Solubility Data Series 76
Solubility of Ethyne in Liquids
Peter G. T. Fogg,
Sim-wan Annie Bligh, M. Elizabeth Derrick, Yuri P. Yampol'skii, H.
Lawrence Clever, Adam Skrzecz, and Colin L. Young
IUPAC-NIST Solubility Data Series. 76.
Journal of Physical and Chemical Reference Data, Vol. 30, No.
6, pp. 1693-1875, 2001
Ethyne was probably first made in the laboratory by Edmund Davy in
1836. It was rediscovered nearly a quarter of a century later by Berthelot
who gave it the name acetylene. Since that time ethyne has become
a cheap raw material for the synthesis of organic materials and an
important industrial fuel. A summary of the available solubility data
for ethyne was published by Miller in 1965 [S. A Miller, Acetylene—Its
Properties, Manufacture, and Uses (Academic, New York, 1965),
Vol. I]. Many more data are now available in a wide range of research
papers and patent applications. These data vary in their reliability.
In the current work the data for systems included in Miller's book
have been reassessed and complemented by data published more recently.
Literature has been surveyed to 1999. Data for a system may be unreliable
unless two or more groups of workers have published values in close
agreement. Where possible values of the mole fraction solubility at
a partial pressure of 101.3 kPa have been tabulated. Equations have
been given for the variation of mole fraction with temperature in
cases in which values over a temperature range are available. The
greater the number of independent sources of the data the more the
reliance which can be placed on the utility of the resulting equation.
Extrapolation of such equations beyond the temperature range of experimental
measurements can lead to errors. In many of the systems it may be
assumed that approximate values of the mole fraction solubility, x1,
at a partial pressure of 101.3 kPa may be obtained by linear extrapolation
of values for lower partial pressures, p1, on the
assumption that x1/p1 is approximately
constant. However a similar linear extrapolation of solubilities at
pressures appreciably higher that 101.3 kPa to give mole fraction
solubilities at 101.3 kPa can lead to gross errors. For the purpose
of evaluation of data use has been made of the Krichevsky–Il'inskaya
equation to obtain approximate values of solubilities at 101.3 kPa
from measurements at higher pressures. These values were then compared
with measurements made at or near to 101.3 kPa.
©2002 American Institute of Physics.
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