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HELP - Molar mass changes at stp?

  1. Apr 17, 2005 #1
    PLZ HELP - Molar mass changes at stp?!?!

    Hey, I have this lab report due tomorrow, and I seem to be getting some discrepencies in my calculations. I am calculating the molar mass of butane, without using the values from the periodic table, using data obtained by the experiment below:

    Pressure: 101.09 kPa
    Temperature: 23ºC --> 296 K
    Initial Mass of Lighter: 18.19g
    Secondary Mass of Lighter: 18.06g
    Mass of Butane used: 0.15g
    Volume of Butane: 50.2

    I won't bother you with error propagation as it is easy to caculate, so disregard that. Below are my calculations for the molar mass of butane, at the temp and pressure given above and at STP (standard temp and pressure).
    Am I doing this properly? Do my results make sense? (Ignore the "..." they are for placement)

    Molar Mass of Butane at Given Temperature and Pressure:

    50.2 +/- 1.0mL X 1.0L = 5.02 x 10^-2 L

    P = nRT --> n = PV

    n = 101.09kPa (5.02 x 10-2L)
    .......8.31kPa.L/mol.K (296K)

    n = 2.06 x 10^-3 molButane

    M = m

    M = 0.15g .
    ......2.06 x 10^-3 molButane

    M = 72.71g/molButane

    Molar Mass of Butane at STP:

    T1 = 296K P1 = PTotal – PH20 P2 = 101.3kPa
    T2 = 273K = 101.09kPa – 2.81kPa V1 = 50.2mL
    = 98.28kPa

    50.2 mL X 273K X 101.3kPa = 47.7mL = 4.77 x 10^-2 L

    P = nRT --> n = PV

    n = 101.3kPa(4.77 x 10^-2 L)
    ........8.31kPa.L/mol.K (273K)

    n = 2.13 x 10^-3 molButane

    M = m

    M = 0.15g .
    .......2.13 x 10^-3 molButane

    M = 70.42g/molButane

    I know i've done something wrong but don't know what.

    Thanks you SO much,
  2. jcsd
  3. Apr 17, 2005 #2
    OMG!!!!! Sorry, i made the dumbest error. The mass of butane is 0.13g not 0.15....i subtracted the data wrong by 0.02 and it changed the answer by around 9g/mol!!!!!!!!

    but still, should i be getting different answers for each case? Why is this or is it not?

    Last edited: Apr 17, 2005
  4. Apr 18, 2005 #3


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    Staff Emeritus
    Science Advisor

    No, you should not be getting different answers. One mol of a quantity contains a specific number of molecules (Avogadro's number) and so has a specific mass. That doesn't change just because you change temperature and pressure (although the volume might.)
  5. Apr 18, 2005 #4


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    Science Advisor
    Homework Helper
    Gold Member

    You might try the "easy" part.
  6. Apr 18, 2005 #5
    Oh I did the "easy" part in my lab notebook of course. Since i made the correction (post 2 of mine) i have values approx 61 and 64. But I think I'm using the wrong equation or something..because ivy is right, molar mass should always stay the same.
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