The first step in producing pure lead from galena $(PbS)$ is as follows: $ 2{PbS}(s) + 3{O}_2(g) \longrightarrow 2{PbO}(s) + 2{SO}_2(g) $. All of the following are true concerning this reaction except:
Ammonia burns in air to form nitrogen dioxide and water. $4{NH}_3(g) + 7{O}_2(g) \longrightarrow 4{NO}_2(g) + 6{H}_2{O}(l) $ If 8 moles of $NH_3$ are reacted with 14 moles of $O_2$ in a rigid container with an initial pressure of 11 atm, what is the partial pressure of $NO_2$ in the container when the reaction runs to completion? (Assume constant temperature)