

$CuSO_4$ solution is electrolysed for $15 \ minutes$ to deposit $0.4725 \ g$ of copper at the cathode. The current in amperes required is (Faraday $= 96,500 \ C \ mol^{-1}$,atomic weight of copper $= 63$)

The amount of copper metal deposited at the cathode on passing an electric current of $500 \, mA$ for $20 \, minutes$ in a cupric chloride solution is ............ $g$.

The electrochemical equivalent of a metal is $3.3 \times 10^{-7} \ kg/C$. The mass of the metal liberated at the cathode when a $3 \ A$ current is passed for $2 \ s$ will be: