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30 May, 04:18

At a particular temperature, 12.6 mol of SO3 is placed into a 4.0-L rigid container, and the SO3 dissociates by the reaction given below. 2 SO3 (g) equilibrium reaction arrow 2 SO2 (g) + O2 (g) At equilibrium, 3.4 mol of SO2 is present. Calculate K for this reaction.

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  1. 30 May, 04:40
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    At equilibrium, Kc = 0.058

    Explanation:

    Step 1: Data given

    Mol SO3 = 12.6

    Volume = 4.0 L

    At equilibrium we have:

    3.4 mol of SO2

    Step 2: The balanced equation

    2SO3 (g) + ⇆ 2SO2 (g) + O2 (g)

    Step 3: ICE-chart

    The initial number of moles are:

    SO3: 12.6 moles

    SO2 : 0 mol

    O2: 0 mol

    There will react:

    SO3: - 2x

    SO2: + 2x

    O2: + x

    The number of moles at the equilibrium are:

    SO3: 12.6 - 2x

    SO2: 2x = 3.4 mol

    O2: x

    Since at the equilibrium, we have 2x = 3.4 mol. x = 1.7 mol

    This means at the equilibrium we have 1.7 mol of O2 and 12.6 - 3.4 = 9.2 mol of SO3

    Step 4: Calculate the equilibrium constant Kc

    Kc = [3.4/4]² * [1.7/4] / [9.2/4]²

    Kc = 0.058

    At equilibrium, Kc = 0.058
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