Keq for the reaction below is 2400. If the initial conditions of the reaction are a 1.0 L flask that contains 0.024 mol NO (g), 2.0 mol N2 (g) and 2.6 moles of O2 (g), determine if this reaction is at equilibrium, and, if not which direction it will shift to reach equilibrium.

The answer to your question is it is not at equilibrium, it will move to the products.

Explanation:

Data

Keq = 2400

Volume = 1 L

moles of NO = 0.024

moles of N₂ = 2

moles of O₂ = 2.6

Process

1.- Determine the concentration of reactants and products

[NO] = 0.024 / 1 = 0.024

[N₂] = 2/1 = 2

[O₂] = 2.6/ 1= 2.6

2.- Balanced chemical reaction

                     N₂ + O₂    ⇒   2NO

3.- Write the equation for the equilibrium of this reaction

                     Keq = [NO]²/[N₂][O₂]

- Substitution

                    Keq = [0.024]² / [2][2.6]

-Simplification

                    Keq = 0.000576 / 5.2

-Result

                    Keq = 1.11 x 10⁻⁴

Conclusion

It is not at equilibrium, it will move to the products because the experimental Keq was lower than the Keq theoretical-

                         1.11 x 10⁻⁴ < 2400

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