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13 September, 02:23

To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 2.2-L bulb, then filled it with the gas at 2.00 atm and 27.0 ∘C and weighed it again. The difference in mass was 5.1 g. Identify the gas. Express your answer as a chemical formula.

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  1. 13 September, 02:26
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    N2

    Explanation:

    We use the ideal gas equation to calculate the number of moles of the diatomic gas. Then from the number of moles we can get

    Given:

    P = 2atm

    1atm = 101,325pa

    2atm = 202,650pa

    T = 27 degrees Celsius = 27 + 273.15 = 300.15K

    V = 2.2L

    R = molar gas constant = 8314.46 L. Pa/molK

    PV = nRT

    Rearranging n = PV/RT

    Substituting these values will yield:

    n = (202,650 * 2.2) / (8314.46 * 300.15)

    n = 0.18 moles

    To get the molar mass, we simply divide the mass by the number of moles.

    5.1/0.18 = 28.5g/mol

    This is the closest to the molar mass of diatomic nitrogen N2.

    Hence, the gas is nitrogen gas
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