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Am I doing this vapour pressure problem correctly?

  1. Aug 30, 2015 #1
    1. The problem statement, all variables and given/known data
    'The vapour pressure of ethanol (C2H5OH) at 19°C is 40.0 torr. A 1.00-g sample of ethanol is placed in a 2.00 L container at 19°C. If the container is closed and the ethanol is allowed to reach equilibrium with its vapour, how many grams of liquid ethanol remain?'

    2. Relevant equations
    PV = nRT
    R = 62.36 L⋅torr / mol⋅K

    3. The attempt at a solution
    Basically, when I tried to plug in all the numbers into the ideal gas equation (with the given mol number of 1/46), it wasn't quite equal. Then I figured, that not all the ethanol is converted into vapour; only some of it. And this equation really only applies to gases (a.k.a. vapours). I didn't know how much, so that's basically what I set out to find out with what I was given.

    (40.0 torr)(2.00 L) = (x mol)(62.36 L⋅torr/1 mol⋅K)(292 K)
    80 L⋅torr = x19209.12 L⋅torr
    x = 0.0044 mol C2H5OH (g)
    0.0044 mol(46.06844 g/1 mol) = 0.203 g C2H5OH (g)
    1.00 - 0.203 = 0.797 g C2H5OH (l)
     
    Last edited: Aug 30, 2015
  2. jcsd
  3. Aug 30, 2015 #2

    Borek

    User Avatar

    Staff: Mentor

    Looks OK to me.
     
  4. Aug 30, 2015 #3
    Thank you.
     
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