Analysis of Rates of Geochemical Reactions

  • Susan L. Brantley
  • Christine F. Conrad

Over the last several billion years, rocks formed at equilibrium within the mantle of the Earth have been exposed at the surface and have reacted to move towards a new equilibrium with the atmosphere and hydrosphere. At the same time that minerals, liquids, and gases react abiotically and progress toward chemical equilibrium at the Earth’s surface, biological processes harvest solar energy and use it to store electrons in reservoirs which are vastly out of equilibrium with the Earth’s other surface reservoirs. In addition to these processes, over the last several thousand years, humans have produced and disseminated non-equilibrated chemical phases into the Earth’s pedosphere, hydrosphere, and atmosphere. To safeguard these mineral and fluid reservoirs so that they may continue to nurture ecosystems, we must understand the rates of chemical reactions as driven by tectonic, climatic, and anthropogenic forcings.


Batch Reactor Elementary Reaction Continuously Stir Tank Reactor Geochemical Reaction Initial Rate Method 
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  1. Bandstra J. Z. and Tratnyek P. G. (2005) Central limit theorem for chemical kinetics in complex systems. J. Math. Chem. 37(4), 409-422.CrossRefGoogle Scholar
  2. Brantley S. L. and Mellott N. (2000) Specific surface area and porosity of primary silicate minerals. Am. Mineral. 85, 1767-1783.Google Scholar
  3. Capellos C. and Bielski B. H. J. (1972) Kinetic Systems. Wiley-Interscience.Google Scholar
  4. Chen Y. and Brantley S. L. (1997) Temperature-and pH-dependence of albite dissolution rate at acid pH. Chem. Geol. 135, 275-292.CrossRefGoogle Scholar
  5. Chou L. and Wollast R. (1985) Steady-state kinetics and dissolution mechanisms of albite. Am. J. Sci. 285, 963-993.Google Scholar
  6. Conrad C. F., Icopini G. A., Yasahura H., Brantley S. L. and Heaney P. J. (2007) Modeling the Kinetics of Silica Nanocolloid Formation and Precipitation in Geo-logically Relevant Aqueous Solutions. Geochimica et Cosmochimica Acta 71(3), 531-542.CrossRefGoogle Scholar
  7. Drever J. I. (1997) The Geochemistry of Natural Waters: Surface and Groundwater Environments. Prentice Hall, Englewood Cliffs, NJ.Google Scholar
  8. Driehaus W., Seith R., and Jekel M. (1995) Oxidation of arsenate(III) with manganese oxides in water treatment. Wat. Res. 29(1), 297-305.CrossRefGoogle Scholar
  9. Hamilton J. P., Brantley S. L., Pantano C. G., Criscenti L. J., and Kubicki J. D. (2001) Dissolution of nepheline, jadeite and albite glasses: Toward better models for aluminosilicate dissolution. Geochim. Cosmochim. Acta 65(21), 3683-3702.CrossRefGoogle Scholar
  10. Hem J. D., Roberson C. E., Lind C. J., and Polzer W. L. (1973) Chemical interactions of aluminum with aqueous silica at 25C, pp. 57. US Geological Survey.Google Scholar
  11. Hill C. G. (1977) An Introduction to Chemical Engineering Kinetics and Reactor Design. John Wiley & Sons, Inc., New York.Google Scholar
  12. Hossner L. R. and Doolittle J. J. (2003) Iron sulfide oxidation as influenced by calcium carbonate application. J. Environ. Qual. 32, 773-780.CrossRefGoogle Scholar
  13. Icopini G. A., Brantley S. L., and Heaney P. J. (2005) Kinetics of silica oligomerization and nanocolloid formation as a function of pH and ionic strength at 25 C. Geochim. Cosmochim. Acta 69(2), 293-303.CrossRefGoogle Scholar
  14. Kalinowski B. E. and Schweda P. (1996) Kinetics of muscovite, phlogopite, and biotite dissolution and alteration at pH 1-4, room temperature. Geochim. Cosmochim. Acta 60, 367-385.CrossRefGoogle Scholar
  15. Kraemer S. M. (2004) Iron oxide dissolution and solubility in the presence of siderophores. Aquat. Sci. 66, 3-18.CrossRefGoogle Scholar
  16. Laidler K. J. (1987) Chemical Kinetics. Harper & Row, Publishers, Inc., New York.Google Scholar
  17. Laidler K. J. and Meiser J. H. (1995) Physical Chemistry. Houghton Mifflin Company, Boston, MA.Google Scholar
  18. Lasaga A. C. (1981) Rate laws of chemical reactions. In Kinetics of Geochemical Processes, Vol. 8 (ed. A. C. Lasaga and R. J. Kirkpatrick), pp. 1-68. Mineralogical Society of America.Google Scholar
  19. Nagy K. L. (1995) Dissolution and precipitation kinetics of sheet silicates. In Chemical Weathering Rates of Silicate Minerals, Vol. 31 (ed. A. F. White and S. L. Brantley), pp. 173-225. Mineralogical Society of America.Google Scholar
  20. Oelkers E. H., Schott J., and Devidal J.-L. (2001) On the interpretation of closed system mineral dissolution experiments: Comment on “mechanism of kaolinite dissolution at room temperature and pressure part II: Kinetic study” by Huertas et al. (1999). Geochim. Cosmochim. Acta 65(23), 4429-4432.CrossRefGoogle Scholar
  21. Perez J. R., Banwart S. A., and Puigdomenech I. (2005) The kinetics of O2(aq) reduction by structural ferrous iron in naturally occurring ferrous silicate minerals. App. Geochem. 20, 2003-2016.CrossRefGoogle Scholar
  22. Posey-Dowty J., Crerar D., Hellmann R., and Chang C. D. (1986) Kinetics of mineral-water reactions; theory, design and application of circulating hydrothermal equipment. Am. Mineralog. 71, 85-94.Google Scholar
  23. Prigogine I. (1967) Introduction to Thermodynamics of Irreversible Processes. John Wiley & Sons, Inc., New York.Google Scholar
  24. Rimstidt J. D. and Newcomb W. D. (1993) Measurement and analysis of rate data: The rate of reaction of ferric iron with pyrite. Geochim. Cosmochim. Acta 57, 1919-1934.CrossRefGoogle Scholar
  25. Rimstidt J. D. and Dove P. M. (1986) Mineral solution reaction rates in a mixed flow reactor: Wollastonite hydrolysis. Geochim. Cosmochim. Acta 50(11), 2509-2516.CrossRefGoogle Scholar
  26. Rodgers W. B. and Rodgers R. E. (1848) On the decomposition and partial solution of minerals and rocks by pure water and water charged with carbonic acid. Am. J. Sci. 5, 401-405.Google Scholar
  27. Shiraki R. and Brantley S. L. (1995) Kinetics of near-equilibrium calcite precipitation at 100 C: An evaluation of elementary reaction-based and affinity-based rate laws. Geochim. Cosmochim. Acta 59(8), 1457-1471.CrossRefGoogle Scholar
  28. Skinner G. B. (1974) Introduction to Chemical Kinetics. Academic Press.Google Scholar
  29. Taylor A. S., Blum J. D., and Lasaga A. C. (2000) The dependence of labradorite dissolution and Sr isotope release rates on solution saturation state. Geochim. Cosmochim. Acta 64(14), 2389-2400.CrossRefGoogle Scholar
  30. Van Straten H. A., Schoonen M. A. A., and De Bruyn P. L. (1985) Precipitation from supersaturated aluminate solutions III. Influence of alkali ions with special reference to Li+ . J. Colloid Interface Sci. 103, 493-507.CrossRefGoogle Scholar
  31. White A. F. and Brantley S. L. (2003) The effect of time on the experimental and natural weathering rates of silicate minerals. Chem. Geol. 202, 479-506.CrossRefGoogle Scholar
  32. Williamson M. A. and Rimstidt J. D. (1994) The kinetics and electrochemical rate-determining step of aqueous pyrite oxidation. Geochim. Cosmochim. Acta 58(24), 5443-5454.CrossRefGoogle Scholar

Copyright information

© Springer Science+Business Media, LLC 2008

Authors and Affiliations

  • Susan L. Brantley
    • 1
  • Christine F. Conrad
    • 1
  1. 1.Center for Environmental Kinetics Analysis, Earth and Environmental Systems InstituteThe Pennsylvania State UniversityUSA

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