Nitrogen and hydrogen are combined in a reaction vessel. Equilibrium is then established, producing a gaseous mixture of nitrogen, hydrogen and ammonia. $\text{N}_2 + 3\text{H}_2 \rightleftharpoons 2\text{NH}_3$ At equilibrium, the gas mixture has a total pressure of $300\,\text{atm}$. The amounts present are shown below. Nitrogen: $180$ mol Hydrogen: $590$ mol Ammonia: $160$ mol Calculate the equilibrium constant, $K_p$, for the forward reaction.
- A$6.65 \times 10^{-6}\,\text{atm}^{-2}$
- B$7.13 \times 10^{-5}\,\text{atm}^{-2}$
- C$0.599\,\text{atm}^{-2}$
- D$1.50 \times 10^{5}\,\text{atm}^{2}$