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Henry's Law Constants

www.henrys-law.org

Rolf Sander

Atmospheric Chemistry Division

Max-Planck Institute for Chemistry
Mainz, Germany


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Henry's Law Constants

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When referring to the compilation of Henry's Law Constants, please cite this publication:

R. Sander: Compilation of Henry's law constants (version 4.0) for water as solvent, Atmos. Chem. Phys., 15, 4399-4981 (2015), doi:10.5194/acp-15-4399-2015


Henry's Law ConstantsInorganic speciesSulfur (S) → sulfur dioxide

FORMULA:SO2
CAS RN:7446-09-5
STRUCTURE
(FROM NIST):
InChIKey:RAHZWNYVWXNFOC-UHFFFAOYSA-N

Hscp d ln Hs cp / d (1/T) Reference Type Notes
[mol/(m3Pa)] [K]
1.3×10−2 2900 Sander et al. (2011) L
1.3×10−2 2900 Sander et al. (2006) L
1.2×10−2 3100 Yoo et al. (1986) L
1.2×10−2 3200 Maahs (1982) L
1.2×10−2 3000 Edwards et al. (1978) L
1.4×10−2 2800 Wilhelm et al. (1977) L
4.0×10−1 St-Pierre et al. (2014) M 75)
1.2×10−2 3100 Johnstone and Leppla (1934) M
1.1×10−2 1400 Terraglio and Manganelli (1967) V
1.2×10−2 3100 Chameides (1984) T
1.3×10−2 2900 Young (1983) X 5)
1.2×10−2 3100 Pandis and Seinfeld (1989) C
1.5×10−2 2900 Dean (1992) ? 6)
1.2×10−2 3100 Seinfeld (1986) ? 7)
1.2×10−2 3100 Hoffmann and Jacob (1984) ? 7)

References

  • Chameides, W. L.: The photochemistry of a remote marine stratiform cloud, J. Geophys. Res., 89D, 4739–4755, doi:10.1029/JD089ID03P04739 (1984).
  • Dean, J. A.: Lange’s Handbook of Chemistry, McGraw-Hill, Inc. (1992).
  • Edwards, T. J., Maurer, G., Newman, J., & Prausnitz, J. M.: Vapor-liquid equilibria in multicomponent aqueous solutions of volatile weak electrolytes, AIChE J., 24, 966–976, doi:10.1002/AIC.690240605 (1978).
  • Hoffmann, M. R. & Jacob, D. J.: Kinetics and mechanisms of the catalytic oxidation of dissolved sulfur dioxide in aqueous solution: An application to nighttime fog water chemistry, in: SO2, NO and NO2 Oxidation Mechanisms: Atmospheric Considerations, edited by Calvert, J. G., pp. 101–172, Butterworth Publishers, Boston, MA (1984).
  • Johnstone, H. F. & Leppla, P. W.: The solubility of sulfur-dioxide at low partial pressures, J. Am. Chem. Soc., 56, 2233–2238, doi:10.1021/JA01326A009 (1934).
  • Maahs, H. G.: Sulfur-dioxide/water equilibria between 0  and 50 C. An examination of data at low concentrations, in: Heterogeneous Atmospheric Chemistry, Geophysical Monograph 26, edited by Schryer, D. R., pp. 187–195, Am. Geophys. Union, Washington, D.C., doi:10.1029/GM026P0187 (1982).
  • Pandis, S. N. & Seinfeld, J. H.: Sensitivity analysis of a chemical mechanism for aqueous-phase atmospheric chemistry, J. Geophys. Res., 94D, 1105–1126, doi:10.1029/JD094ID01P01105 (1989).
  • Sander, S. P., Friedl, R. R., Golden, D. M., Kurylo, M. J., Moortgat, G. K., Keller-Rudek, H., Wine, P. H., Ravishankara, A. R., Kolb, C. E., Molina, M. J., Finlayson-Pitts, B. J., Huie, R. E., & Orkin, V. L.: Chemical Kinetics and Photochemical Data for Use in Atmospheric Studies, Evaluation Number 15, JPL Publication 06-2, Jet Propulsion Laboratory, Pasadena, CA, URL http://jpldataeval.jpl.nasa.gov (2006).
  • Sander, S. P., Abbatt, J., Barker, J. R., Burkholder, J. B., Friedl, R. R., Golden, D. M., Huie, R. E., Kolb, C. E., Kurylo, M. J., Moortgat, G. K., Orkin, V. L., & Wine, P. H.: Chemical Kinetics and Photochemical Data for Use in Atmospheric Studies, Evaluation No. 17, JPL Publication 10-6, Jet Propulsion Laboratory, Pasadena, URL http://jpldataeval.jpl.nasa.gov (2011).
  • Seinfeld, J. H.: Atmospheric Chemistry and Physics of Air Pollution, Wiley-Interscience Publication, NY (1986).
  • St-Pierre, J., Wetton, B., Zhai, Y., & Gea, J.: Liquid water scavenging of PEMFC contaminants, J. Electrochem. Soc., 161, E3357–E3364, doi:10.1149/2.0291409JES (2014).
  • Terraglio, F. P. & Manganelli, R. M.: The absorption of atmospheric sulfur dioxide by water solutions, J. Air Pollut. Control Assoc., 17, 403–406, doi:10.1080/00022470.1967.10468999 (1967).
  • Wilhelm, E., Battino, R., & Wilcock, R. J.: Low-pressure solubility of gases in liquid water, Chem. Rev., 77, 219–262, doi:10.1021/CR60306A003 (1977).
  • Yoo, K.-P., Lee, S. Y., & Lee, W. H.: Ionization and Henry’s law constants for volatile, weak electrolyte water pollutants, Korean J. Chem. Eng., 3, 67–72, doi:10.1007/BF02697525 (1986).
  • Young, C. L., ed.: IUPAC Solubility Data Series, vol. 12 of Sulfur Dioxide, Chlorine, Fluorine and Chlorine Oxides, Pergamon Press, Oxford, England (1983).

Type

Table entries are sorted according to reliability of the data, listing the most reliable type first: L) literature review, M) measured, V) VP/AS = vapor pressure/aqueous solubility, R) recalculation, T) thermodynamical calculation, X) original paper not available, C) citation, Q) QSPR, E) estimate, ?) unknown, W) wrong. See Section 3.1 of Sander (2015) for further details.

Notes

5) Value given here as quoted by Lide and Frederikse (1995).
6) Only the tabulated data between T = 273 K and T = 303 K from Dean (1992) were used to derive Hs and its temperature dependence. Above T = 303 K, the tabulated data could not be parameterized very well. The partial pressure of water vapor (needed to convert some Henry's law constants) was calculated using the formula given by Sander et al. (1995). The quantities A and α from Dean (1992) were assumed to be identical.
7) Several references are given in the list of Henry's law constants but not assigned to specific species.
75) Value at T = 353 K.

The numbers of the notes are the same as in Sander (2015). References cited in the notes can be found here.

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