Chapter 12, Problem 28E

At a particular temperature a 2.00-L flask at equilibrium contains 2.80 × 10⁻⁴ mole of N₂, 2.50 × 10⁻⁵ mole of O₂, and 2.00 × 10⁻² mole of N₂O. Calculate K at this temperature for the reaction

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

If [N₂] = 2.00 × 10⁻⁴ M, [N₂O] = 0.200 M, and [O₂] =0.00245 M, does this represent a system at equilibrium?