Chapter 6, Problem 107CP

At 1000 K the ${\text{N}}_{\text{2}}\text{(}g{\text{) and O}}_{\text{2}}\text{(}g\text{)}$ in air (78% N2, 21% ${\text{O}}_{\text{2}}$ ,by moles) react to form a mixture of NO(g) and ${\text{NO}}_{\text{2}}\text{(}g\text{)}$ .The values of the equilibrium constants are $1.5\times {10}^{-4}\text{and }1.0\times {10}^{-5}$ for the formation of NO(g) and ${\text{NO}}_{\text{2}}\text{(}g\text{)}$ ,respectively. At what total pressure will the partial pressuresof NO(g) and ${\text{NO}}_{\text{2}}\text{(}g\text{)}$ be equal in an equilibriummixture of ${\text{N}}_{\text{2}}\text{(}g\text{)}$ , ${\text{O}}_{\text{2}}\text{(}g\text{)}$ , NO(g), and ${\text{NO}}_{\text{2}}\text{(}g\text{)}$ ?