The atomic weight of $Fe$ is $56$. The weight of $Fe$ deposited from $FeCl_3$ solution by passing $0.6$ Faraday of electricity is $............$ $g$.

$A$ solution of copper sulphate $(CuSO_4)$ is electrolysed for $10 \, \text{minutes}$ with a current of $1.5 \, \text{amperes}$. The mass of copper deposited at the cathode (atomic mass of $Cu = 63 \, u$) is ............ $g$.

For the given reaction how much quantity of electricity in Coulomb is required? $\frac{2}{3} Al_2O_3 \rightarrow \frac{4}{3} Al + O_2$

How much time is required for complete decomposition of $4 \, \text{moles}$ of water using $4 \, \text{A}$ current?

Aluminum oxide is electrolyzed at $1000^\circ C$ to produce aluminum metal. The cathode reaction is $Al^{3+} + 3e^- \rightarrow Al$. What quantity of electricity is required to produce $5.12 \ kg$ of aluminum metal? (Given: $1 \ Faraday = 96500 \ C$)

Two electrolytic cells containing molten solutions of nickel chloride and aluminium chloride are connected in series. If the same amount of electric current is passed through them,what will be the weight of nickel obtained when $18 \ g$ of aluminium is obtained (in $g$)? $[Al = 27 \ g/mol, Ni = 58.5 \ g/mol]$