$A$ current of $2.0 \ A$ is passed for $5 \ hours$ through a molten metal salt,which deposits $22.2 \ g$ of metal (At. wt. $= 177$). The oxidation state of the metal in the metal salt is:

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

For the reaction $Al^{3+} + 3e^{-} \rightarrow Al$ (atomic mass of $Al = 27 \ g \ mol^{-1}$),calculate the quantity of electricity in coulombs required to produce $5.12 \ kg$ of $Al$.

$108 \ g$ of silver (molar mass $108 \ g \ mol^{-1}$) is deposited at the cathode from $AgNO_3(aq)$ solution by a certain quantity of electricity. The volume (in $L$) of oxygen gas produced at $273 \ K$ and $1 \ bar$ pressure from water by the same quantity of electricity is ............. $L$.

How many Faraday of electricity is required to produce $5 \ g$ of magnesium from magnesium chloride (in $F$)? (Molar mass $Mg = 24 \ g \ mol^{-1}$)

When a current of $10800 \ C$ is passed through an electrolyte,$2.977 \ g$ of a metal is deposited. If the molar mass of the metal is $106.4 \ g \ mol^{-1}$,what is the charge on the metal cation?