Research Article  Open Access
Dedolomitization Potential of Fluids from GypsumtoAnhydrite Conversion: Mass Balance Constraints from the Late Permian Zechstein2Carbonates in NW Germany
Abstract
The Zechstein2Carbonates represent one of the most prolific hydrocarbon systems of Central Europe. Carbonate reservoir quality is primarily controlled by mineralogy, with dolomite representing moderatetogood porosities and calcite commonly representing low porosities. Current models suggest that this calcite is the result of a basinwide phase of dedolomitization. The calcium (Ca) source for the dedolomites is thought to be derived from the fluids liberated during gypsumtoanhydrite conversion. We present an easytouse and generally applicable template to estimate the dedolomitization potential of these fluids. Depending on reaction stoichiometry, salinity, and temperature, we estimate that between 0^{−3 }m^{3} and 0^{−3 }m^{3} of calcite may replace dolomite for each m^{3} of anhydrite created. Within the constraints dictated by the environment of the late Permian Zechstein basin, we estimate that about 0^{−3 }m^{3} of dedolomite is created for each m^{3} of anhydrite. Mass balance constraints indicate that fluids derived from gypsumtoanhydrite conversion account for less than 1% of the observed dedolomite in most of the studied industry wells from northern Germany.
1. Introduction
The Zechstein2Carbonate (Ca2) of the Southern Permian Basin represents one of the major gas plays in northern Germany. Reservoir quality is mainly controlled by mineralogy. Where the mineralogy is dominated by dolomite, reservoir quality is predicted to be moderate to good and poor where the mineralogy is mainly calcitic [1–3]. Early studies suggested that the vast majority of this calcite is not of primary origin but rather formed due to dedolomitization [4, 5].
Dedolomitization or dolomite calcitisation describes the replacement process of dolomite by calcite [6]. The general reaction for dedolomitization can be written as follows:Dolomite dissolves and calcite precipitates. This process consumes calcium and liberates magnesium [7]. Several conditions have to be met for dedolomitization to take place. A low Mg^{2+} to Ca^{2+} ratio of the pore fluid is necessary, so that dolomite is undersaturated and calcite is oversaturated. Once dedolomitization starts the liberated Mg^{2+} has to be transported by a steady fluid flow. Otherwise the Mg^{2+}/Ca^{2+} ratio increases and dedolomitization ceases [8]. While small amounts of CO_{2} are necessary to bring dolomite into solution [9], a high CO_{2} partial pressure inhibits dedolomitization due to calcite being also undersaturated (.5 atm, de Groot [8]). Instead of calcite precipitation, dissolutionrelated secondary porosity is created. An early experimental study by de Groot (1967) further concluded that dedolomite may only form at temperatures lower than 50°C. This led to the general assumption that dedolomite is related to nearsurface processes, either linked to ancient paleosurfaces or linked to a phase of late surface weathering [10, 11]. Since then, several studies have found that dedolomitization takes place in a wide range of diagenetic settings, including shallow to deep burial [12–15]. Escorcia et al. [16] concluded that temperatures above 50°C may slow down dedolomitization rather than fully stopping it.
Due to the specific conditions under which dedolomite forms, it commonly occurs either connected to meteoric exposure surfaces or connected to enhanced fluid conduits such as faults and fractures [17, 18]. In contrast, dedolomites with similar macro and microfabrics have been described in other parts of the Southern Permian Basin from timeequivalent Zechstein2Carbonates, ranging from eastern Poland to the NE coast of England, sometimes affecting carbonate with hundreds of meters of thickness [2, 3, 9, 19–23].
The majority of the Ca2 dedolomite reported in Germany [9, 24–26], the Netherlands [21, 27], and Poland [28] is linked to burial. This interpretation is based on isotope data [9], which shows slight shifts in δ^{18}O relative to dolomite, elevated fluid inclusion temperatures of dedolomite [19, 28], and the absence of any signs of meteoric exposure after initial dolomitization [9, 25].
The CO_{2}, which is responsible for dedolomitization within the Ca2, is thought to be internally sourced [9]. The organic material, which is mostly present in the basin and lower slope facies, was subjected to thermal degradation and thereby released CO_{2}. The total organic carbon (TOC) of basin and lower slope is usually smaller than 1% with an average of 0.54% [29]. The thermal conversion takes place during the early stages of thermal organic matter maturation [30]. The CO_{2} then migrated upslope and initiated dedolomitization (Figure 1). Dissolution of dolomite also took place and led to local creation of secondary porosity, especially in the lower slope facies [9, 27]. In this model the origin as well as the migration path of the CO_{2} explains the spatial distribution of dedolomite within the Zechstein2Carbonates. Dedolomitization was most effective within the basin facies, which was nearly completely calcified. Towards the platform, the relative amount of dedolomite decreases gradually [9, 23]. Largest absolute amounts of dedolomite can be found on the upper to middle slope, where the Ca2 achieves its largest thickness [27].
Following the initial proposal by Clark [9], calcium sources for the Zechstein dedolomites have been largely attributed to the fluids released during gypsumtoanhydrite conversion of the over and underlying anhydrite sequences (A2 and A1) [9, 21, 23, 27]. During this process the gypsum sequence loses 49% of its volume in the form of intercrystalline water [31, 32]. These fluids are saturated with respect to CaSO_{4} [33]. The conversion reaction for this process is as follows:
Even though gypsumtoanhydrite conversion fluids are thought to be the only source for dedolomitization of the Zechstein2Carbonates [9], there has been no attempt to estimate their actual dedolomitization potential. The goal of this research is to quantitatively test the conventional Ca2 dedolomitization model. This will be achieved through a combination of geochemical batch modelling and mass balance calculations. In a first step, we will estimate the dedolomitization potential of fluids expelled by the conversion of gypsum to 1 m^{3} of anhydrite. That is to say, how much dolomite can potentially be transformed into calcite when gypsum dehydrates to 1 m^{3} of anhydrite. Subsequently, we will use the Northern Germany Zechstein basin as a case study to test how much of the observed dedolomite can be explained by this process. The results of this study may have direct implications for dedolomitization processes in other carbonate evaporite successions worldwide.
2. Geological Background
The Zechstein2Carbonates, also known as the Stassfurt Carbonate or the Ca2, were deposited in Southern Permian Basin (SPB) which itself forms part of the Central European Basin System (CEBS) [37]. The CEBS ranges from the east coast of England to Poland (Polish Trough) and from Norway to the central parts of Germany [38, 39].
Due to the hot arid climate and the lowering of source areas at the end of the Lower Permian Rotliegend, subsidence began to outpace sedimentation, resulting in the development of a basin with elevations way below the sea level. The onset of rifting combined with a general rise in sea level then led to the flooding of the depression by the Boreal Sea, which also marks the beginning of Zechstein sedimentation [40].
Further flooding led to the cyclic precipitation of thick sequences of carbonates, sulfates, and salt. Traditionally four carbonate/claystoneevaporite cycles have been described in Germany, known as the Werra (Z1), Stassfurt (Z2), Leine (Z3), and Aller (Z4) Series. More recently three additional cycles (Ohre Z5, Friesland Z6, and Fulda Z7) have been recognized in the axial parts of the Northern German Basin [28] (Figure 2).
Each cycle represents progressive evaporation with carbonates (Ca) and/or siliciclastics at their base transitioning into anhydrites (A) and topped by thick sequences of salt (Na) and small amounts of potassium and magnesium salts [1, 39, 41]. The Stassfurt carbonates are therefore abbreviated with Ca2. The Ca2 overlies the Werra Anhydrite (A1) and is itself succeeded by the Basal Anhydrite (Figure 2).
The depositional environment of the Ca2, within the study area, ranges from lower slope to platform (Figure 3). The thickness ranges between 20 and 80 m for platform and 10 and 250 m for slope deposits, with decreasing thickness from upper to lower slope. The basinal facies is usually thinner than 10 m. The overall trend in thickness and facies distribution is influenced by sealevel variations, tectonic subsidence, syndepositional tectonic, and the geometry of the underlying Werra Anhydrite [42]. Highest thicknesses are achieved within the upper slope, where the Ca2 directly overlies the former A1 slope [35].
3. Materials and Methods
The simulations include data from 18 industry wells situated southwest of Bremen in NW Germany, with each well drilled through the entirety of the A2, Ca2, and A1 providing a continuous and complete stratigraphic record. Calcite within the welllogs provided by ExxonMobil Production Deutschland GmbH (EMPG) was identified by reaction with hydrochloric acid (HCl). Based on this observation we calculated the calcitedolomite ratios which have been used for the presented model. Extensive petrographic evaluations have shown that the overwhelming majority of the calcite within the Ca2 displays textures which are typical for dedolomite [2–5, 9, 19, 20, 25, 43]. Therefore, calcite is assumed to be a good proxy for total amount of dedolomite. The well data is furthermore thought to be an approximation of the cumulative thickness of dedolomite layers.
Chemical batch analysis was achieved with the geochemical modelling software PHREEQC [44]. All PHREEQC calculations are based on the Specific Ion Interaction Theory database (sit.dat) developed by the French National Radioactive Waste Management Agency (ANDRA). The sit database was selected due to its compatibility with fluids of high ionic strength.
The creation of contour maps was achieved by linear interpolation using the Scientific Python (SciPy) library. Scipy is an open source Pythonbased library commonly used for scientific and technical computing [45].
4. Approach
To specify the dedolomitization potential of gypsumtoanhydrite dehydration fluids it is essential to define the volume of fluid released as well as the calcium concentration of those fluids. The total dissolved calcium is referenced to as Ca, to be inclusive of all aqueous species.
Taking molar volumes into consideration it can be calculated that 1 m^{3} of anhydrite may be formed due to the dehydration of 1.62 m^{3} of gypsum, releasing a total of 0.8 m^{3} of water [46]. This is equal to an overall volume increase of about 10%.
The solubility of anhydrite in water mainly depends on salinity and temperature and to a lesser degree on pressure [47]. A simple PHREEQC batch model, where anhydrite is brought into solution at different temperatures (10°C–70°C) and different salinities (0.0 moles/kgw–7.0 moles/kgw), shows that an increase in temperature decreases the solubility of anhydrite and that an increase in salinity increases the solubility of anhydrite (Figure 4). The influence of salinity on solubility is higher for low temperatures and decreases slightly at high temperatures. Solubilities displayed in Figure 4 are in good agreement with the batch modelling results of Li and Duan [47] and experimental data by Kushnir [48]. The Ca concentration of fluids released by gypsum dehydration therefore depends on temperature and salinity during the conversion into anhydrite.
A plot derived from the experimental data provided by Hardie [36] yielded transition temperatures of about 58°C in pure water. If the pore fluid composition approaches halite saturation the temperature needed for gypsumtoanhydrite conversion drops to approximately 18°C (Figure 5).
The highest Ca concentrations are reached when gypsumtoanhydrite dehydration occurs at high salinities and therefore at shallow burial depths and low temperatures (Figure 4).
Compared to salinity and temperature, the effect of pressure on the gypsumtoanhydrite conversion is small [49]. MacDonald [50] calculated a theoretical decrease of one degree in conversion temperature for an increase in pressure of 39.45 bar (3.945 MPa) under hydrostatic conditions. Assuming an average bulk density of 2.3 g/cm^{3} about 175 m of overburden would be necessary to decrease the conversion temperature by 1°C.
The amount of Ca necessary to replace 1 mole of dolomite with calcite depends on the reaction stoichiometry. The commonly denoted dedolomite reaction assumes that 1 mole of dolomite gets replaced by 2 moles of calcite (R1, Evamy [6]), consuming 1 mole of Ca. The dedolomitization potential increases exponentially for lower reaction stoichiometries, since less and less external calcium is needed for the replacement reaction (Figure 6). Due to the larger molar volume of 2 moles of calcite as compared to 1 mole of dolomite this reaction leads to an increase in solid volume and thereby a decrease in porosity (Figure 6). Dedolomitization may however also lead to the creation [11, 51, 52] or the preservation of porosity [6]. A pseudomorphic volumepervolume replacement is defined by the reaction stoichiometry of 1.74 : 1 which is the ratio between the molar volume of dolomite and calcite. We stopped modelling at the arbitrary ratio of 1.2 : 1 to display the range and influence of reaction stoichiometry on the dedolomitization potential (Figure 6). However, most dedolomite observed is associated with a loss or preservation of porosity rather than the increase thereof [6, 7, 53]. To determine the reaction stoichiometry during dedolomitization it is necessary to quantify the porosity within the original dolomite and dedolomite. Petrographic study of stained thinsections is best suited for this task since it allows for the differentiation between changes in porosity due to dedolomitization and other diagenetic processes. The resulting reaction stoichiometry can then be calculated withwhere [cm^{3}/mole] and [cm^{3}/mole] represent the molar volume of dolomite and calcite and and are equal to the porosity of dolomite and calcite expressed as decimal values.
The amount of dedolomite which is created ( [m^{3}]) is then defined bywhere [mole] represents the total amount of Ca ions in solution, Rs [/] is defined by the reaction stoichiometry, [m^{3}/mole] represents the molar volume of calcite, and [/] is equal to the porosity of the resulting dedolomite expressed as decimal value. The volume increases, if the resulting dedolomite contains residual porosity. This value has to be defined beforehand by means of petrographic observations, well log analysis, and/or petrophysical measurements.
The resulting dedolomitization potential is relatively low with values ranging between 0^{3 }m^{3} and 0^{3 }m^{3} of dedolomite created for each m^{3} of anhydrite, assuming that reaction stoichiometries vary from 1.74 to 2 (Figure 6). Correspondingly 126 m^{3} to 278 m^{3} of dehydration fluids is needed to create 1 m^{3} of calcite, assuming a 100% effective process.
5. Case Study: Zechstein2Carbonates
To test the dedolomitization potential of gypsumtoanhydrite conversion fluids we apply the aforementioned considerations regarding anhydrite solubility at the point of dehydration onto the Ca2 dedolomite system. To present a stronger argument we assume boundary conditions under which dedolomitization is favored. This implies low temperatures and high salinities during a shallow burial conversion (Figure 4). This assumption follows existing interpretations of very shallow conversion depths [54, 55] as well as shallow dedolomitization depths [9].
For the purpose of this model we estimate the conversion depth to be 50 m. Note that we do not propose that this depth is the real conversion depth but rather the depth at which the conversion fluid would have yielded a high dedolomitization potential.
The temperature for conversion at such low depths is dictated by the sea surface temperature during the late Permian, which is estimated to be 26°C [56]. The salinity necessary to achieve gypsumtoanhydrite conversion at such temperatures is equal to 6.1 (Figure 5). Since there is hardly any overburden at such low depths the pressure effect on conversion temperature and anhydrite solubility can be neglected. The solubility of anhydrite at the salinity and temperature specified above is equal to 83 moles per kg of water. This is equal to 65.3 moles per m^{3} of anhydrite created during dehydration.
The reaction stoichiometry was calculated with average porosities of dolomite (16.9%) and calcite (3.8%) for the Zechstein2Carbonates in NW Germany as determined by Biehl et al. [2]. The resulting reaction stoichiometry is equal to about 2 : 1. This fits the observed connection between dedolomitization and a nearcomplete loss of porosity within the study area [23].
Taking the above described boundary conditions into consideration we estimate that 0^{3 }m^{3} of dedolomite may be produced for each m^{3} of anhydrite. This dedolomitization potential can then be applied onto the selected wells to determine if the gypsumtoanhydrite conversion fluids represent a sufficient calcium source within each well. The amount of calcite in each well is determined by multiplying the calcitedolomite ratio with the thickness of the Ca2 of the selected well (Table 1).

The well data provided by EMPG includes the thickness of the over and underlying anhydrite sequences (A2 and A1, resp.). This value is then multiplied with the dedolomitization potential for the selected boundary conditions defined in this section. The result represents the amount of dedolomite which can potentially be created by the fluids released during gypsumtoanhydrite conversion for each well. This number is then compared with the actual amount of dedolomite observed in each well to estimate the amount of dedolomite which is accounted for by the gypsumtoanhydrite dehydration fluids (Table 1), as well as the spatial distribution of this ratio (Figure 7).
(a)
(b)
(c)
(d)
For the vast majority of the wells the dehydration fluids represent an insufficient Ca source. On the slope, where massive amounts of dedolomite can be found, the dehydration fluids account for less than 1% of the encountered dedolomite (Table 1). From slope to platform, a decrease of dedolomite content is observed to correlate with a decrease in insufficiency of the dehydration fluids. Five wells did not contain any dedolomite and were mainly included to better demonstrate the spatial distribution of dedolomite within the study area (Figure 7).
Due to the simplistic setup of the model the results include several uncertainties. For once we do not account for horizontal migration of conversion fluids. It has been shown that the wells studied from the platform environment of deposition contain low to no amounts of calcite (Table 1). Therefore, conversion fluids should be locally overabundant. The migration of these fluids to the slope, where the volume of over and underlying gypsum is insufficient, could lead to the additional input of Ca. However, excess dedolomite of the platform is about two orders of magnitude smaller than unaccounted dedolomite in the upper portion of the slope (Table 1). Therefore, it appears unlikely that the redistribution of conversion fluids could be responsible for this discrepancy (Figure 7).
The transport of conversion fluids from source (A2 and A1) to sink (Ca2) is treated as a 100% effective process. This likely leads to an overestimation dedolomitization potential. For once, the conversion fluids may lose Ca along the migration path due to processes other than dedolomitization. One possible additional sink for calcium is the cementation of the Ca2carbonates with anhydrite, which Clark [9] has linked to the influx of dehydration fluids.
The assumption that the total amount of fluids created during dehydration migrates into the Ca2 may also be flawed. The A2 is overlain by thick sequences of impermeable salt. It is therefore reasonable to assume that fluids migrated dominantly into the underlying Ca2. This is, however, not applicable to the A1, which overlies the Zechstein Limestone (“WerraKarbonat,” Ca1) (Figure 2). It has to be assumed that some amount of the dehydration fluids migrated downwards into the Ca1, therefore being unavailable for dedolomitization of the Ca2. This statement increases in relevance since the A1 is up to 20 times thicker than the A2 within the study area, thus contributing higher amounts of conversion fluids to the model (Table 1). Due to similar reasons it is possible that the assumed salinity ( = 6.1) is not representative for the A1, which was succeeded by a carbonate system, dominated by fluids of marine composition.
We propose the following processes as a potential alternative Ca source for the pervasive dedolomitization of the Zechstein2Carbonates:(i)Gypsum mush compaction(ii)Pressure solution of gypsum and/or anhydrite
At surface, gypsum can accumulate as a highly porous mush with reported porosities ranging between 30% and 67% [57, 58] and Ca pore fluid saturations being as high as 0.035 moles/liter [57]. During the early stages of compaction these fluids could be expelled into the Ca2 carbonates, thereby introducing fluids rich in Ca into the system [59]. However, since the volume and Ca saturation of these fluids range within the same order of magnitude as those which are produced during gypsum dehydration it appears unlikely that this process introduced enough Ca into the Ca2 system to explain the large amounts of dedolomite observed (Figure 4).
Another possible calcium source could be the dissolution of anhydrite or gypsum due to pressure. Bäuerle et al. [55] reported a high abundance of stylolites within the A3 “Hauptanhydrit” (Main Anhydrite) of the Gorleben salt dome in northern Germany. Assuming a volume loss of 26% [55] it is possible to calculate the amount of Ca which could potentially be introduced into the Ca2 of the study area by a similar stylolitization of the A1 and A2. Like dehydration, the amount of dedolomite which can be produced due to pressure solution is then primarily defined by the reaction stoichiometry as well as the porosity within the dedolomite.
A simulation run with equal boundary conditions compared to those proposed for the dehydration fluids reveals that the dedolomitization potential of pressure solution is substantially higher than that of dehydration fluids (Figure 7(c)). The platform, where dedolomite is rare and anhydrite thicknesses are rather large, displays a dedolomitization potential which greatly exceeds demand. Towards the upper and middle slope the model still fails to predict the large amounts of dedolomite encountered. However, the redistribution of excess Carich fluids predicted for the platform could explain the large quantities of dedolomite observed within the upper and middle slope.
6. Conclusion
Geochemical batch modelling and mass balance constraints reveal that fluids derived from gypsumtoanhydrite dehydration represent a potential Ca source for dedolomitization during burial. The amount of solid dedolomite created for each m^{3} of anhydrite ranges between 0^{−3} and 0^{3 }m^{3} depending on the temperature, salinity, and reaction stoichiometry (1.74 to 2) during dedolomitization, with highest values being achieved at low temperatures and high salinities. Dedolomitization due to gypsumtoanhydrite dehydration is therefore most effective during shallow burial.
However, the modelling results of the Zechstein2Carbonate case study challenge the classical dedolomitization model that has been applied for diagenetic reservoir models of the Ca2 across the Southern Permian Basin. Mass balance constraints show that additional calcium sources are necessary, to account for the large amounts of observed dedolomite. Considering that our calculations represent a bestcase scenario it may be concluded that gypsumtoanhydrite dehydration is not capable of producing the vast amounts of dedolomite, which can be found within the study area and by extension the Ca2 of the Southern Permian Basin. Instead this research suggests the presence of additional sources of calcium, such as pressure solution within the A2 and A1 sulfates. Further research is needed to shed light on the presence, magnitude, and distribution of pressure solution as well as the potential correlation with dedolomite distribution.
Conflicts of Interest
The authors declare that there are no conflicts of interest regarding the publication of this paper.
Acknowledgments
The authors like to thank ExxonMobil Production Deutschland GmbH (EMPG) for granting the right to publish the results of this study. Furthermore, they are grateful to EMPG for providing the large quantities of data used within this study. Sven Fellmin is acknowledged for the determination of calcitedolomite ratios within the studied wells. The authors deeply thank Christian Strohmenger and Franz Brauckmann for insightful discussions and thoughts.
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