Question: 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

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
2N2(g) + O2(g) ⇌ 2N2O(g)
If [N2] = 2.00 × 10-4 M, [N2O] = 0.200 M, and [O2] = 0.00245 M, does this represent a system at equilibrium?

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