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    bashful's Avatar
    bashful Posts: 1, Reputation: 1
    New Member

    Mar 4, 2007, 05:44 PM
    Convert: 5.6 liters of H2 at STP to molecules
    Capuchin's Avatar
    Capuchin Posts: 5,255, Reputation: 656
    Uber Member

    Mar 5, 2007, 12:26 AM
    PV = nRT?

    I don't understand the qestion :p

    H2 is a molecule...
    Evil dead's Avatar
    Evil dead Posts: 116, Reputation: -5
    Junior Member

    Mar 5, 2007, 02:35 PM
    ... what kind of question is this?

    Erm anyway I'll try my best.

    5.6 Litres of H2 (like they'll give a question with a well known gas as a liquid -.-) is 0.0056m3 as a volume (which it should be at)

    1 litre = 0.001m3 (or something like that)

    Any gas at STP occupied 24,000cm3... SO, maybe you're trying to find the grams or the moles of gas?

    wait are you on about? H2 is already a molecule (diatomic)... if you wanted it as a gas in normal volume units then what I did above is the way to go...
    rudi_in's Avatar
    rudi_in Posts: 251, Reputation: 45
    Full Member

    Mar 5, 2007, 02:47 PM
    Thank you for posting your question to the Ask Me Help Desk.

    Using the conversion factor of 1 mol H2/22.4 L H2 we can figure this out.

    5.6 L H2 x 1 mol H2/22.4 L H2 x 6.02x10^23 molecules H2/1 mol H2

    You should be able to solve it from here.
    fattybum4444's Avatar
    fattybum4444 Posts: 19, Reputation: 4
    New Member

    Nov 11, 2008, 10:01 AM

    use the equation pv=nrt
    p= pressure
    v= volume
    n= number of moles
    r= gas constant = 8.31jk-1mol-1
    t= temperature
    ... you have to convert the units into SI units first

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