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8 July, 00:22

For the chemical equation SO2 (g) + NO2 (g) SO3 (g) + NO (g) SO2 (g) the equilibrium constant at a certain temperature is 3.00. At this temperature, calculate the number of moles of NO2 (g) that must be added to 2.30 mol SO2 (g) in order to form 1.00 mol SO3 (g) at equilibrium.

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  1. 8 July, 00:50
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    The number of initial moles of NO2 are 1.256 moles

    Explanation:

    Step 1: Data given

    K = 3.00

    Moles of SO2 = 2.30 moles

    Moles SO3 formed = 1.00 moles

    Step 2: The balanced equation

    SO2 (g) + NO2 (g) → SO3 (g) + NO (g)

    Step 3: The initial number of moles

    SO2 = 2.30 moles

    NO2 = Y moles

    SO3 = 0 moles

    NO = 0 moles

    Step 4: The number of moles at equilibrium

    For 1 mol SO2 we need 1 mol NO2 to produce 1 mol SO3 and 1 mol NO

    SO2 = 2.30 - X moles

    NO2 = Y - X moles

    SO3 = X moles

    NO = X moles

    At the equilibrium we have 1.00 mol SO3

    SO3 = X moles = 1.00

    X = 1.00

    Moles SO2 = 2.30 - 1.00 = 1.30

    Moles NO2 = Y-1.00

    SO3 = 1.00 moles

    NO = 1.00 moles

    Step 5: Calculat Kc

    Kc = [NO][SO3] / [NO2][SO2]

    3.00 = (1.00 * 1.00) / (1.30 * (Y-1.00))

    3.00 = 1 / (1.30Y - 1.30)

    1 = 3 * (1.30Y - 1.30)

    1 = 3.90Y - 3.90

    4.90 = 3.90Y

    Y = 1.256

    The number of initial moles of NO2 are 1.256 moles
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