Problem: At a particular temperature a 2.00-L flask at equilibrium contains 2.80 x 10 -4 mole of N2, 2.50 x 10 -5 mole of O2, and 2.00 x 10 -2 mole of N2O. Calculate K at this temperature for the reaction2N2(g) + O2(g) ⇌ 2N2O(g)If [N2] = 2.00 x 10 -4 M, [N2O] = 0.200 M, and [O2] = 0.00245 M, does this represent a system at equilibrium?

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

2N2(g) + O2(g) ⇌ 2N2O(g)

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

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