The replacement of sulfate minerals by calcium carbonate polymorphs (carbonation) has important implications in various geological processes occurring in Earth surface environments. In this paper we report the results of an experimental study of the interaction between anhydrite (100), (010), and (001) surfaces and Na2CO3 aqueous solutions under ambient conditions. Carbonation progress was monitored by glancing incidence X-ray diffraction (GIXRD) and scanning electron microscopy (SEM). We show that the reaction progresses through the dissolution of anhydrite and the simultaneous growth of calcite. The growth of calcite occurs oriented on the three anhydrite cleavage surfaces and its formation is accompanied by minor vaterite. The progress of the carbonation always occurs from the outer-ward to the inner-ward surfaces and its rate depends on the anhydrite surface considered, with the (001) surface being much more reactive than the (010) and (100) surfaces. The thickness of the formed carbonate layer grows linearly with time. The original external shape of the anhydrite crystals and their surface details (e.g., cleavage steps) are preserved during the carbonation reaction. Textural characteristics of the transformed regions, such as the gradation in the size of calcite crystals, from ~2 μm in the outer region to ~17 μm at the calcite-anhydrite interface, the local preservation of calcite crystalographic orientation with respect to anhydrite and the distribution of the microporosity mainly within the carbonate layer without development of any significant gap at the calcite-anhydrite interface. Finally, we compare these results on anhydrite carbonation with those on gypsum carbonation and can explain the differences on the basis of four parameters: (1) the molar volume change involved in the replacement process in each case, (2) the lack/existence of epitactic growth between parent and product phases, (3) the kinetics of dissolution of the different surfaces, and (4) the chemical composition (amount of structural water) of the parent phases.
Mineral replacement reactions are common phenomena in a wide variety of environments and physicochemical conditions within the Earth. Such reactions often involve the dissolution of the parent phase as a result of its interaction with an aqueous fluid and the simultaneous precipitation of the product (Putnis 2002). The coupling between the kinetics of both processes, dissolution and crystallization, determines the preservation of the shape of the reactant to a scale that can reach the accurate reproduction of delicate details of its surface as well as its internal microstructure (Xia et al. 2009a). The scale of the pseudomorphism is indeed the result of how perfect this coupling is (Pöml et al. 2007; Fernández-Díaz et al. 2009).
The progress of mineral replacement reactions requires the continuous contact between the fluid phase and the interface between the primary and secondary phases where the reactions occur. Such contact is guaranteed when the mineral replacement involves the generation of significant microporosity (Putnis 2002). Such porosity is frequently a consequence of differences in solubility and molar volumes between the primary dissolving phase and the secondary precipitating phase. However, other factors such as the starting fluid composition and the solid-liquid volume ratio can also play an important role in the kinetics of mineral replacement reactions (Putnis 2002, 2009; Putnis et al. 2007; Ruiz-Agudo et al. 2014). When the reactant solid phase is more soluble and/or has a significantly higher molar volume than the product, the mineral replacement reaction can be accompanied by a volume reduction. This volume reduction is balanced by the generation of porosity, which allows the preservation of the original external shape (Pollok et al. 2011; Putnis 2009; Ruiz-Agudo et al. 2014, 2016). The specific contribution of the differences in solubility, molar volume, starting fluid composition, and solid-liquid volume ratio to porosity generation needs to be evaluated in each particular case.
Additionally, the existence of crystallographic relationships between the primary and secondary phases can promote the epitactic growth of the product on the surface of the reactant (Xia et al. 2009a, 2009b; Qian et al. 2011). This can lead to the partial armoring of the primary phase from the fluid and the subsequent stoppage of the replacement process (Prieto et al. 2003, 2013; Rodríguez-Blanco et al. 2007; Rodríguez et al. 2008; Pérez-Garrido et al. 2007) after a “partial equilibrium” end point is reached (Astilleros et al. 2006).
Gypsum (CaSO4·2H2O) and anhydrite (CaSO4) are the most common sulfate minerals in Earth's surface environments (Anthony et al. 2003). Both sulfate minerals can be replaced by other phases as a result of their interaction with fluids of variable compositions and this happens particularly often under Earth surface conditions (e.g., Freyer and Voigt 2003). Different studies have highlighted the relevance of replacement phenomena involving sulfate minerals in the context of a range of geological problems. For example, Hanor (2004) proposed the interaction of gypsum and/or anhydrite with fluids that bear Ba and Sr as a key process in the formation of large sedimentary deposits of celestine (SrSO4). Many other authors have reported that calcium sulfate minerals can be replaced by calcium carbonate polymorphs in sedimentary basins where a steady aqueous carbonate supply is warranted (Pierre and Rouchy 1988; Rouchy et al. 1998; Dejonghe et al. 1998; Sanz-Rubio et al. 2001; Azam 2007; Stafford et al. 2008). Nevertheless, the actual kinetics and mechanisms of the calcium sulfate to calcium carbonate replacement reactions are still poorly understood.
Although gypsum is thermodynamically the most stable calcium sulfate phase below ~60 °C, the solubility of anhydrite and gypsum are within the same order of magnitude (Ksp,gypsum = 10-4.58, Ksp,anhydrite = 10-4.36; Freyer and Voigt 2003). Both minerals have been reported to transform into CaCO3 when in contact with a carbonate-bearing aqueous solution (Flörke and Flörke 1961; Freyer and Voigt 2003). For both polymorphs this transformation involves dissolution-crystallization reactions and commonly results in the preservation of the external shape of the initial sulfate crystals (Freyer and Voigt 2003). Experiments following the interaction between acidic, SO42–-bearing solutions and calcite surfaces have shown that gypsum grows oriented on calcite cleavage surfaces (Booth et al. 1997; Offedu et al. 2014). Similarly, limestone sulfation experiments at around 700 °C confirmed that anhydrite also grows oriented on calcite (104) surfaces (Hu et al. 2008), suggesting in both cases the existence of crystallographic relationship between both structures. However, we have previously shown that the interaction between gypsum (010) surfaces and carbonate-bearing aqueous solutions at ambient Earth surface conditions proceed by an initial random nucleation of calcite on gypsum (010) surfaces, although as the reaction progresses, competitive growth between the randomly oriented calcite crystals results in an orientation selection that leads the formation of parallel, column-like calcite crystals elongated along  and perpendicularly arranged with respect to the original gypsum (010) surface (Barna and Adamik 1998; Fernández-Díaz et al. 2009). The possible existence or absence of epitactic relationships between calcite, the stable CaCO3 polymorph at Earth surface conditions, and calcium sulfate phases together with the similar solubility products at 25 °C for gypsum and anhydrite, make the carbonation of these phases an interesting case study for mineral replacement investigations. Moreover, the carbonation of calcium sulfate minerals has been recognized as responsible for the formation of large volumes of diagenetic carbonates in sedimentary rocks from the Precambrian to the Tertiary (Kendall 2001; Alonso-Zarza et al. 2002). Therefore, such reactions have likely played an important role in the evolution of sedimentary trapping of natural fluids (water and oil) since the generation of porosity increases the number of possible fluid pathways and the permeability of the host rocks. In addition to this, these reactions are important because recent studies have showed that CaSO4 phases can potentially be used as raw materials for sequestering CO2 by mineralization of carbonate phases (Pérez-Moreno et al. 2015; Azdarpour et al. 2015). Finally, understanding the factors that control the reaction pathways involved in the carbonation of calcium sulfate minerals can shed light on the mechanism that leads to the development of specific textures in a range of mineral replacement processes (Ruiz-Agudo et al. 2015, 2016).
To fill this gap in our knowledge, we report here on the results of an experimental study of the kinetics and mechanism of anhydrite carbonation under conditions that are relevant for industrial processes and can be extrapolated to those commonly found in natural environments. We compare our observations on anhydrite to results previously obtained on gypsum carbonation. Our goal was to evaluate to what extent (1) differences in the molar volume change involved in the replacement and (2) the lack/existence of epitactic growth between primary and secondary phases influences carbonation reaction pathways. We will show how the combination of both factors determines the development of specific textural features and affects the progress of the replacement reaction.
Experiments were carried out by putting freshly cleaved anhydrite fragments in glass vessels containing 1 mL of a commercial 0.5 M Na2CO3 aqueous solution (pH ≈ 11.4; Fluka). The vessels were immediately closed with a polypropylene cap to avoid exchange with CO2 in the atmosphere and evaporation. All experiments were performed using natural slightly blue, highly pure anhydrite crystals from Naica, Chihuahua (Mexico). Prior to the experiments, the crystals were cleaved parallel to (100), (010), and (001) faces with a knife edge to obtain fragments of approximately 2 × 2 × 1.5 mm. Anhydrite fragments were bounded by surfaces parallel to the main cleavage planes (100), (010), and (001), all of which are F-faces (Aquilano et al. 1992; Redfern and Parker 1998) and, therefore, very stable surfaces. Moreover, (100) together with the (010) are the most common surfaces in natural anhydrite crystals (Aquilano et al. 1992). All the experiments were run in triplicate at 25 ± 0.5 °C and atmospheric pressure. The samples were recovered from the solutions after times that ranged between 1 min and 1 month, followed by rapid drying using absorbent paper, and subsequently placing the resulting solids into a desiccator at room temperature prior to further analyses.
Samples were analyzed using glancing incident X-ray diffraction (GIXRD) analyses with a PANalytical X'Pert PRO MRD diffractometer equipped with a CuKα X-ray source, an X-ray parabolic mirror in the incident beam and a parallel plate collimator with flat graphite monochromator in the diffracted beam (Xe proportional detector). Scans were recorded between 2 and 80 °Θ at 2 °/s scan rate and a step size of 0.05°. The angle of incidence was 1°, which allowed obtaining information corresponding to the shallow layers, minimizing the presence of peaks coming from the bulk of the anhydrite crystal. Diffraction patterns were compared to standard powder diffraction files from the ICDD-PDF2 database (release 2007): 00-037-1496 for anhydrite, 01-071-3699 for calcite, and 00-024-0030 for vaterite. A semi-quantitative estimate of the percentage of the different crystalline phases forming on the outer part of the carbonated layer was performed using the reference intensity ratio (RIR) method (Snyder 1992). Reacted samples were placed on an aluminum stub covered by a sticky carbon pad or mounted on glass slide and embed in a synthetic epoxy resin and polished using diamond laps to investigate the contact between the anhydrite and the replaced layer. Then samples were imaged using a JEOL JSM6400 Scanning Electron Microscope (SEM) (20 kV; working distance of 15 nm) equipped with a LINK Ex1 energy dispersive spectrometer. Both GIXRD analyses and SEM observations were conducted on specific anhydrite surfaces after set interaction times. In those cases the orientation of the anhydrite surface of interest was established prior to the experiments by observing the interference figures in a polarized light microscope. The progress of the replacement and its thickness were determined by measuring the width of the transformed layer on SEM images of sections of post-reaction samples using the Image J software (Rasband 2016).
Reaction pathways in anhydrite carbonation
The carbonation reaction begins on anhydrite surfaces immediately after the crystals are immersed into the 0.5 M Na2CO3 aqueous solution. GXRD data (Fig. 1) confirm calcite as the main component forming on the outer layer of the reacted anhydrite samples from the very early stages of the carbonation process. This was irrespective the anhydrite surface considered. This reaction seems to progress via the dissolution of anhydrite and the simultaneous formation of calcite crystals. Evidences of both processes can be clearly detected on the images of anhydrite surfaces that even after 1 min are covered by small calcite crystals (Fig. 2a).
Although at the very beginning calcite nuclei are small and scarce (Fig. 2a), their density and sizes rapidly increase on all considered anhydrite surfaces during the first 30 min of interaction (Fig. 2b). The newly formed calcite crystals were not randomly distributed on the anhydrite surface but they were spatially related to etch pits or step edges (Fig. 2b) and their size increases with increasing interaction time: after 1 min the size of calcite crystals varied between ~0.2–0.5 μm and it reached ~12 μm after 1 week (Fig. 2d). The progress of the interaction leads to a complete coverage of the anhydrite surface after a few hours (~5 h) (Fig. 2c). Calcite crystals show the typical rhombohedral habit, with flat (104) faces and sharp edges and no modification in the general characteristics of the rhombohedral habit of calcite were observed.
Significant differences in the extent of coverage by CaCO3 phases and the pathway of carbonation were detected at the early stages of the reaction on different anhydrite surfaces. For example, after 1 h of reaction, the coverage was almost complete on the anhydrite (001) surface (Fig. 3a), while on the (100) surface it reached ~33% (Fig. 3b) and on the (010) surface ~47% only (Fig. 3c). In addition, both calcite and vaterite were present on the anhydrite surfaces. However, the amount of vaterite observed coexisting with calcite at the early stages of reaction also varies depending on the anhydrite surface considered. Numerous vaterite aggregates could be distinguished on anhydrite (010) and (001) surfaces, while these were scarce on the (100) surface (Figs. 3d, 3e, and 3f). GXRD patterns collected on reacted samples 2 h after the beginning of experiments evidence that irrespective the anhydrite surface studied calcite was the most abundant CaCO3 polymorph. Weak reflections that could be assigned to vaterite were distinguishable in the GXRD pattern collected from (001) anhydrite surfaces (Fig. 4a). These reflections are extremely weak in the GXRD pattern collected on the (010) surface and absent on the patterns obtained from the (100) anhydrite surface (Figs. 4b and 4c). These results were also confirmed by the scarcity observed of vaterite aggregates in SEM images of each surface (Figs. 3a and 3d). Semi-quatitative estimates derived from GXDR patterns using the Reference Intensity Ratio (RIR) method (Snyder 1992) yielded vaterite percentages in the carbonate layer after 2 h reaction below 1% on the (010) and ~1.5% on the (001) surface, respectively. After 15 h of reaction the GXRD patterns revealed the presence of only reflections that could be assigned to calcite and this was irrespective the anhydrite cleavage surface considered (e.g., Fig. 1c).
Textural characteristics of calcite pseudomorphs after anhydrite
SEM photomicrographs reveal that calcite crystals appear to share a mutual orientation with the initial anhydrite, suggesting epitactic growth on each anhydrite surface (Fig. 2). We focus from hereon on the observations on the anhydrite (100) surface. Similar features are also observed on (010) and (001). On (100) this epitactic relationship becomes apparent after 1 min of interaction (Fig. 2a) and, at least locally, remains well defined after prolonged interaction times (7 days; Fig. 2d).
The original external shape of the anhydrite crystals as well as fine details of their surfaces including their cleavage steps are preserved during the carbonation reaction (Fig. 5a). Calcite pseudomorphs after anhydrite are bounded by well-defined faces and sharp edges (Fig. 5a). The backscatter electron (BSE) micro-graph in Figure 5b shows a section of an anhydrite crystal partially transformed into CaCO3 after 3 days of reaction. Differences in contrast between the CaSO4 and CaCO3 phase evidence the extent of the transformation. It is apparent that the carbonation reaction progresses from outward to inward of the anhydrite crystal and a well-defined reaction front developed. Eventually, the reaction progresses and finishes with the formation of pseudomorphs exclusively consisting of calcite (Fig. 5a). The replaced layer consists of calcite crystals, which at least locally were oriented with respect to the original anhydrite surface (Figs. 5c and 5d). A gradual increase in the size of the formed calcite crystals is also apparent, with those closer to the interface with the retreating anhydrite surface being significantly larger (mean size 17 ± 2.5 μm) than those on the outer rim (mean size 2.2 ± 0.8 μm). The contact between the replaced layer and the retreating anhydrite surface is sharp and no significant gap was observed at the interface. The replaced layer armoring the original anhydrite shows a homogeneous aspect, yet the carbonate layer also shows an evenly distributed porosity consisting of small pores located at the contact between slightly misoriented calcite crystals or between calcite crystals that show different orientations with respect to anhydrite (Fig. 5d).
Reaction kinetics of anhydrite carbonation
The change in the width of the transformed region over time as obtained from evaluating SEM images is show in Figure 6. The thickness of the carbonate layer increase linearly with time, indicating no change in the transformation rate as the thickness of the carbonate layer (coating the anhydrite core) increases. It takes approximately 14 days for the whole replacement of an anhydrite single crystal to occur (crystal volume ≈ 6 mm3).
The interaction between carbonate-bearing solution with anhydrite leads to the generation of pseudomorphs consisting of aggregates of calcite crystals. This interaction shows the typical characteristics of a mineral replacement process (Putnis 2002; Putnis and Putnis 2007). Our data reveal that the reaction progresses via the dissolution of the primary phase (anhydrite) and the growth of CaCO3 at the anhydrite-solution interface. The reaction involves the formation of a sharp, inward moving, reaction front separating the primary and secondary phases. Although anhydrite carbonation shares major characteristics with gypsum carbonation (Fernández-Díaz et al. 2009), it also shows specific differences regarding (1) the reaction pathways, (2) the textural characteristics of the calcite crystal aggregates forming the pseudomorphs after the specific calcium sulfate mineral, and (3) the reaction kinetics. The factors responsible for these differences between anhydrite and gypsum carbonation are discussed below.
Reaction pathways in anhydrite carbonation vs. gypsum carbonation
The interaction between anhydrite (100) surface and a 0.5 M Na2CO3 aqueous solution involves the formation of the CaCO3 polymorph calcite since the very early stages of the reaction, with vaterite appearing only as a very minor phase that readily transforms into calcite after a few hours. The vaterite to calcite transformation is well known to proceed via dissolution and re-precipitation specially in the presence of sulfate (Fernández-Díaz et al. 2010; Rodriguez-Blanco et al. 2011; Bots et al. 2012). This relatively simple reaction pathway contrast with the more complex sequence of dissolution-crystallization reactions observed during the carbonation of gypsum under identical experimental conditions (Fernández-Díaz et al. 2009). In the case of gypsum carbonation the reaction started with the formation of a thin layer of amorphous calcium carbonate (ACC) within the first minutes of the replacement process. This early ACC layer readily transformed to a mixture of vaterite and calcite. Furthermore, both crystalline carbonate polymorphs were still present after the carbonation reaction had finished, although the proportion of vaterite continued to decrease as a result of its solvent mediated transformation into calcite and after 72 h of reaction only calcite was detected.
Two main factors can explain the different reaction pathways observed in the carbonation of both calcium sulfate phases. The first factor and, probably, the most important one is the existence or absence of epitactic relationships between the calcite over-growth and the calcium sulfate substrate. Whereas the overgrowth clearly is epitactic on anhydrite (100) surface (Figs. 2 and 3), no evident epitactic relationship were observed when calcite crystals initially form on gypsum (010) surfaces (Fernandez-Diaz et al. 2009). Indeed, during the carbonation of gypsum calcite crystals first nucleate randomly oriented within the thin ACC layer that carpeted the initial gypsum (010) surface after the first minutes of reaction. Only later did the calcite crystals become oriented with their c axis perpendicular to the retreating (010) gypsum surface as their growth progressed. The formation of metastable phases like ACC and vaterite at the early stages of the interaction in the case of gypsum carbonation was the consequence of the predominance of kinetic factors over thermodynamics. This predominance is associated with the energy barrier that needs to be overcome for the heterogeneous nucleation of calcite on the surface of a calcium sulfate mineral to occur. This energy barrier significantly decreases when heterogeneous nucleation has an epitactic character, as it is the case for calcite forming on anhydrite (100) surface (Chernov 1984). The difference in complexity of the reaction pathways operating during the interaction between a carbonate-bearing aqueous solution and anhydrite or gypsum highlights the importance of crystallographic relationships in defining mineralogical evolutions during mineral replacement processes. A significant influence of crystallographic relationships in the development of mineral replacement processes has been found in several systems. For example, Xia et al. (2009a) showed that the similarity of the crystal structures of pentlandite, (Fe,Ni)9S8, and violarite, (NiFe)3S4, which facilitates the epitactic nucleation, promotes the replacement of petlandite by violarite under conditions at which other sulfides ([e.g., vaesite (NiS2) and polydymite (Ni3S4)] are thermodynamically more stable than violarite. Similarly, Qian et al. (2011) concluded that the replacement of pyrrhotite by marcasite instead of pyrite under low-temperature hydrothermal conditions is facilitated by the higher crystallographic similarity between the S lattices in pyrrhotite and marcasite structures.
The second factor that might influence the different reaction pathways observed during the carbonation reaction is the differences in dissolution kinetics of gypsum vs. anhydrite. Bulk experiments revealed that anhydrite dissolves around two orders of magnitude slower than gypsum (Jeschke et al. 2001; Jeschke and Draybrodt 2002). Similarly, macroscopic dissolution measurements conducted on anhydrite (010) and gypsum (010) surfaces yielded dissolution rate constants (k) of 2.6 and 46 ± 6 μmol m-2s-1, respectively (Pachon-Rodriguez and Colombani 2013). Based on atomic force microscopic (AFM) studies much faster dissolution kinetics for gypsum than for anhydrite were also confirmed (Bosbach et al. 1995; Shindo et al. 1996). Consequently, supersaturation of the aqueous solution at the interface with respect to CaCO3 phases increases much more rapidly during interaction with gypsum (010) surfaces than with anhydrite (100) surfaces, thereby explaining the formation of metastable ACC as well as higher amounts of vaterite during the early stages of the carbonation of gypsum compared to the total lack of ACC and only minor vaterite for anhydrite carbonation.
The influence of the different dissolution kinetics for each face could also explain the slightly different mineralogical pathways observed on anhydrite (010) and (001) surfaces in comparison to observed on anhydrite (100) surface. While only calcite is detected on (100) anhydrite surface by GXRD at any reaction step, SEM observations evidence the formation of small amounts of vaterite together to calcite at early stages of the interaction on both (010) and (001) surfaces, being these amounts larger in the later. AFM studies by Shindo et al. (2010) showed that anhydrite (001) dissolves at much faster rate than (100) and (010), which are similarly reactive. This means that Ca2+ ions are released to the solution at a faster rate from (001), leading to larger departures from equilibrium in the layer of aqueous solution close to this surface. This can explain both the formation of higher percentages of vaterite and its preservation during longer times as a main component of the carbonate layer on (001) anhydrite cleavage surfaces.
Textural characteristics of calcite pseudomorphs after anhydrite vs. calcite pseudomorphs after gypsum
Calcite pseudomorphs after gypsum are characterized by a thin, fine-grained rim (15–20 μm) of randomly oriented calcite crystals and a core of parallel columns of calcite crystals in a stockade-like arrangement (Fernández-Díaz et al. 2009). This textural feature is the consequence of an initial nucleation of randomly oriented calcite crystals on gypsum (010). Due to the faster calcite growth along the  direction, differently oriented crystals compete for space as they grow. Only those calcite crystals whose c-axis is perpendicular to the original gypsum surface are able to grow without interfering with other crystals. As a result, the progress of the replacement leads to the development of parallel column-like calcite crystals elongated along , which grow perpendicular to the retreating gypsum surface.
Stockade-like textures are absent in calcite pseudomorphs after anhydrite. As explained above, calcite nucleation on anhydrite cleavage surfaces is epitactic. In all the cases, the first calcite crystals to form have one of their (104) surfaces laying on the corresponding anhydrite cleavage surface. As all these calcite crystals are equally oriented on anhydrite surface, competitive growth between them does not occur. On the contrary, the existence of epitactic relationships promotes their growth parallel to the anhydrite surface (Sunagawa 1987), which leads to their coalescence and the formation of a compact calcite layer that shields the anhydrite.
Further textural differences between gypsum and anhydrite result from the very different change in molar volume involved in the carbonation of these two calcium sulfate phases. Both gypsum and anhydrite have larger molar volumes than calcite. This means that in both cases carbonation is accompanied by a negative volume change. Consequently for a pseudomorphic process this volume change needs to be balanced by the generation of porosity. This is indeed the case in the replacement of anhydrite by calcite, which involves a volume change of ~ –9.2 cm3/mol; ~20% (Smyth and McCormick 1995). The porosity generated to compensate this volume change is confined within the transformed layer and shows a basically homogeneous distribution during the early stages of the carbonation process. The difference between the molar volumes of gypsum and calcite is significantly larger (~ –37.6 cm3/mol; >50%) (Smyth and McCormick 1995), which determines that the volume change associated to the carbonation reaction can only be partially compensated by the generation of porosity. Part of this volume change is compensated by the formation of a gap between the replaced layer and the retreating surface of gypsum. The size of this gap increases as the transformation advances. The formation of similar gaps at the interface between primary and secondary phases has been observed during replacement processes, which either involve large volume changes, i.e., replacement of pyrochlore as a result of hydrothermal alteration (Pöml et al. 2007), or are kinetically limited by the precipitation of the secondary phase, i.e., pentlandite, (Fe,Ni)9S8, by violarite (NiFe)3S4 (Xia et al. 2009b). The development of such a gap during the carbonation of gypsum determines the loss of adhesion between the retreating gypsum surface and the replaced layer and eventually leads to the formation of a hollow core within calcite pseudomorphs after gypsum. This, together to the larger amount of porosity formed, confers these pseudomorphs with a much more fragile nature than calcite pseudomorphs formed after anhydrite. In nature the transformation of anhydrite to calcite generates reduction of volume that may cause the development of porosity or deformation in the sediment layers. For example: the nodules of sulfur of the Messinian of Cyprus (Rouchy et al. 1994), and the sulfate evaporates in the Middle Miocene (Pierre and Rouchy 1988) in the Gulf of Suez are associated with abnormally deformed secondary carbonates formation associated to sulfate evaporates in the Middle Miocene (Pierre and Rouchy 1988).
Reaction kinetics of anhydrite carbonation vs. gypsum carbonation
The carbonation of anhydrite occurs at much lower rate than the carbonation of gypsum. For example, a gypsum single crystal with volume ≈ 6 mm3 is completely replaced by CaCO3 after being in contact with a 0.5 M Na2CO3 aqueous solution during 1 day (Fernández-Díaz et al. 2009). In contrast, the whole replacement of an anhydrite single crystal of similar volume takes approximately 14 days. This much slower kinetics of anhydrite carbonation is a consequence of two factors. The first factor is the different dissolution kinetics of gypsum and anhydrite. Since the solution layer closer to the calcium sulfate mineral surface becomes rapidly supersaturated with respect to any CaCO3 polymorphs, CaCO3 precipitation occurs immediately. Therefore, dissolution of the calcium sulfate mineral is the rate determining step of the carbonation process. Consequently, the much slower dissolution of anhydrite in comparison to gypsum can explain the much slower anhydrite carbonation. The second factor that can contribute to make anhydrite carbonation a slower process is the significantly smaller volume of porosity that is generated during the former reaction. For the carbonation process to proceed, a permanent communication between the interface where the reaction occurs and the bulk solution is required. This communication through the formed porosity guarantees continuous supply of CO32– ions toward the calcium sulfate surface and those can react with the Ca2+ released to the fluid as a result of mineral dissolution. A calcium carbonate layer with a significantly smaller amount of porosity will decrease the diffusion of CO32– toward the surface of the calcium sulfate due to partial armoring of the primary phase, anhydrite in this case. This leads then to a slower carbonation process.
It is interesting that, although anhydrite carbonation occurs at a much slower rate than that of gypsum, its rate remains constant until the process is complete and anhydrite single crystals are fully transformed into aggregates of small calcite crystals. On the contrary, gypsum carbonation rate is very high during the early stages of the process but it significantly slows down at later stages. Fernández-Díaz et al. 2009 explained this change in the gypsum carbonation kinetics as due to three main causes: (1) the formation of a thick layer coating the gypsum surface that prevent percolation of the fluid to the interface, (2) the depletion of CO32– in the aqueous solution due to the formation of CaCO3 phases, and (3) the progressive increase of the SO42–/CO32– ratio in the aqueous solution at the interface. However, this explanation is not in good agreement with the observation that anhydrite carbonation rate remains constant during the whole process. Indeed, the formation of a thick layer of CaCO3, which is significantly less porous than that formed during the carbonation of gypsum, should lead to a clearer slow down of the reaction in the case of anhydrite. The chemical composition of the sulfate phases can also play a decisive role. During gypsum dissolution two molecules of water for each Ca2+ and SO42– ions are being released to the aqueous solution confined into the gap developed between the replaced layer and the retreating surface of gypsum. This has a dilution effect that leads to a reduction of the supersaturation with respect to any CaCO3 phase at interface. As a result, the carbonation reaction will temporally slow down or even stop until a high enough amount of CO32– ions diffuse to the aqueous solution filling the gap between the carbonate layer and the gypsum surface. Since the communication between the carbonate-bearing bulk fluid and the gypsum surfaces becomes progressively more difficult as the carbonate layer becomes thicker, the slow down of the carbonation reaction becomes apparent as the process progresses. In contrast, the dissolution of anhydrite is not accompanied by any dilution effect, which can, at least partially, explain that anhydrite carbonation proceeds at approximately constant rate, even though the volume of porosity generated during anhydrite carbonation is much smaller than during gypsum carbonation. Qualifying the influence of factors like the textural characteristics of the porosity distribution on the kinetics of the pseudomorphic carbonation of calcium sulfate phases will be the object of further investigation.
Implications for calcium sufate carbonation processes
The experimental results show that the carbonation of anhydrite involves the early nucleation of epitactic calcite on the three main anhydrite cleavage surfaces. Calcite can be accompanied by small amounts of vaterite at early stages of the carbonation processes in two of these surfaces, defining two different surface-related reaction pathways: anhydrite → calcite and anhydrite → calcite + vaterite → calcite. We interpret these reaction pathways as reflecting the differences in supersaturation with respect to CaCO3 phases at the fluid-anhydrite interface that result from the different dissolution rate of anhydrite cleavage surfaces. We interpret these pathways during anhydrite carbonation as resulting from two factors: (1) The two orders of magnitude slower dissolution kinetics of anhydrite in comparison to gypsum, which determines a much slower supersaturation rate for CaCO3 phases at the fluid-anhydrite interface. (2) The existence of epitatic relationships between calcite and all three main anhydrite cleavage surfaces. Anhydrite carbonation reaction involves a negative volume change, which is compensated by the generation of microporosity. For the reaction times considered in this work, this microporosity is homogeneously distributed within the carbonate layer and a sharp contact exists between the carbonate layer and the anhydrite core. This porosity provides a continuous communication between the carbonate-bearing fluid and the calcite-anhydrite interface, thereby guaranteeing the progress of anhydrite carbonation at a constant rate. Anhydrite carbonation progresses at a much slower rate than the carbonation of gypsum. The different carbonation kinetics of these two calcium sulfate phases can be explain as arising from (1) the slower dissolution kinetics of anhydrite compared to gypsum and (2) the much higher volume change and, thus, microporosity generated in gypsum carbonation.
This study was supported by the MINECO (Spain) under projects CGL2013-47988-C2-1-P and CGL2016-77138-C2-1-P, the Marie Curie EU-FP6 Mineral Nucleation and Growth Kinetics (MIN-GRO) Research and Training Network under contract MRTNCT-2006-035488, and by the UK Engineering and Physical Research Council through grant number EP/P015514/1.