i$)$ Calculate the production rate of aluminum $($in $kg/$day$)$ in a $150,000$amp Hall$-$Heroult cell

operating at $95\%$ current efficiency with respect to the formation of $Al$ at the cathode.

The overall reaction involving aluminum reduction is

$2A{l}_2{O}_3(l)+3C(s)4Al(l)+3C{O}_2(g)$

Carbon is fed continuously into the cell and is "baked" by the heat within the reactor to

continually form anodes which are consumed by the above reaction. Determine the rate

$($in $k\frac{g}{?}$ day$)$ at which carbon must be fed into the cell to maintain the above current under

steady state conditions assuming the oxidation of carbon to $C{O}_2(g)$ is the only anodic

process that occurs.

ii$)$ Under normal conditions, a small amount of the $C{O}_2$ produced at the anode can be

transported to the cathode where it is reduced to $CO$ by the reaction

$C{O}_2(g)+2e^{-}CO(g)+O^{2-}$

Consider that this is the side reaction that consumes $5\%$ of the cathodic current for the

conditions described in i$)$ above. Determine the rate $($in $k\frac{g}{?}$ day $)$ at which $C{O}_2(g)$ and

$CO(g)$ are produced in the cell.