a$.$ Tyrosine $(C_9{H}_{11}N{O}_3)$ is one of the amino acids that are used by cells to synthesize proteins. Assume tyrosine is oxidized to $C{O}_2,H_{2}O,$ and $N{H}_3$ in aerobic conditions, complete the following equation to check the process of this reaction.

$C_9{H}_{11}N{O}_3+O_2$

b$.$ Calculate the carbonaceous COD $($as in $mg\frac{O_2}{L})$ of the solution if initial tyrosine concentration is $100m\frac{g}{L}.$

c$.$ Assuming that the $BO{D}_5$ of a water sample containing tyrosine is $65m\frac{g}{L},$ bacterial consumption rate constant $k=0\mathrm{.}22d^{-1}($base e$),$ calculate its ultimate BOD.

BOD rate equation:

Where,

$BO{D}_t=L(1-e^{-k*t})$

$L$ is ultimate BOD$[m\frac{g}{L}],$

$BO{D}_t$ is oxygen consumed after time $t[m\frac{g}{L}],$

$k$ is the rate constant for bacteria consumption of organic matters $d^{-1},$

$t$ is time $[$d$].$