Problem #$1$: Reaction to form ammonia. Ammonia is created in high pressure and high temperature according to the following reaction in the gas phase. A gas stream enters a reactor with a flowrate of $10$ moles $\frac{?}{h{r}^{-}{N}_2},33$ moles$/$hr of $H_2$ and $0\mathrm{.}5$ moles $\frac{?}{hr}$ of $N{H}_3$ along with $1\mathrm{.}5mo\frac{l}{h}r$ of argon gas $($this is an inert and doesn't react$).$ You measure the outlet and find that there are $5\mathrm{.}55$ moles$/$hr of $N_2$ leaving the reactor. Your job is to calculate the mass fraction of $N_2,H_2,N{H}_3$ and inert in the stream leaving the reactor.

$N_2(g)+3H_2(g)=2N{H}_3(g)$

a$.(2)$Draw and label the diagram. Include all species entering and leaving the reactor.

b$.(2)$ Write out the mole balance for each species present. Use this to determine the limiting reactant and the extent of reaction $($B$).$

c$.(2)$ Fill out a SPICEY table and determine the mol fraction of each species leaving the reactor.