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Find the pressure of the elements.

  1. May 23, 2015 #1
    1. The problem statement, all variables and given/known data
    A compound of ether (0.287 g) and chloroform (0.568 g) evaporates in the temperature 373 K in an empty container with volume 0.0001m3. Find the pressure of each element. I don't know which formula of ether should I use since there are many. However even if I knew the n of moles for example n I would do these actions: pV=nRT. Since the T is the same: T=p1V1/n1R=p2V2/n2R=> 373=p1x/n1=p2(0.0001-x)/n2. What should I do next?

    2. Relevant equations
    pV=nRT
    3. The attempt at a solution
    I don't know which formula of ether should I use since there are many. However even if I knew the n of moles for example n I would do these actions: pV=nRT. Since the T is the same: T=p1V1/n1R=p2V2/n2R=> 373=p1x/n1=p2(0.0001-x)/n2. What should I do next?
     
  2. jcsd
  3. May 23, 2015 #2

    SteamKing

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    You can roll the dice and assume the problem is talking about diethyl ether, which is the compound commonly referred to when talking about "ether":

    http://en.wikipedia.org/wiki/Diethyl_ether

    Like chloroform, ether was once used as an anesthetic.
     
  4. May 23, 2015 #3
    ok, but what should I do next?
     
  5. May 23, 2015 #4

    SteamKing

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  6. May 23, 2015 #5
  7. May 23, 2015 #6

    Borek

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    Just treat each substance separately, as if there were no other present. That's how gases behave (and that's what partial pressures are about).
     
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