Chemistry

H2 (g) + I2 (g) 2 HI (g)
If the initial concentrations of H2 and I2 are 1.0 M and the initial concentration of HI is 0.5 M (Kc = 54.3 at 430oC).
(a) Is the reaction at equilibrium?

(b) If not, which way will the reaction proceed?

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asked by Troy
  1. Let K=[HI]²/([H2][I2])

    The given reaction is in equilibrium at 430°C, if K=Kc=54.3

    Substitute given concentrations to get
    K=[HI]²/([H2][I2])
    =0.5²/(1*1)
    =0.25 < 54.3
    Therefore the reaction is not in equilibrium and will proceed in the forward direction until K=Kc.

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    posted by MathMate

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