Author's personal copy - University of Brighton Repository
Author's personal copy - University of Brighton Repository
Author's personal copy - University of Brighton Repository
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<strong>Author's</strong> <strong>personal</strong> <strong>copy</strong><br />
Phase transitions in the system MgO–CO 2–H 2O during<br />
CO 2 degassing <strong>of</strong> Mg-bearing solutions<br />
Laurence Hopkinson a,⇑ , Petra Kristova b,1 , Ken Rutt b,2 , Gordon Cressey c,3<br />
a School <strong>of</strong> Environment and Technology, <strong>University</strong> <strong>of</strong> <strong>Brighton</strong>, Cockcr<strong>of</strong>t Building, Lewes Road, <strong>Brighton</strong> BN2 4GJ, United Kingdom<br />
b School <strong>of</strong> Pharmacy and Biomolecular Sciences, <strong>University</strong> <strong>of</strong> <strong>Brighton</strong>, Cockcr<strong>of</strong>t Building, Lewes Road, <strong>Brighton</strong> BN2 4GJ, United Kingdom<br />
c Department <strong>of</strong> Mineralogy, Natural History Museum, Cromwell Road, London SW7 5BD, United Kingdom<br />
Abstract<br />
Received 5 January 2011; accepted in revised form 12 October 2011; available online 18 October 2011<br />
This study documents the paragenesis <strong>of</strong> magnesium carbonates formed during degassing <strong>of</strong> CO2 from a 0.15 M Mg 2+<br />
aqueous solution. The starting solutions were prepared by CO2 sparging <strong>of</strong> a brucite suspension at 25 °C for 19 h, followed<br />
by rapid heating to 58 °C. One experiment was performed in an agitated environment, promoted by sonication. In the second,<br />
CO2 degassing was exclusively thermally-driven (static environment). Electric conductance, pH, and temperature <strong>of</strong> the experimental<br />
solutions were measured, whereas Mg 2+ was determined by atomic absorption spectros<strong>copy</strong>. Precipitates were analysed<br />
by X-ray diffraction, Fourier transform (FT) mid-infrared, FT-Raman, and scanning electron micros<strong>copy</strong>.<br />
Hydromagnesite [Mg5(CO3)4(OH)2 4H2O] precipitated at 25 °C was followed by nesquehonite [Mg(HCO3,OH) 2H2O]<br />
upon heating to 58 °C. The yield <strong>of</strong> the latter mineral was greater in the agitated solution. After 120 min, accelerated CO2<br />
degassing resulted in the loss <strong>of</strong> nesquehonite at the expense <strong>of</strong> an assemblage consisting <strong>of</strong> an unnamed mineral phase:<br />
[Mg5(CO3)4(OH)2 8H2O] and hydromagnesite. After 240 min, dypingite [Mg5(CO3)4(OH)2 5H2O (or less H2O)] appears with<br />
hydromagnesite. The unnamed mineral shows greater disorder than dypingite, which in turn shows greater disorder than hydromagnesite.<br />
In the static environment, there is no evidence for nesquehonite loss or the generation <strong>of</strong> [Mg5(CO3)4(OH)2 X-<br />
H 2O] phases over the same timeframe. Hence, results indicate that the transformation <strong>of</strong> nesquehonite to hydromagnesite<br />
displays mixed diffusion and reaction-limited control and proceeds through the production <strong>of</strong> metastable intermediates,<br />
and is interpreted according to the Ostwald step rule. Nevertheless, variations in the chemistry <strong>of</strong> nesquehonite, combined<br />
with the established tendency <strong>of</strong> the mineral to desiccate, implies that its transformation to hydromagnesite is unlikely to follow<br />
a single simple sequential reaction pathway.<br />
Ó 2011 Elsevier Ltd. All rights reserved.<br />
1. INTRODUCTION<br />
Available online at www.sciencedirect.com<br />
Geochimica et Cosmochimica Acta 76 (2012) 1–13<br />
For several important groups <strong>of</strong> minerals, including<br />
carbonates, mineral paragenesis frequently results in<br />
⇑ Corresponding author. Tel.: +44 (0) 1273 642239; fax: +44 (0)<br />
1273 642285.<br />
E-mail addresses: l.hopkinson@brighton.ac.uk (L. Hopkinson),<br />
p.kristova@brighton.ac.uk (P. Kristova), k.rutt@brighton.ac.uk<br />
(K. Rutt), g.cressey@nhm.ac.uk (G. Cressey).<br />
1<br />
Tel.: +44 (0) 1273 642065; fax: +44 (0) 1273 642285.<br />
2<br />
Tel.: +44 (0) 1273 642076; fax: +44 (0) 1273 642285.<br />
3<br />
Tel.: +44 (0) 20 7942 5711; fax: +44 (0) 20 7942 5537.<br />
0016-7037/$ - see front matter Ó 2011 Elsevier Ltd. All rights reserved.<br />
doi:10.1016/j.gca.2011.10.023<br />
www.elsevier.com/locate/gca<br />
assemblages that do not conform to predictions based on<br />
equilibrium thermodynamics (e.g., Morse and Casey,<br />
1988). In the system MgO–CO2–H2O at 0–60 °C, the stable<br />
phases in equilibrium with aqueous solutions containing<br />
Mg ions and carbon dioxide are brucite [Mg(OH) 2] at very<br />
low partial pressures <strong>of</strong> CO2, and magnesite [MgCO3], the<br />
most stable magnesium carbonate under Earth surface conditions<br />
(e.g., Königsberger et al., 1999; Hänchen et al.,<br />
2008). Nevertheless, Mg-carbonate precipitation is strongly<br />
kinetically-controlled (e.g., Königsberger et al., 1999). Inhibition<br />
<strong>of</strong> magnesite formation has been ascribed to the high<br />
hydration energy <strong>of</strong> Mg 2+ (e.g., Hänchen et al., 2008).<br />
Instead <strong>of</strong> magnesite, a variety <strong>of</strong> magnesium hydrate and