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13 June, 15:37

Consider the gas-phase reaction:

N2 (g) + 3H2 (g) ⇆ 2NH3 (g)

, for which Kp = 43 at 400 K.

If the mixture is analyzed and found to contain 0.18 bar of N2, 0.36 bar of H2 and 0.59 bar of NH3, describe the situation:

a) Q > K and more products will be made to reach equilibrium.

b) Q < K and more reactants will be made to reach equilibrium.

c) Q < K and more products will be made to reach equilibrium.

d) Q > K and more reactants will be made to reach equilibrium.

e) Within 1 decimal place, Q = K and the reaction is at equilibrium.

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Answers (1)
  1. 13 June, 19:27
    0
    Q < K and more products will be made to reach equilibrium (option C)

    Explanation:

    Step 1: Data given

    Kp = 43 at 400 K

    pressure of N2 = 0.18 bar

    Pressure of H2 = 0.36 bar

    Pressure of NH3 = 0.59 bar

    Step 2: The balanced equation

    N2 (g) + 3 H2 (g) 2 NH3 (g),

    Step 3: Calculate Q

    Kp = 43 = [NH3]² / [N2] [H2]³

    Q = [NH3]² / [N2] [H2]³

    Q = [0.59]² / [0.18] [0.36]³

    Q = 0.3481 / 0.00839808

    Q = 41.45

    Q < Kp

    When Q
    Option C is correct (Q < K and more products will be made to reach equilibrium)
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