In the Hall-Heroult process,if a current of $10 \ A$ is passed for $8 \ \text{days}$ and $1 \ \text{hour}$,how many kilograms of carbon anode will be consumed?

On passing $1 \ F$ of electricity through electrolytic cells containing $Ag^{+}$,$Ni^{2+}$,and $Cr^{3+}$ ions,the mass of $Ag$ $(At. wt. = 108)$,$Ni$ $(At. wt. = 59)$,and $Cr$ $(At. wt. = 52)$ deposited is:

How many total Faraday currents will be required to obtain $1 \ mole$ of $Ag$,$Mg$,and $Al$ respectively?

The electrochemical equivalent of a metal is $x \ g \ C^{-1}$. The equivalent weight of the metal is:

Faraday's laws of electrolysis will fail when

$A$ constant current $(0.5 \, A)$ is passed for $1 \, hour$ through $(i)$ aqueous $AgNO_3$,$(ii)$ aqueous $CuSO_4$ and $(iii)$ molten $AlF_3$,separately. The ratio of the mass of the metals deposited on the cathode is $[M_{Ag}, M_{Cu}, M_{Al}$ are molar masses of the respective metals.]