Faraday's $2^{nd}$ law of electrolysis states that the mass of a substance deposited at an electrode is directly proportional to its:

The mass of carbon anode consumed (giving only carbon dioxide) in the production of $270 \ kg$ of aluminium metal from bauxite by the Hall process is ............... $kg$.

What current strength is required to deposit $36 \ g$ of $Ag$ in $7 \ minute$ from $AgNO_3$ solution by electrolysis (in $A$)? (Atomic mass $Ag = 108$)

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

In electrolysis,if the duration of the passage of current is doubled,the mass liberated is

Aqueous copper sulphate solution and aqueous silver nitrate solution are electrolysed by $1 \ A$ current for $10 \ minutes$ in separate electrolytic cells. Will the mass of copper and silver deposited on the cathode be same or different? Explain your answer.