Given that the reaction between nitrogen and hydrogen to produce ammonia is written as

$\frac{1}{2}{N}_2+\frac{3}{2}{H}_2>N{H}_3$

and the equilibrium constant, $K_p$ given as

$K_p=\frac{p_{N{H}_3}}{p_{N_2}^{\frac{1}{2}}{p}_{H_2}^{\frac{3}{2}}}=\frac{y_{N{H}_2}}{y_{N_2}^{\frac{1}{2}}{y}_{H_2}^{\frac{3}{2}}}\frac{1}{p}$

Find the molar flow rates of all species out of an equilibrium reactor at $589K$ when the inlet values of

nitrogen, hydrogen, and ammonia flow rates are $1\mathrm{.}1,3,$ and $0\mathrm{.}2mo\frac{l}{h}$ and the equilibrium constant is

$0\mathrm{.}05.$ Use $220$atm for the pressure.