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Finding the number of molecules

  1. Nov 8, 2006 #1
    :confused:

    Current vacuum technology can achieve a pressure of 1 * 10^-10 mm of Hg. At this pressure, and at a temperature of 30.0 C, how many molecules are in 5.00 cm3 ?

    ok so atomic number of Hg = 80

    80 * 1.661 * 10^-27 yields 1.33 * 10 ^-25 which is the mass of one molecule

    converting from mm to atmospheres i get 1*10^-10 mm = 1.32 * 10 ^-13 atm since 760 mm = 1 atm

    T = 303
    5 cm3 = 5 ml = 5 * 10 ^ -3

    so using pV = nRT
    (1.32*10^-13)(5*10^-3) = n(.08206)pressure constant(303)
    solving for n... n = 2.6459

    n = M(in grams)/M of molecule so :
    2.6459 = M/80
    which gives me 211.67 grams....

    N (number of molecules = M/m = .21167 Kg/1.33 * 10^-25 (mass of one molecule)

    which yields me 1.59 * 10^ 24 molecules.... this answer is incorrect... any ideas?
     
  2. jcsd
  3. Nov 8, 2006 #2
    actually i think that i should be using 201 for the atomic number of mercury... this still ends up yielding 3.99 *10^24 which is still incorrect.
     
  4. Nov 8, 2006 #3
    actually, it yields 1.59 * 10^24....
     
  5. Nov 9, 2006 #4

    OlderDan

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  6. Nov 10, 2006 #5
    I'm not sure why you are going into mass of molecules... if you use PV=nRT, n is the number of moles. You can convert directly from moles to molecules using good ole 6.02E23. According to the IDEAL GAS LAW, the same number of moles of a gas ALWAYS occupy the same volume... regardless of WHAT the gas is.
     
  7. Nov 10, 2006 #6

    dextercioby

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    Incidentally, Hg (mercury) is a metal, and with metals we never speak about "molecules". In this problem it instructve to use the van der Waals state law, too and compare the 2 results.

    Daniel.
     
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