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11 May, 09:58

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.

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  1. 11 May, 13:01
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    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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