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At a particular temperature a 2.00-L flask at equilibrium contains 2.80 x 10 ^{-4} mole of N_{2}, 2.50 x 10 ^{-5} mole of O_{2}, and 2.00 x 10 ^{-2} mole of N_{2}O. Calculate *K* at this temperature for the reaction

2N_{2}(*g*) + O_{2}(*g*) ⇌ 2N_{2}O(*g*)

If [N_{2}] = 2.00 x 10 ^{-4} M, [N_{2}O] = 0.200 M, and [O_{2}] = 0.00245 M, does this represent a system at equilibrium?