Nitrogen Can React with Oxygen to Form Nitrogen Monoxide $\mathrm{N}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})$

Nitrogen can react with oxygen to form nitrogen monoxide. $\mathrm{N}_{2}(\mathrm{~g}) +\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})$ $\quad$$\quad$$\quad$ $K=1.0 \times 10^{30} \text { at } 25^{\circ} \mathrm{C}$
When equilibrium is established,the partial pressures of nitrogen and oxygen are 1.2 atm and 3.1 atm,respectively.What is the equilibrium pressure of nitrogen monoxide?

A) 3.7 × 10−³⁰ atm
B) 1.9 × 10−¹⁵ atm
C) 2.7 × 10−¹³ atm
D) 1.9 × 10−¹⁰ atm
E) 3.7 × 10−⁷ atm