Chapter 14, Problem 14.2A

APPLY 14.2 Nitrogen dioxide, a pollutant that contributes to photochemical smog, isformed by a series of two reactions.

$\begin{array}{l}{\text{N}}_2\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)\rightleftarrows 2\text{NO}\left(g\right)K_{C1}=4.3\times {10}^{-25}\\ 2\text{NO}\left(g\right)+{\text{O}}_2\left(g\right)\rightleftarrows 2{\text{NO}}_{\text{2}}\left(g\right)K_{C2}=6.4\times {10}^9\end{array}$

__________________________________________

${\text{N}}_2\left(g\right)+2{\text{O}}_{\text{2}}\left(g\right)\rightleftarrows 2{\text{NO}}_{\text{2}}\left(g\right)K_C\left(\text{overall}\right)=?$

(a) Write the equilibrium constant expression for the overall reaction.

(b) What is the value of K_C(overall)?