Please use this identifier to cite or link to this item: https://apo.ansto.gov.au/dspace/handle/10238/1098
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dc.contributor.authorLowson, RTen_AU
dc.contributor.authorBrown, PLen_AU
dc.contributor.authorComarmond, MJen_AU
dc.contributor.authorRajaratnam, Gen_AU
dc.date.accessioned2008-04-22T05:21:23Zen_AU
dc.date.accessioned2010-04-30T05:02:31Z-
dc.date.available2008-04-22T05:21:23Zen_AU
dc.date.available2010-04-30T05:02:31Z-
dc.date.issued2007-03-15en_AU
dc.identifier.citationLowson, R. T., Brown, P. L., Comarmond, M. C. J., & Rajaratnam, G. (2007). The kinetics of chlorite dissolution. Geochimica Et Cosmochimica Acta, 71(6), 1431-1447. doi:10.1016/j.gca.2006.12.008en_AU
dc.identifier.govdoc1156-
dc.identifier.issn0016-7037en_AU
dc.identifier.urihttp://dx.doi.org/10.1016/j.gca.2006.12.008en_AU
dc.identifier.urihttp://apo.ansto.gov.au/dspace/handle/10238/1098en_AU
dc.description.abstractA model for the dissolution of chlorite has been developed based on fast ligand assisted proton attack of the alumina tetrahedra within the alumina-silica lattice followed by slower dissolution of the remnant silica lattice. While the rate determining step is within the silica dissolution regime, the rate is a function of the H+ and Al3+ concentrations and the dominant aqueous Al species. Individual rates may be described by a generic rate equation applicable across the spectrum of Al species: where rn is the rate subscripted for the nth Al species, k is the rate constant of the rate controlling step, K is the surface exchange constant, β is the solution stability constant subscripted for the Al species, a is the species activity subscripted for species and raised to the power of the stoichiometry, p and q are stoichiometric coefficients, z is the ligand charge and τ is the fractional coefficient for the precursor of the rate defining step. The observed rate is the sum of the individual rates. When the observed rate is in a domain of dominance for a single aluminium species and in the absence of strong complexing agents such as oxalate, the observed rate is proportional to (a3H+/aAl3+)τn. The model is supported by experimental data for the dissolution of chlorite over a pH range of 3–10 and temperature range 25–95°C. The results have hydrometallurgical application. © 2007, Elsevier Ltd.en_AU
dc.language.isoenen_AU
dc.publisherElsevieren_AU
dc.subjectKineticsen_AU
dc.subjectChlorite mineralsen_AU
dc.subjectDissolutionen_AU
dc.subjectLigandsen_AU
dc.subjectAluminatesen_AU
dc.subjectSilicaen_AU
dc.titleKinetics of chlorite dissolutionen_AU
dc.typeJournal Articleen_AU
dc.date.statistics2007-03en_AU
Appears in Collections:Journal Articles

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