Chemistry Gas and STP problem? Help!!?

What is the molecular weight of a gas that occupies a volume of 278 mL, at a pressure of 680.0 mm Hg, a temperature of 21.7 degrees C, and a mass of 35.9 grams?

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  • Lexi R
    Lv 7
    9 years ago
    Favorite Answer

    Using the STP method involves ...

    1. Using the combined gas equation to calculate the volume of the gas at STP

    2. using this volume to calculate moles of gas (since 1 mole any ideal gas at STP occupies 22.4 L

    3. You now know the mass and moles of the sample (molar mass = mass / moles)

    P1V1/T1 = P2V2/T2

    P1 = 680.0 mmHg

    V1 = 278 ml

    T1 = 294.85 K

    P2 = 760.0 mmhg

    V2 = ? ml

    T2 = 273.15 K

    V2 = P1V1T2 / P2T1

    = 680.0 mmHg x 278 ml x 273.15 K / (760.0 mmHg x 294.85 K)

    = 230.4 ml

    Now, at STP the volume of 1 mole of any ideal gas = 22.4 L

    So moles gas = volume at STP / 22.4 L/mol

    = 0.2304 L / 22.4 L/mol

    = 0.01029 mol

    moles = mass / molar mass

    Therefore molar mass = mass / moles

    = 35.9 g / 0.01029 mol

    = 3488.8 g/mol

    = 3490 g/mol (3 sig figs)

    The alternative way of doing this problem is to use the equation

    PV = mRT / Mw

    where

    Mw = molar mass

    P = pressure

    V = volume

    m = mass

    R = gas constant

    T = temp in Kelvin

    (obviously you have to be able to either remember or look up the gas constant (R) to do this one.)

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