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Jenna
Jenna asked in Science & MathematicsChemistry · 5 years ago

Chemistry Help?

To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 4.1-L bulb, then filled it with the gas at 1.70 atm and 26.0 ∘C and weighed it again. The difference in mass was 7.9 g . Identify the gas.

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  • Ash
    Lv 7
    5 years ago

    P = 1.70 atm

    V = 4.1 L

    T = 26°C = 26 + 273.15 = 299.15 K

    m = 7.9 g

    R = 0.082 L atm / K mol

    PV = nRT

    PV = (m/M)RT

    M = mRT/PV = (7.9 x 0.082 x 299.15) / (1.70 x 4.1) = 27.80 mol/gm

    which is close to 28 g/mol for N₂ gas

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