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16 May, 12:47

Consider the reaction at 500 ° C 500°C. N 2 (g) + 3 H 2 (g) - ⇀ ↽ - 2 NH 3 (g) K c = 0.061 N2 (g) + 3H2 (g) ↽--⇀2NH3 (g) Kc=0.061 If analysis shows that the composition of the reaction mixture at 500 ° C 500°C is 1.14 mol ⋅ L - 1 N 2 1.14 mol⋅ L-1N2, 5.52 mol ⋅ L - 1 H 2 5.52 mol⋅ L-1H2, and 3.42 mol ⋅ L - 1 NH 3 3.42 mol⋅ L-1NH3, what is the value of the reaction quotient Q Q?

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  1. 16 May, 13:00
    0
    Q = 0.061 = Kc

    Explanation:

    Step 1: Data given

    Temperature = 500 °C

    Kc=0.061

    1.14 mol/L N2

    5.52 mol/L H2

    3.42 mol/L NH3

    Step 2: Calculate Q

    Q=[products]/[reactants]=[NH3]² / [N2][H2]³

    If Qc=Kc then the reaction is at equilibrium.

    If Qc
    If Qc>Kc then the reaction will shift left to reach equilibrium.

    Q = (3.42) ² / (1.14 * 5.52³)

    Q = 11.6964/191.744

    Q = 0.061

    Q = Kc the reaction is at equilibrium.
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