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21 February, 20:39

On analysis, an equilibrium mixture for the reaction 2H2S (g) LaTeX: / longleftrightarrow⟷ 2H2 (g) + S2 (g) was found to contain 1.0 mol H2S, 4.0 mol H2, and 0.80 mol S2 in a 4.0 L vessel. Calculate the equilibrium constant, Kc, for this reaction. Group of answer choices

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  1. 21 February, 21:00
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    The equilibrium constant Kc = 3.2

    Explanation:

    Step 1: Data given

    Number of moles H2S = 1.0 moles

    Number of moles H2 = 4.0 moles

    Number of moles S2 = 0.8 moles

    Volume = 4.0 L

    Step 2: The balanced equation

    2H2S (g) ⟷ 2H2 (g) + S2 (g)

    Step 3: Calculate concentration

    Concentration = moles / volume

    [H2S] = 1.0 moles / 4.0 L

    [H2S] = 0.25 M

    [H2] = 4.0 moles / 4.0 L

    [H2] = 1.0 M

    [S2] = 0.80 moles / 4.0 L

    [S2] = 0.20 M

    Step 4: Calculate Kc

    Kc = [S2][H2]² / [H2S]²

    Kc = (0.20 * 1.0²) / 0.25²

    Kc = 3.2

    The equilibrium constant Kc = 3.2
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