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27 August, 04:26

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [H2]eq = 0.14 M, [Cl2]eq = 0.39 M, [HCl]eq = 1.6 M. H2 (g) + Cl2 (g) ⇌ 2 HCl (g) 8.7 * 10-22.1 * 10-229473.4 * 10-2

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  1. 27 August, 05:51
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    Kc = 47

    Explanation:

    From the given equation,

    H₂ (g) + Cl₂ (g) ⇌ 2 HCl (g)

    The equilibrium constant for the above reaction, can be written as the product of the concentration of product raised to the power of stoichiometric coefficients in a balanced equation of dissociation divided by the product of the concentration of reactant raised to the power of stoichiometric coefficients in the balanced equation of dissociation.

    Hence,

    Kc = [HCl (g) ]² / [ Cl₂ (g) ] [ H₂ (g) ]

    From the question,

    [HCl (g) ] = 1.6 M

    [ Cl₂ (g) ] = 0.39 M

    [ H₂ (g) ] = 0.14 M

    Now, putting it in the above equation,

    Kc = [HCl (g) ]² / [ Cl₂ (g) ] [ H₂ (g) ]

    Kc = [ 1.6 M ]² / [ 0.39 M ][ 0.14 M ]

    Kc = 47
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