Chapter 6, Problem 27E

At a particular temperature, a 2.00-L flask at equilibriumcontains $\text{2}{\text{.80×10}}^{\text{-4}}{\text{mole of N}}_{\text{2}}\text{, 2}{\text{.50×10}}^{\text{-5}}{\text{mole of O}}_{\text{2}}\text{, and 2}{\text{.00×10}}^{\text{-2}}{\text{mole of N}}_{\text{2}}\text{O}$ . Calculate K at thistemperature for the reaction

${\text{2N}}_2\left(g\right)+{\text{O}}_2\left(g\right)\rightleftharpoons {\text{2N}}_2\text{O}\left(g\right)$

If [N2] 5 2.00 3 1024 M, [N2O] 5 0.200 M, and [O2] 50.00245 M, does this represent a system at equilibrium?