IUPAC-NIST Solubility Database
NIST Standard Reference Database 106

Glass Ball as Bullet Solubility System: Ethene with Methanol
Components:
   (1) Ethene; C2H4; [74-85-1]  NIST Chemistry WebBook for detail
   (2) Methanol; CH4O; [67-56-1]  NIST Chemistry WebBook for detail
Original Measurements:
   Boyer, F. L.; Bircher, L. J., J. Phys. Chem. 1960, 64, 1330 - 1331.

 Variables:
   Temperature = 298.15 K
   Pressure = 101.325 kPa (1 atm)

 Prepared By:
   M.E. Derrick, H.L. Clever

 Experimental Remarks:
   The Bunsen coefficient was calculated by the compiler.
The mole fraction solubility was taken from Boyer's thesis1.
The author's observed a linear relationship between the logarithm of the mole fraction solubility and the number of linear alcohol carbon atoms. Boyer's thesis gives the equations:
log x1 = –2.387 + 0.543 log C for 298.15 K
log 1 = –2.474 + 0.580 log C for 308.15 K
where C is the number of alcohol carbon atoms. Most of the mole fraction solubility values given in Table II fo the paper were calculated from the equation for 298.15 K.

 Experimental Data:   (Subscripts 1,2,3, ..., in column headings refer to components 1,2,3, ...)
   
T/KOstwald coefficient L [cm3 cm–3]αα NoteMole Fraction (x1)
298.152.63 ± 0.022.41143.9
 Notes:
   1  α/cm3 (STP) cm–3 atm–1

 Method/Apparatus/Procedure:
   A commercial Van Slyke blood gas apparatus (E. H. Sargent Co.) was modified by the authors.

The total pressure of the gas and the solvent vapor in the solution chamber was adjusted to a pressure of one atm. The pressure was maintained at one atm during the solution process. The saturated solution was transferred to a bulb below the lower stopcock of the extraction vessel and sealed off. The gas and solvent vapor were then brought to volume over mercury. See2 for details of the extraction procedure.

Source and Purity of Materials:
   (1) Ethene. Matheson Co. Stated to be 99.5 mol per cent.
   (2) Methanol. Source not given. Treated by standard methods to remove aldehydes and ketones, then dried and distilled.

 Estimated Errors:
   Solubility: δL/cm3 = ± 0.02
   Temperature: δT/K = ± 0.01

 References:
   1. Boyer, F. L., Ph.D. thesis, 1959, Vanderbilt Univ., Nashville, TN.
   2. Peters, J. P.; Van Slyke, D. D.; Quantitative Clinical Chemistry, Baltimore, MD, 1932, Volume II.