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2 July, 07:34

To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed

an empty 3.1-L bulb, then filled it with the gas at 1.00 atm and 28.0 °C and weighed it again.

The difference in mass was 3.5 g. Identify the gas.

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Answers (1)
  1. 2 July, 09:05
    0
    Aluminium

    Explanation:

    Given dа ta:

    Volume = 3.1 L

    Pressure = 1.0 atm

    Temperature = 28.0 °C (28 + 273.15 = 301.15 K)

    Mass = 3.5 g

    Identify the gas.

    Solution:

    First of all we will find the number of moles.

    PV = nRT

    n = PV/RT

    n = 1 atm * 3.1 L / 0.0821 L. atm. K⁻¹. mol⁻¹ * 301.15 K

    n = 3.1 L. atm / 24.72 L. atm. mol⁻¹

    n = 0.13 mol

    Now we will find the molar mass.

    molar mass = 3.5 g / 0.13 mol

    molar mass = 26.9 g/mol

    The gas is diatomic so, atomic mass will be half of 26.9 g/mol.

    26.9 g/mol / 2 = 13.45 g/mol

    The element which has atomic mass closer to the 13.45 is aluminium.
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