# Supercritical Fluid Geochemistry in Geothermal Systems

Authors: Matylda Heřmanská; Barbara I. Kleine; Andri Stefánsson
Journal: Geofluids
 (2019)

---

## Abstract

Supercritical fluids exist in the roots of many active high-temperature geothermal systems. Utilization of such supercritical resources may multiply energy production from geothermal systems; yet, their occurrence, formation mechanism, and chemical properties are poorly constrained. Flow-through experiments at 260°C and 400-420°C were performed to study the chemical and mineralogical changes associated with supercritical fluid formation near shallow magmatic intrusions by conductive heating and boiling of conventional subcritical geothermal fluids. Supercritical fluids formed by isobaric heating of liquid geothermal water had similar volatile element concentrations (B, C, and S) as the subcritical water. In contrast, mineral-forming element concentrations (Si, Na, K, Ca, Mg, and Cl) in the supercritical fluid were much lower. The results are consistent with the observed mineral deposition of quartz, aluminum silicates, and minor amount of salts during boiling. Similar concentration patterns have been predicted from geochemical modeling and were observed at Krafla, Iceland, for the IDDP-1 supercritical fluid discharge. The experimental results confirm previous findings that supercritical fluids may originate from conductive heating of subcritical geothermal reservoir fluids characterized by similar or lower elemental concentrations with minor input of volcanic gas.


---

## Body

## 1. Introduction

Volcanic geothermal systems are associated with magmatic intrusions in the upper part of the Earth’s crust characterized by increased temperature, specific fluid enthalpy, and convection of groundwater [1]. Conventional exploitation of geothermal fluids from such systems typically produces an average of ~3–5 MW electric power per well [2] with a world total exploitation of geothermal energy in 2018 corresponding to ~14.4 GW [3]. Conductive heat transfer from a magmatic intrusion to the surrounding groundwater occurs in the roots of the geothermal system below the depth of typical conventional geothermal wells. Recent modeling suggests that supercritical fluids with temperatures and enthalpies exceeding ~400°C and ~3000 kJ kg-1, respectively, exist at the boundary between geothermal systems and the magmatic heat source, with such fluids possibly capable of generating up to ~30-50 MW of electricity from a single well or ten times more than conventional geothermal wells [4].Supercritical geothermal fluids have commonly been classified based on the critical temperatureTc=373.976°C and pressure Pc=22.01MPa of pure water (H2O) [5]. Such a definition can lead to an artificial boundary in the phase diagram of water, across which there is actually a continuous change in fluid properties. Moreover, for binary salt-water fluids, the term “supercritical” may not fully describe the fluid phase properties, as critical behavior occurs along critical temperature and pressure, implying fluid phase separation rather than homogenization. Here and following Liebscher and Heinrich [6], the term supercritical is defined as a single-phase vapor with a temperature above the critical temperature. Supercritical fluids have been suggested to form by groundwater circulation near the intrusion [1, 7, 8] with or without input from magmatic gas [9–11]. More than 25 deep wells sunk into the geothermal fields at The Geysers, Salton Sea, and Hawaii (USA); Kakkonda (Japan); Larderello (Italy); Krafla, Nesjavellir, and Reykjanes (Iceland); Los Humeros (Mexico); and Menengai (Kenya) have reached temperatures in excess of the critical temperature of water and, in some cases, have even encountered magma [12]. The most extensive project aiming at obtaining supercritical fluids for geothermal utilization is the Iceland Deep Drilling Project (http://www.iddp.is). In 2009, the IDDP-1 well at Krafla (NE Iceland) came to a halt after drilling into molten magma at ~2.1 km depth [13]. After an initial heating period, the well discharged supercritical fluids with temperatures of ~440°C and eventually reached a maximum temperature of 459°C and specific enthalpy of ~3200 kJ kg-1 [14, 15]. From March 2010 until September 2011, series of flow tests were conducted; however, due to the corrosive nature of the fluids, silica scaling, and thermal damage to the well casings, utilization proved to be challenging and the fluid discharge was eventually terminated [16]. In 2017, the second IDDP-2 well at Reykjanes (SW Iceland) reached its target depth of 4.6 km with a measured bottom hole temperature of 426°C [17]. At present, fluid discharges from IDDP-2 at surface are not characterized by supercritical temperatures. Thus, deep reservoir fluid composition has been estimated from fluid inclusion analysis of felsic veins consisting of a vapor phase dominated by water (97.5 mol% H2O, ~1.5 mol% CO2, 0.7 mol% H2S, and traces of H2), Cl-rich brine (Fe-K chlorides, sylvite-halide solid solutions), and sulfides [18].Magmatic intrusions emplaced into the upper parts of the Earth’s crust may exsolve magmatic fluids at near lithostatic pressure, resulting in fracturing of the surrounding rocks and magmatic fluid migration [19, 20]. Near magmatic intrusions, conductive heat addition to the surrounding groundwater system may also potentially form high-temperature supercritical fluids [1, 7]. However, permeability may rapidly decrease at the brittle-ductile transition (BDT), possibly limiting the formation of such supercritical fluids to lithologies with basaltic glass transition temperatures above ~400-450°C [1, 7, 21–23]. While the relations between rock permeability and brittle-ductile behavior, as well as reservoir simulations around magmatic intrusions, have received considerable interest, less attention has been drawn to the geochemical properties of such supercritical fluids. Fluids originating from degassing magma are rich in CO2, SO2, HCl, and HF [24]. In contrast, supercritical fluids formed by boiling of subcritical geothermal water of meteoric or seawater origin are considered to display similar concentrations of many volatile elements (CO2, H2S, H2, and B) as the original water, much lower than corresponding magmatic-gas concentrations, but negligible nonvolatile element concentrations (Si, Na, K, Ca, and Mg) [25–31]. The formation of supercritical fluids may also produce a silica deposit around the magmatic intrusion [25, 31, 32] (Figure 1).Figure 1
Main characteristics of a volcanic geothermal system. (a) Conceptual model showing fluid flow paths, the brittle-ductile transition (BDT) between the magmatic heat source and the circulating geothermal fluid, and depressurization boiling near the surface. Constructed based on Arnórsson et al. [60] and Scott et al. [8]. (b) The boiling curve of water. (c) The phase diagram of water showing pressure, specific enthalpy, and temperature relations. Also shown are the subcritical (SubC) to supercritical (SupC) conditions of the experiments carried out in this study.In this study, flow-through experiments at 260°C and 400-420°C were performed to study how conductive heating of subcritical water form geothermal fluids at supercritical temperatures and how this affects fluid chemistry and associated secondary mineral formation. The results of the experiments were further compared with the recent model simulations of the chemical nature of supercritical fluids near magmatic intrusions and with the observed composition of the supercritical fluid discharged by the IDDP-1 [31].


## 2. Methods

### 2.1. Experimental Set-Up

Flow-through experiments at 260°C and 400-420°C and 6.9 MPa reproduce geothermal reservoir conditions at subcritical and supercritical temperatures, respectively. A schematic illustration of the experimental set-up is shown in Figure2, and a summary of experimental conditions is given in Table 1. All wetted parts of the experimental apparatus were made of inert material, including PEEK, titanium, and Inconel. Inlet solutions were pumped at a flow rate of ~0.20 ml/min using an HPLC pump (Chromatech®). The pressure was controlled at the end of the line by a back-pressure regulator (BPR, Biotech).Figure 2
Schematic set-up of the experiments described in this study.Table 1
Initial conditions of the experiments.
#
t (°C)
P (MPa)
Q (g min-1)
Material
Grain size (μm)
SubC-1
260
6.9
0.09-0.26
BAS
45-125
SupC-1
420
6.9
0.19-0.21
SS316-rod
SupC-2
400
6.9
0.10-0.19
SS316-rodThe first reactor (SubC), representing subcritical conditions, was heated to 260°C and filled with fine-grained basaltic glass (grain size fraction < 45μm) from Stapafell, Iceland (Table 2). The second reactor (SupC), representing supercritical conditions, was heated to 400-420°C. This reactor contained a stainless steel (316) threaded rod to capture deposits precipitating from the fluids. Three different experiments were carried out to test the effects of temperature and solution composition on fluid composition and alteration mineralogy. The initial solution in all cases was of natural geothermal water from Krafla, Iceland (Table 3). In experiment 1, interaction between geothermal liquid water and basaltic rocks at subcritical temperatures (260°C) was conducted. In experiments 2 and 3, the geothermal water either from the outlet subcritical reactor or directly from the inlet solution was pumped into a flow-through reactor with a supercritical temperature of 400-420°C. In all cases, the fluids were cooled down by an in-line cooling jacket, followed by depressurization by a BPR and collection of fluid samples. At the end of each experiment, the solid deposits from the reactor were collected, dried at 50°C, and mounted on a sample holder. Loose precipitates from the rod collected from the supercritical reactor were directly mounted on a sample holder to study the morphology of the deposits. The rod itself was imbedded into epoxy and cut parallel and perpendicular to the flow direction in the reactor and then polished.Table 2
Basaltic glass composition (BAS)a.
Element
SiO2
wt.%
48.12
Al2O3
wt.%
14.62
FeO
wt.%
9.82
Fe2O3
wt.%
1.11
MgO
wt.%
9.08
CaO
wt.%
11.82
Na2O
wt.%
1.97
K2O
wt.%
0.29
Clb
ppm
220
CO2b
ppm
100
Bb
ppm
1.0
aBasaltic glass from Stapafell [62]. bTaken as for average basalts in Iceland, after Kaasalainen and Stefánsson [64].


### 2.2. Chemical Analyses

For the fluid samples, the pH was analyzed using a pH electrode and meter calibrated against commercial buffer solutions. Measurements of CO2 and H2S concentrations were carried out using a modified alkalinity and Hg-precipitation titration using dithizone as an indicator, respectively [33, 34]. For CO2 determination, the samples from the supercritical reactor were collected into a base (0.01 M NaOH) to prevent degassing prior to analyses. For major elemental analyses (Si, B, Na, K, Ca, Mg, Al, Fe, Cl, and SO4), the samples were filtered through a 0.2 μm filter (cellulose acetate), acidified to 1% with HNO3 (Merck, Suprapur®), followed by analysis using ICP-OES (Spectro Ciros Vision). The analytical precision of major element analyses was based on repeated analysis of the GYG13 standard and was found to be <3% at the 95% confidence level for all elements except Fe, where it was ~14%. The analytical precision for pH was ±0.05.The secondary mineral phases and the morphology of the solid products from the two reactors were determined using a HITACHI TM-3000 scanning electron microscope (SEM) with an accelerating voltage of 15 kV.


## 2.1. Experimental Set-Up

Flow-through experiments at 260°C and 400-420°C and 6.9 MPa reproduce geothermal reservoir conditions at subcritical and supercritical temperatures, respectively. A schematic illustration of the experimental set-up is shown in Figure2, and a summary of experimental conditions is given in Table 1. All wetted parts of the experimental apparatus were made of inert material, including PEEK, titanium, and Inconel. Inlet solutions were pumped at a flow rate of ~0.20 ml/min using an HPLC pump (Chromatech®). The pressure was controlled at the end of the line by a back-pressure regulator (BPR, Biotech).Figure 2
Schematic set-up of the experiments described in this study.Table 1
Initial conditions of the experiments.
#
t (°C)
P (MPa)
Q (g min-1)
Material
Grain size (μm)
SubC-1
260
6.9
0.09-0.26
BAS
45-125
SupC-1
420
6.9
0.19-0.21
SS316-rod
SupC-2
400
6.9
0.10-0.19
SS316-rodThe first reactor (SubC), representing subcritical conditions, was heated to 260°C and filled with fine-grained basaltic glass (grain size fraction < 45μm) from Stapafell, Iceland (Table 2). The second reactor (SupC), representing supercritical conditions, was heated to 400-420°C. This reactor contained a stainless steel (316) threaded rod to capture deposits precipitating from the fluids. Three different experiments were carried out to test the effects of temperature and solution composition on fluid composition and alteration mineralogy. The initial solution in all cases was of natural geothermal water from Krafla, Iceland (Table 3). In experiment 1, interaction between geothermal liquid water and basaltic rocks at subcritical temperatures (260°C) was conducted. In experiments 2 and 3, the geothermal water either from the outlet subcritical reactor or directly from the inlet solution was pumped into a flow-through reactor with a supercritical temperature of 400-420°C. In all cases, the fluids were cooled down by an in-line cooling jacket, followed by depressurization by a BPR and collection of fluid samples. At the end of each experiment, the solid deposits from the reactor were collected, dried at 50°C, and mounted on a sample holder. Loose precipitates from the rod collected from the supercritical reactor were directly mounted on a sample holder to study the morphology of the deposits. The rod itself was imbedded into epoxy and cut parallel and perpendicular to the flow direction in the reactor and then polished.Table 2
Basaltic glass composition (BAS)a.
Element
SiO2
wt.%
48.12
Al2O3
wt.%
14.62
FeO
wt.%
9.82
Fe2O3
wt.%
1.11
MgO
wt.%
9.08
CaO
wt.%
11.82
Na2O
wt.%
1.97
K2O
wt.%
0.29
Clb
ppm
220
CO2b
ppm
100
Bb
ppm
1.0
aBasaltic glass from Stapafell [62]. bTaken as for average basalts in Iceland, after Kaasalainen and Stefánsson [64].


## 2.2. Chemical Analyses

For the fluid samples, the pH was analyzed using a pH electrode and meter calibrated against commercial buffer solutions. Measurements of CO2 and H2S concentrations were carried out using a modified alkalinity and Hg-precipitation titration using dithizone as an indicator, respectively [33, 34]. For CO2 determination, the samples from the supercritical reactor were collected into a base (0.01 M NaOH) to prevent degassing prior to analyses. For major elemental analyses (Si, B, Na, K, Ca, Mg, Al, Fe, Cl, and SO4), the samples were filtered through a 0.2 μm filter (cellulose acetate), acidified to 1% with HNO3 (Merck, Suprapur®), followed by analysis using ICP-OES (Spectro Ciros Vision). The analytical precision of major element analyses was based on repeated analysis of the GYG13 standard and was found to be <3% at the 95% confidence level for all elements except Fe, where it was ~14%. The analytical precision for pH was ±0.05.The secondary mineral phases and the morphology of the solid products from the two reactors were determined using a HITACHI TM-3000 scanning electron microscope (SEM) with an accelerating voltage of 15 kV.


## 3. Results

### 3.1. Chemical Composition of the Outlet Solutions

The chemical compositions of the outlet solutions from the experiments are given in Table3 and shown in Figure 3. The outlet solutions from the subcritical reactor (experiment 1) were mildly alkaline (pH 8.00- 9.79 at 21°C) with concentrations of SiO2 (325-674 ppm), B (3.35-3.48 ppm), Na (160-212 ppm), K (18.6-55.5 ppm), Cl (43.2-50.0 ppm), CO2 (55.5-99.0 ppm), SO4 (98-207 ppm), and H2S (17.4-57.9 ppm) similar to concentrations in the inlet solution (Table 3). Concentrations of Ca (0.69-3.04 ppm) were significantly lower than corresponding concentrations in the inlet solution (7.61 ppm) whereas Al concentrations (4.86-8.04 ppm) were significantly higher in the outlet solutions than in the inlet solution (0.84 ppm). The outlet solutions from the supercritical reactors were mildly acidic (pH 3.24 to 5.06 at 21°C). In experiment 2, concentrations of SiO2 (1.3-5.3 ppm), Na (0.1-0.2 ppm), K (<0.07 ppm), Ca (0.02-0.09 ppm), Al (0.018-0.081 ppm), Cl (0.35-0.48 ppm), and SO4 (0.27-0.49 ppm) were considerably lower than the corresponding concentrations of the inlet solution from the subcritical reactor. Concentrations of B (2.58-4.16 ppm), CO2 (8.32-225 ppm), and H2S (7.56-28.0 ppm) of the outlet solution did not differ much from the inlet solution (Figure 3). In experiment 3, similar trends were observed. Concentrations of SiO2 (1.2-4.6 ppm), Na (0.4-1.6 ppm), K (<0.3 ppm), Ca (0.06-0.17 ppm), Al (0.041-0.17 ppm), Cl (1.41-2.85 ppm), and SO4 (0.26-1.74 ppm) were substantially lower than the corresponding concentrations in the inlet solution (Figure 3). Again, concentrations of B (1.30-1.47 ppm), CO2 (35.4-135 ppm), and H2S (10.7-40.0 ppm) of the outlet solutions did not differ significantly from the inlet solution. Concentrations of Fe and Mg in all fluid samples were close to the detection limit and/or affected by contamination and were not considered further in this study.Table 3
Chemical composition of the solutions from the SubC and SupC reactors. Concentrations are in ppm.
Run #
t (°C)
pH
/
°C
SiO2
B
Na
K
Ca
Mg
Fe
Al
Cl
CO2
SO4
H2S
Subcritical
SubC-1-S1
260
8.08
/
21
535
3.46
165
21.1
0.70
0.023
0.029
6.88
45.4
82.3
98.0
44.0
SubC-1-S2
260
8.02
/
21
526
3.36
160
30.8
1.00
0.010
0.060
6.21
43.2
87.1
180
38.5
SubC-1-S3
260
8.21
/
21
548
3.44
165
22.5
0.69
0.003
0.023
6.69
43.6
83.2
138
57.9
SubC-1-S4
260
8.50
/
21
493
3.46
168
23.0
1.72
0.004
0.154
5.13
44.7
99.0
142
40.9
SubC-1-S5
260
8.70
/
21
440
3.41
173
22.0
2.71
0.003
0.028
4.86
44.0
94.2
124
40.6
SubC-1-S6
260
9.03
/
21
383
3.38
177
21.9
3.04
0.002
0.019
5.61
43.2
73.9
164
40.6
SubC-1-S7
260
9.18
/
21
356
3.35
186
21.3
2.90
0.000
0.032
6.50
44.0
78.3
173
36.1
SubC-1-S8
260
9.37
/
21
336
3.38
196
20.7
2.45
0.005
0.020
6.48
46.1
76.6
137
49.1
SubC-1-S9
260
9.79
/
21
327
3.36
200
19.5
2.43
0.000
0.017
6.61
44.7
70.9
158
36.1
SubC-1-S10
260
9.63
/
21
332
3.38
205
19.3
2.22
0.002
0.046
6.48
45.4
63.8
188
36.1
SubC-1-S11
260
9.64
/
21
325
3.36
207
18.6
2.14
0.007
0.036
6.15
45.4
65.1
164
37.8
SubC-1-S12
260
9.60
/
21
329
3.36
212
55.5
2.21
0.005
0.058
5.96
50.0
66.0
202
26.9
SubC-1-S13
260
8.09
/
21
634
3.48
167
21.5
1.47
0.054
0.079
8.04
44.7
55.5
154
30.7
SubC-1-S14
260
8.00
/
21
674
3.46
161
21.9
1.58
0.012
0.042
5.26
44.0
90.7
152
27.3
SubC-1-S15
260
8.40
/
21
559
3.46
171
22.4
1.44
0.005
0.012
6.23
44.3
67.3
207
17.4
SubC-1 inleta
260
8.82
/
21
453
3.41
181
24.1
1.91
0.009
0.044
6.21
44.8
76.9
159
37.3
Krafla w17b
275d
9.30
/
21
699
1.49
144
24.0
0.35
0.012
0.025
1.94
24.6
49.1
79.6
53.5
Krafla w37c
265e
7.95
/
20
488
3.46
156
22.8
7.61
0.012
0.018
0.84
46.1
106
90.8
40.9
Supercritical
SupC-1-S17
420
5.06
/
21
5.3
3.19
0.2
0.07
0.06
0.002
0.050
0.022
0.35
8.32
0.45
13.9
SupC-1-S18
420
4.96
/
21
3.6
4.16
0.1
0.06
0.09
0.005
0.069
0.062
19.8
0.49
17.2
SupC-1-S19
420
4.75
/
21
2.3
3.30
0.1
0.02
0.02
0.002
0.042
0.027
0.46
24.5
0.32
8.18
SupC-1-S20
420
4.90
/
21
2.1
3.35
0.1
0.02
0.02
0.002
0.026
0.018
0.37
15.7
0.27
10.5
SupC-1-S21
420
4.50
/
21
1.5
2.58
0.2
0.04
0.02
0.003
0.024
0.044
0.48
268
0.40
12.0
SupC-1-S22
420
5.00
/
21
1.4
3.47
0.2
0.05
0.05
0.003
0.029
0.029
0.46
25.1
0.38
7.56
SupC-1-S23
420
4.40
/
21
1.4
3.42
0.1
<0.1
0.03
0.004
0.039
0.081
225
0.35
28.0
SupC-1-S24
420
4.60
/
21
1.3
2.92
0.1
0.04
0.02
0.003
0.037
0.064
0.36
105
0.33
13.9
SupC-2-SSE1
400
3.99
/
22
4.6
1.30
0.5
<0.1
0.12
0.029
0.208
0.173
1.89
46.5
0.26
13.8
SupC-2-SSE2
400
4.17
/
22
4.3
1.43
1.6
0.25
0.15
0.041
0.181
0.060
2.13
35.4
0.78
10.7
SupC-2-SSE3
400
3.97
/
22
3.1
1.47
1.1
0.26
0.08
0.019
0.099
0.075
1.90
38.0
0.67
40.0
SupC-2-SS34
400
3.68
/
22
2.9
1.32
1.5
0.19
0.06
0.021
0.083
0.059
2.85
59.6
0.54
29.9
SupC-2-SSE5
400
3.24
/
21
2.8
1.37
0.4
<0.1
0.11
0.019
0.058
0.041
2.05
55.3
0.36
24.9
SupC-2-SSE6
400
3.65
/
21
1.2
1.38
1.0
<0.1
0.17
0.028
0.102
0.071
1.41
53.7
1.74
25.1
SupC-2-SSE7
400
3.41
/
21
1.4
1.44
0.8
<0.1
0.04
0.023
0.080
0.056
1.75
135
1.50
31.2
aThe average inlet composition of subcritical experiments SubC-1-n that served as inlet solution for supercritical experiment SupC-1-n. bKrafla w17 was used as an inlet for subcritical experiments SubC-1-n. Note: the inlet solution represents the liquid phase only discharge from the well w17. cThe Krafla w37 was used as inlet for the supercritical experiments SupC-2-n. Note: the inlet solution represents the liquid phase only discharge from the well w37. dBased on Gudmundsson and Arnórsson [41]. eBased on Ntihabose [63].Figure 3
Elemental concentrations of inlet and outlet solutions of the experiments. Abbreviations: SubC and SupC refer to subcritical and supercritical conditions, respectively.


### 3.2. Mineralogy and Chemical Composition of the Solid Products

Secondary minerals associated with alteration of the basaltic glass at subcritical temperatures (260°C) occurred mainly as thin layers on the surface of the primary glass. The main secondary minerals identified were chlorites, Na-Ca zeolite (wairakite), Ca-silicate (wollastonite), and calcite (Figure4(a) and (b)). For supercritical temperatures, abundant white deposits on the steel rod were observed, mainly composed of quartz (Figure 4(c)). Microcline and wollastonite were found in minor amounts. Thick deposits (1-2 mm) occurred on the part of the rod located closest to the inlet of the reactor. Here, silicate layers were most massive closest to the rod, becoming highly porous with increasing distance from the rod. Towards the outlet of the reactor, quartz precipitates occurred as amorphous silica (spheres with <1 μm in diameter) interconnected with fine silica branches up to 10 μm long (Figure 4(d)).Figure 4
Selected SEM microphotographs and EDS spectras of minerals precipitated at both subcritical (a, b) and supercritical temperatures (c, d).


## 3.1. Chemical Composition of the Outlet Solutions

The chemical compositions of the outlet solutions from the experiments are given in Table3 and shown in Figure 3. The outlet solutions from the subcritical reactor (experiment 1) were mildly alkaline (pH 8.00- 9.79 at 21°C) with concentrations of SiO2 (325-674 ppm), B (3.35-3.48 ppm), Na (160-212 ppm), K (18.6-55.5 ppm), Cl (43.2-50.0 ppm), CO2 (55.5-99.0 ppm), SO4 (98-207 ppm), and H2S (17.4-57.9 ppm) similar to concentrations in the inlet solution (Table 3). Concentrations of Ca (0.69-3.04 ppm) were significantly lower than corresponding concentrations in the inlet solution (7.61 ppm) whereas Al concentrations (4.86-8.04 ppm) were significantly higher in the outlet solutions than in the inlet solution (0.84 ppm). The outlet solutions from the supercritical reactors were mildly acidic (pH 3.24 to 5.06 at 21°C). In experiment 2, concentrations of SiO2 (1.3-5.3 ppm), Na (0.1-0.2 ppm), K (<0.07 ppm), Ca (0.02-0.09 ppm), Al (0.018-0.081 ppm), Cl (0.35-0.48 ppm), and SO4 (0.27-0.49 ppm) were considerably lower than the corresponding concentrations of the inlet solution from the subcritical reactor. Concentrations of B (2.58-4.16 ppm), CO2 (8.32-225 ppm), and H2S (7.56-28.0 ppm) of the outlet solution did not differ much from the inlet solution (Figure 3). In experiment 3, similar trends were observed. Concentrations of SiO2 (1.2-4.6 ppm), Na (0.4-1.6 ppm), K (<0.3 ppm), Ca (0.06-0.17 ppm), Al (0.041-0.17 ppm), Cl (1.41-2.85 ppm), and SO4 (0.26-1.74 ppm) were substantially lower than the corresponding concentrations in the inlet solution (Figure 3). Again, concentrations of B (1.30-1.47 ppm), CO2 (35.4-135 ppm), and H2S (10.7-40.0 ppm) of the outlet solutions did not differ significantly from the inlet solution. Concentrations of Fe and Mg in all fluid samples were close to the detection limit and/or affected by contamination and were not considered further in this study.Table 3
Chemical composition of the solutions from the SubC and SupC reactors. Concentrations are in ppm.
Run #
t (°C)
pH
/
°C
SiO2
B
Na
K
Ca
Mg
Fe
Al
Cl
CO2
SO4
H2S
Subcritical
SubC-1-S1
260
8.08
/
21
535
3.46
165
21.1
0.70
0.023
0.029
6.88
45.4
82.3
98.0
44.0
SubC-1-S2
260
8.02
/
21
526
3.36
160
30.8
1.00
0.010
0.060
6.21
43.2
87.1
180
38.5
SubC-1-S3
260
8.21
/
21
548
3.44
165
22.5
0.69
0.003
0.023
6.69
43.6
83.2
138
57.9
SubC-1-S4
260
8.50
/
21
493
3.46
168
23.0
1.72
0.004
0.154
5.13
44.7
99.0
142
40.9
SubC-1-S5
260
8.70
/
21
440
3.41
173
22.0
2.71
0.003
0.028
4.86
44.0
94.2
124
40.6
SubC-1-S6
260
9.03
/
21
383
3.38
177
21.9
3.04
0.002
0.019
5.61
43.2
73.9
164
40.6
SubC-1-S7
260
9.18
/
21
356
3.35
186
21.3
2.90
0.000
0.032
6.50
44.0
78.3
173
36.1
SubC-1-S8
260
9.37
/
21
336
3.38
196
20.7
2.45
0.005
0.020
6.48
46.1
76.6
137
49.1
SubC-1-S9
260
9.79
/
21
327
3.36
200
19.5
2.43
0.000
0.017
6.61
44.7
70.9
158
36.1
SubC-1-S10
260
9.63
/
21
332
3.38
205
19.3
2.22
0.002
0.046
6.48
45.4
63.8
188
36.1
SubC-1-S11
260
9.64
/
21
325
3.36
207
18.6
2.14
0.007
0.036
6.15
45.4
65.1
164
37.8
SubC-1-S12
260
9.60
/
21
329
3.36
212
55.5
2.21
0.005
0.058
5.96
50.0
66.0
202
26.9
SubC-1-S13
260
8.09
/
21
634
3.48
167
21.5
1.47
0.054
0.079
8.04
44.7
55.5
154
30.7
SubC-1-S14
260
8.00
/
21
674
3.46
161
21.9
1.58
0.012
0.042
5.26
44.0
90.7
152
27.3
SubC-1-S15
260
8.40
/
21
559
3.46
171
22.4
1.44
0.005
0.012
6.23
44.3
67.3
207
17.4
SubC-1 inleta
260
8.82
/
21
453
3.41
181
24.1
1.91
0.009
0.044
6.21
44.8
76.9
159
37.3
Krafla w17b
275d
9.30
/
21
699
1.49
144
24.0
0.35
0.012
0.025
1.94
24.6
49.1
79.6
53.5
Krafla w37c
265e
7.95
/
20
488
3.46
156
22.8
7.61
0.012
0.018
0.84
46.1
106
90.8
40.9
Supercritical
SupC-1-S17
420
5.06
/
21
5.3
3.19
0.2
0.07
0.06
0.002
0.050
0.022
0.35
8.32
0.45
13.9
SupC-1-S18
420
4.96
/
21
3.6
4.16
0.1
0.06
0.09
0.005
0.069
0.062
19.8
0.49
17.2
SupC-1-S19
420
4.75
/
21
2.3
3.30
0.1
0.02
0.02
0.002
0.042
0.027
0.46
24.5
0.32
8.18
SupC-1-S20
420
4.90
/
21
2.1
3.35
0.1
0.02
0.02
0.002
0.026
0.018
0.37
15.7
0.27
10.5
SupC-1-S21
420
4.50
/
21
1.5
2.58
0.2
0.04
0.02
0.003
0.024
0.044
0.48
268
0.40
12.0
SupC-1-S22
420
5.00
/
21
1.4
3.47
0.2
0.05
0.05
0.003
0.029
0.029
0.46
25.1
0.38
7.56
SupC-1-S23
420
4.40
/
21
1.4
3.42
0.1
<0.1
0.03
0.004
0.039
0.081
225
0.35
28.0
SupC-1-S24
420
4.60
/
21
1.3
2.92
0.1
0.04
0.02
0.003
0.037
0.064
0.36
105
0.33
13.9
SupC-2-SSE1
400
3.99
/
22
4.6
1.30
0.5
<0.1
0.12
0.029
0.208
0.173
1.89
46.5
0.26
13.8
SupC-2-SSE2
400
4.17
/
22
4.3
1.43
1.6
0.25
0.15
0.041
0.181
0.060
2.13
35.4
0.78
10.7
SupC-2-SSE3
400
3.97
/
22
3.1
1.47
1.1
0.26
0.08
0.019
0.099
0.075
1.90
38.0
0.67
40.0
SupC-2-SS34
400
3.68
/
22
2.9
1.32
1.5
0.19
0.06
0.021
0.083
0.059
2.85
59.6
0.54
29.9
SupC-2-SSE5
400
3.24
/
21
2.8
1.37
0.4
<0.1
0.11
0.019
0.058
0.041
2.05
55.3
0.36
24.9
SupC-2-SSE6
400
3.65
/
21
1.2
1.38
1.0
<0.1
0.17
0.028
0.102
0.071
1.41
53.7
1.74
25.1
SupC-2-SSE7
400
3.41
/
21
1.4
1.44
0.8
<0.1
0.04
0.023
0.080
0.056
1.75
135
1.50
31.2
aThe average inlet composition of subcritical experiments SubC-1-n that served as inlet solution for supercritical experiment SupC-1-n. bKrafla w17 was used as an inlet for subcritical experiments SubC-1-n. Note: the inlet solution represents the liquid phase only discharge from the well w17. cThe Krafla w37 was used as inlet for the supercritical experiments SupC-2-n. Note: the inlet solution represents the liquid phase only discharge from the well w37. dBased on Gudmundsson and Arnórsson [41]. eBased on Ntihabose [63].Figure 3
Elemental concentrations of inlet and outlet solutions of the experiments. Abbreviations: SubC and SupC refer to subcritical and supercritical conditions, respectively.


## 3.2. Mineralogy and Chemical Composition of the Solid Products

Secondary minerals associated with alteration of the basaltic glass at subcritical temperatures (260°C) occurred mainly as thin layers on the surface of the primary glass. The main secondary minerals identified were chlorites, Na-Ca zeolite (wairakite), Ca-silicate (wollastonite), and calcite (Figure4(a) and (b)). For supercritical temperatures, abundant white deposits on the steel rod were observed, mainly composed of quartz (Figure 4(c)). Microcline and wollastonite were found in minor amounts. Thick deposits (1-2 mm) occurred on the part of the rod located closest to the inlet of the reactor. Here, silicate layers were most massive closest to the rod, becoming highly porous with increasing distance from the rod. Towards the outlet of the reactor, quartz precipitates occurred as amorphous silica (spheres with <1 μm in diameter) interconnected with fine silica branches up to 10 μm long (Figure 4(d)).Figure 4
Selected SEM microphotographs and EDS spectras of minerals precipitated at both subcritical (a, b) and supercritical temperatures (c, d).


## 4. Discussion

### 4.1. Geochemistry of Subcritical Geothermal Fluids

Studies of alteration mineralogy and fluid composition in geothermal systems show that equilibrium is closely approached between the geothermal fluids and secondary minerals formed in the systems, except for mobile elements such as Cl [35–39]. At Krafla, the most common secondary minerals identified include calcite, quartz, epidote, various clays, chlorite, feldspars, and pyrite. Anhydrite, prehnite, actinolite, wollastonite, garnet, pyrrhotite, and various zeolites, including wairakite, have also been observed [40]. Previous studies on mineral-fluid interaction at Krafla have demonstrated that the major fluid components were in equilibrium with these minerals, which in turn control the fluid composition at depth (Figure 5) [41].Figure 5
Mineral saturation state of selected minerals at subcritical conditions. The reaction quotients were calculated using the Phreeqc program [61] and the llnl.dat database. Also shown are mineral solubilities and the mineral reaction quotients for reservoir fluids at Krafla at the measured reservoir temperatures, both obtained from Gudmundsson and Arnórsson [41].Our experimental results indicate a similar process of mineral-fluid interaction at subcritical temperatures, with formation of secondary minerals upon interaction of geothermal water with the primary basaltic rock and glass. The calculated saturation indices with respect to commonly observed secondary minerals revealed near-equilibrium between the fluids and quartz, whereas supersaturation occurs with respect to calcite, chlorite, feldspars, wollastonite, and zeolites (Figure5). Supersaturation may have resulted from high initial concentrations in the inlet experimental solutions relative to the equilibrium composition at 260°C and experimental durations of hours, compared to residence times of fluids in natural geothermal systems like at Krafla that are in the order of months to years [42, 43]. We conclude that the chemical composition of geothermal fluids at subcritical temperatures is controlled by near-equilibrium with secondary minerals. This agrees with previous findings [35–39, 41].


### 4.2. Supercritical Fluid Formation, Fluid-Rock Interaction, and Control of Elemental Transport

The solubility of mineral-forming elements and salts including Si, Ca, K, Na, and Cl is orders of magnitude lower in supercritical fluids compared to subcritical fluids and has been observed to decrease with decreasing fluid density [44–46]. Indeed, a recent modeling study of the formation of supercritical fluid by conductive boiling of subcritical fluids revealed that the process is expected to result in mineral deposition dominated by silica, aluminum silicates, and salts around the heat source [31]. In contrast, volatile elements like B, CO2, and H2S are expected to partition into the vapor phase upon boiling, resulting in insignificant concentration changes in the total fluid.Elemental behavior upon conductive heating of subcritical liquid water to form supercritical fluid may be demonstrated from the elemental relative mobilities (RM), given by the elemental concentration (mi) ratio between the inlet and outlet solution relative to a mobile element like B:
(1)RM=mi/mBoutletmi/mBinlet.The results demonstrate that volatile elements separate from the major rock-forming elements upon boiling of subcritical fluids to supercritical temperatures (Figure6). Boron, CO2, and H2S partition into the vapor phase, whereas nonvolatile elements like Si, Ca, Na, K, Al, Cl, and SO4 are precipitated into the observed secondary minerals, mainly silica, aluminum silicates, and chlorides. Chloride may also precipitate into salts like halite and sylvite (Figure 4). In this way, <1-10% of these elements are quantitatively removed from the initial concentration of the subcritical fluids.Figure 6
Relative mobility of major elements upon boiling of subcritical geothermal fluids by conductive heating to form supercritical fluids. Elements showing relative mobility close to 1 may be regarded as mobile, whereas elements with relative mobility of <0.1 are immobile.The elemental concentrations can be further compared with the mineral-fluid equilibrium conditions considered to control their concentrations. At subcritical conditions, these reactions and equilibrium conditions are well established and include single mineral reactions as well as mineral-pair reactions [41] (Table 4). In order to calculate the individual elemental concentrations from these mineral-fluid equilibria buffers, further knowledge of the reservoir pH is needed. Here, pH conditions for Krafla fluids were adopted from Stefánsson and Arnórsson [47]. Experimental results are compared with calculated equilibrium compositions in Figure 7. Both experimental results and calculated equilibrium compositions showed good agreement between the two demonstrating a mineral-fluid equilibria control on the subcritical fluid compositions.Table 4
Mineral-fluid reactions that describe how aqueous neutral species and ion activity ratios are presumably controlled at subcritical and supercritical conditions.
Buffer reactions
Controlled neutral species and ion activity ratios
Subcritical buffer reactions
qtz+2H2O=H4SiO4
H4SiO4
py+pyrr+2pre+H2O=2epi+3H2S
H2S
4pyrr+2pre+2H2O=2epi+2py+3H2
H2
2czo+2cc+3qtz+2H2O=3pre+2CO2
CO2
1.5pre+2H+=1.5qtz+1.5czo+2H2O+Ca2+
Ca2+/(H+)2
4.5qtz+czo+2Na+=0.5pre+2alb+Ca2+
Ca2+/(Na+)2
alb+K+=mic+Na+
Na+/K+
0.67epi+0.67pyrr+2H+=0.33py+0.67pre+1.5H2O+Fe2+
Fe2+/(H+)2
czo+2H2O+OH−=pre+AlOH4-
Al(OH)4-/OH-
chl+3wai+5Ca2+=4pre+3qtz+6H2O+5Mg2+
Mg2+/Ca2+
Supercritical reactions
qtz=SiO2g
SiO2(g)
NaCls+nH2O=NaCl·nH2Og
Na (NaCl)
KCls+nH2O=NaCl·nH2Og
K (KCl)
CaCl2s+nH2O=CaCl2·nH2Og
Ca (CaCl2)
MgCl2s+nH2O=CaCl2·nH2Og
Mg (MgCl2)
Cl (sum of MClx(g) species)Figure 7
The concentration of subcritical and supercritical geothermal fluids observed in the experiments and at Krafla, Iceland [31, 41]. Also shown are predicted equilibrium concentrations assuming mineral-fluid equilibria at subcritical conditions [41, 47] as well as quartz and salt equilibrium solubility concentrations in supercritical water [44–46].At supercritical conditions, it is less certain what processes control the fluid composition. Mineral solubilities are poorly known except for quartz and some common salts [44–46], therefore the experimental results are compared with the calculated solubility of quartz (SiO2) and simple salts (NaCl, KCl, and CaCl2), shown in Figure 7. Excellent agreement was observed for silica, suggesting that equilibrium between quartz and the supercritical fluid controls Si concentration in the fluid. In the case of other mineral-forming elements, concentrations obtained in the experiments were similar to or somehow higher to the calculated equilibrium concentrations of the salts. The elemental concentrations of these salts in the supercritical fluids may be influenced by a combination of different mineral solubilities including salts, oxides, and aluminum silicates. In contrast, the concentration of volatile elements like B, C, and S (Figure 8) remained unchanged in the fluid from subcritical to supercritical conditions, which is in agreement with previous geochemical modeling calculations [31].Figure 8
Concentrations of B, CO2, and H2S in the subcritical to supercritical fluids. Experimental results, concentrations in subcritical geothermal reservoir fluids at Krafla and the IDDP-1 fluid discharge composition [31, 41], and concentration trends predicted by previous geochemical modeling calculations [31].


### 4.3. Comparison of Experimental and Modeling Results with IDDP-1 Fluids

Experimental conductive boiling of a subcritical geothermal fluid to form supercritical fluid decreased mineral-forming element concentrations, whereas concentrations of volatile components remained mostly unchanged. Similar trends were observed in the elemental concentrations measured in the IDDP-1 supercritical fluid discharge when compared to subcritical fluids at Krafla (Table5). However, direct comparison of experimental and IDDP-1 fluids shows that most concentrations of mineral-forming elements (Si, Na, K, and Ca) fall into a similar range, whereas Cl and volatile (CO2, H2S) concentrations differed significantly (Table 5). Concentrations of Cl at laboratory conditions were considerably lower than concentrations observed in the IDDP-1 discharge. Low concentrations of Cl in experimental fluids were caused by precipitation of minor amounts of salts (e.g., halite) in the very late stage of the boiling process. High concentrations of Cl and other volatile elements such as C and S in the IDDP-1 fluids could be attributed to minor magmatic degassing [48–50]. The experimental results thus support previous findings that supercritical IDDP-1 fluids likely form by conductive heating of subcritical geothermal reservoir fluids of meteoric water origin with minor input of magmatic gases [31, 48, 50]. Our experiments, in combination with geochemical modeling [31], revealed that varying the initial concentrations of volatile elements (C, S, and B) in the reservoir geothermal fluid does not affect the chemical composition of the supercritical fluid nor the alteration mineralogy, due to early partitioning of volatile elements into the vapor (Figure 8).Table 5
Comparison of measured and modeled geothermal fluids at Krafla. Concentrations are in ppm.
Subcritical fluid
Supercritical fluid
Experimenta
Kraflab
Experiment w37a
Experiment w17a
IDDP-1c
Modelc
t (°C)
260
295
420
400
440
SiO2
453±121
659
2.4±1.4
2.9±1.3
6.0
3.2
B
3.41±0.05
1.23
3.30±0.46
1.39±0.06
1.41
1.39
Na
181±18
178
0.13±0.04
0.99±0.46
0.51
168
K
21.1±9.1
40.9
0.04±0.02
0.23±0.04
0.12
31.8
Ca
1.91±0.76
1.18
0.04±0.03
0.10±0.05
0.16
0.0002
Mg
0.009±0.013
0.001
0.003±0.001
0.026±0.008
0.024
0.000001
Fe
0.044±0.036
0.036
0.04±0.01
0.12±0.06
5.25
0.004
Al
6.20±0.79
1.27
0.04±0.02
0.08±0.04
0.054
0.001
Cl
44.8±1.6
112
0.41±0.06
1.99±0.44
105
109
CO2
76.9±12.5
858
87±104
60.5±34.2
1637
1628
SO4
157±29
127
0.37±0.07
0.84±0.57
32.7
4.13
H2S
37.3±9.6
266
13.9±6.5
25.1±10.2
630
395
aAn average from the experimental runs (Table 3). bFrom Kaasalainen and Stefánsson [64]. cFrom Heřmanská et al. [31].


### 4.4. Mechanism of Boiling in Cracks and Implications for Exploitation of Supercritical Resources

Our experiments suggest that quartz and other silicates such as feldspar and wollastonite are the dominant secondary mineral phases that precipitate upon conductive boiling of subcritical fluids to form supercritical fluids. Boiling of 1 kg of subcritical fluids from Krafla has been modeled to produce ~50 cm3 of silica [31], and using such results, the time required for complete closure of cracks by secondary mineral formation can be calculated (Figure 9). The permeability in volcanic geothermal systems like Krafla has been shown to range typically from 10-14 to 10-16 m2, which can be equated to a single crack with a width of up to 0.05 mm cutting each cubic meter in the system [51–53]. Based on an average fluid mass flux of 10-5 kg m-2 s-1 [54], conductive boiling of a subcritical fluid to supercritical conditions could lead to the complete closure of a 0.01 to 0.05 mm wide crack over a time period as short as a few hours or as long as ~140 years (Figure 9). These calculated time scales are in line with previous findings on permeability reduction in geothermal systems [25, 30, 32, 55–58]. However, the calculations should be considered as a simplification of real conditions. Mineral deposition was assumed to be immediate and independent of fluid flow, and possible reduced fluid flow upon decreased permeability associated with the mineral deposition was not considered. Formation of supercritical fluids may thus contribute to silica deposits, for example, as observed at the IDDP-1 well orifices [16]. However, such scaling will not occur during the supercritical fluid condensation as supercritical fluids exhibit low concentrations in mineral-forming elements (Figure 7).Figure 9
Mechanism of conductive boiling of subcritical fluids in cracks near the brittle-ductile transition (BDT). (a) Conductive boiling of a subcritical fluid to supercritical conditions along a single crack. (b) Volumes of secondary minerals (from Heřmanská et al. [31]) formed upon conductive boiling as a function of specific enthalpy along a crack. (c) Time for closure of a crack with a width of 0.05 mm as a function of specific enthalpy and fluid mass flux. Values for the range of fluid mass flux are taken from Norton and Knight [54]. (d) Time for closure of a crack with variable width based on permeability values of Norton and Knapp [53], Lamur et al. [51], and Watanabe et al., [52] using an average fluid mass flux of 10-5 kg m-2 s-1 [54]. Closure of the crack accelerates as soon as quartz starts to precipitate.


## 4.1. Geochemistry of Subcritical Geothermal Fluids

Studies of alteration mineralogy and fluid composition in geothermal systems show that equilibrium is closely approached between the geothermal fluids and secondary minerals formed in the systems, except for mobile elements such as Cl [35–39]. At Krafla, the most common secondary minerals identified include calcite, quartz, epidote, various clays, chlorite, feldspars, and pyrite. Anhydrite, prehnite, actinolite, wollastonite, garnet, pyrrhotite, and various zeolites, including wairakite, have also been observed [40]. Previous studies on mineral-fluid interaction at Krafla have demonstrated that the major fluid components were in equilibrium with these minerals, which in turn control the fluid composition at depth (Figure 5) [41].Figure 5
Mineral saturation state of selected minerals at subcritical conditions. The reaction quotients were calculated using the Phreeqc program [61] and the llnl.dat database. Also shown are mineral solubilities and the mineral reaction quotients for reservoir fluids at Krafla at the measured reservoir temperatures, both obtained from Gudmundsson and Arnórsson [41].Our experimental results indicate a similar process of mineral-fluid interaction at subcritical temperatures, with formation of secondary minerals upon interaction of geothermal water with the primary basaltic rock and glass. The calculated saturation indices with respect to commonly observed secondary minerals revealed near-equilibrium between the fluids and quartz, whereas supersaturation occurs with respect to calcite, chlorite, feldspars, wollastonite, and zeolites (Figure5). Supersaturation may have resulted from high initial concentrations in the inlet experimental solutions relative to the equilibrium composition at 260°C and experimental durations of hours, compared to residence times of fluids in natural geothermal systems like at Krafla that are in the order of months to years [42, 43]. We conclude that the chemical composition of geothermal fluids at subcritical temperatures is controlled by near-equilibrium with secondary minerals. This agrees with previous findings [35–39, 41].


## 4.2. Supercritical Fluid Formation, Fluid-Rock Interaction, and Control of Elemental Transport

The solubility of mineral-forming elements and salts including Si, Ca, K, Na, and Cl is orders of magnitude lower in supercritical fluids compared to subcritical fluids and has been observed to decrease with decreasing fluid density [44–46]. Indeed, a recent modeling study of the formation of supercritical fluid by conductive boiling of subcritical fluids revealed that the process is expected to result in mineral deposition dominated by silica, aluminum silicates, and salts around the heat source [31]. In contrast, volatile elements like B, CO2, and H2S are expected to partition into the vapor phase upon boiling, resulting in insignificant concentration changes in the total fluid.Elemental behavior upon conductive heating of subcritical liquid water to form supercritical fluid may be demonstrated from the elemental relative mobilities (RM), given by the elemental concentration (mi) ratio between the inlet and outlet solution relative to a mobile element like B:
(1)RM=mi/mBoutletmi/mBinlet.The results demonstrate that volatile elements separate from the major rock-forming elements upon boiling of subcritical fluids to supercritical temperatures (Figure6). Boron, CO2, and H2S partition into the vapor phase, whereas nonvolatile elements like Si, Ca, Na, K, Al, Cl, and SO4 are precipitated into the observed secondary minerals, mainly silica, aluminum silicates, and chlorides. Chloride may also precipitate into salts like halite and sylvite (Figure 4). In this way, <1-10% of these elements are quantitatively removed from the initial concentration of the subcritical fluids.Figure 6
Relative mobility of major elements upon boiling of subcritical geothermal fluids by conductive heating to form supercritical fluids. Elements showing relative mobility close to 1 may be regarded as mobile, whereas elements with relative mobility of <0.1 are immobile.The elemental concentrations can be further compared with the mineral-fluid equilibrium conditions considered to control their concentrations. At subcritical conditions, these reactions and equilibrium conditions are well established and include single mineral reactions as well as mineral-pair reactions [41] (Table 4). In order to calculate the individual elemental concentrations from these mineral-fluid equilibria buffers, further knowledge of the reservoir pH is needed. Here, pH conditions for Krafla fluids were adopted from Stefánsson and Arnórsson [47]. Experimental results are compared with calculated equilibrium compositions in Figure 7. Both experimental results and calculated equilibrium compositions showed good agreement between the two demonstrating a mineral-fluid equilibria control on the subcritical fluid compositions.Table 4
Mineral-fluid reactions that describe how aqueous neutral species and ion activity ratios are presumably controlled at subcritical and supercritical conditions.
Buffer reactions
Controlled neutral species and ion activity ratios
Subcritical buffer reactions
qtz+2H2O=H4SiO4
H4SiO4
py+pyrr+2pre+H2O=2epi+3H2S
H2S
4pyrr+2pre+2H2O=2epi+2py+3H2
H2
2czo+2cc+3qtz+2H2O=3pre+2CO2
CO2
1.5pre+2H+=1.5qtz+1.5czo+2H2O+Ca2+
Ca2+/(H+)2
4.5qtz+czo+2Na+=0.5pre+2alb+Ca2+
Ca2+/(Na+)2
alb+K+=mic+Na+
Na+/K+
0.67epi+0.67pyrr+2H+=0.33py+0.67pre+1.5H2O+Fe2+
Fe2+/(H+)2
czo+2H2O+OH−=pre+AlOH4-
Al(OH)4-/OH-
chl+3wai+5Ca2+=4pre+3qtz+6H2O+5Mg2+
Mg2+/Ca2+
Supercritical reactions
qtz=SiO2g
SiO2(g)
NaCls+nH2O=NaCl·nH2Og
Na (NaCl)
KCls+nH2O=NaCl·nH2Og
K (KCl)
CaCl2s+nH2O=CaCl2·nH2Og
Ca (CaCl2)
MgCl2s+nH2O=CaCl2·nH2Og
Mg (MgCl2)
Cl (sum of MClx(g) species)Figure 7
The concentration of subcritical and supercritical geothermal fluids observed in the experiments and at Krafla, Iceland [31, 41]. Also shown are predicted equilibrium concentrations assuming mineral-fluid equilibria at subcritical conditions [41, 47] as well as quartz and salt equilibrium solubility concentrations in supercritical water [44–46].At supercritical conditions, it is less certain what processes control the fluid composition. Mineral solubilities are poorly known except for quartz and some common salts [44–46], therefore the experimental results are compared with the calculated solubility of quartz (SiO2) and simple salts (NaCl, KCl, and CaCl2), shown in Figure 7. Excellent agreement was observed for silica, suggesting that equilibrium between quartz and the supercritical fluid controls Si concentration in the fluid. In the case of other mineral-forming elements, concentrations obtained in the experiments were similar to or somehow higher to the calculated equilibrium concentrations of the salts. The elemental concentrations of these salts in the supercritical fluids may be influenced by a combination of different mineral solubilities including salts, oxides, and aluminum silicates. In contrast, the concentration of volatile elements like B, C, and S (Figure 8) remained unchanged in the fluid from subcritical to supercritical conditions, which is in agreement with previous geochemical modeling calculations [31].Figure 8
Concentrations of B, CO2, and H2S in the subcritical to supercritical fluids. Experimental results, concentrations in subcritical geothermal reservoir fluids at Krafla and the IDDP-1 fluid discharge composition [31, 41], and concentration trends predicted by previous geochemical modeling calculations [31].


## 4.3. Comparison of Experimental and Modeling Results with IDDP-1 Fluids

Experimental conductive boiling of a subcritical geothermal fluid to form supercritical fluid decreased mineral-forming element concentrations, whereas concentrations of volatile components remained mostly unchanged. Similar trends were observed in the elemental concentrations measured in the IDDP-1 supercritical fluid discharge when compared to subcritical fluids at Krafla (Table5). However, direct comparison of experimental and IDDP-1 fluids shows that most concentrations of mineral-forming elements (Si, Na, K, and Ca) fall into a similar range, whereas Cl and volatile (CO2, H2S) concentrations differed significantly (Table 5). Concentrations of Cl at laboratory conditions were considerably lower than concentrations observed in the IDDP-1 discharge. Low concentrations of Cl in experimental fluids were caused by precipitation of minor amounts of salts (e.g., halite) in the very late stage of the boiling process. High concentrations of Cl and other volatile elements such as C and S in the IDDP-1 fluids could be attributed to minor magmatic degassing [48–50]. The experimental results thus support previous findings that supercritical IDDP-1 fluids likely form by conductive heating of subcritical geothermal reservoir fluids of meteoric water origin with minor input of magmatic gases [31, 48, 50]. Our experiments, in combination with geochemical modeling [31], revealed that varying the initial concentrations of volatile elements (C, S, and B) in the reservoir geothermal fluid does not affect the chemical composition of the supercritical fluid nor the alteration mineralogy, due to early partitioning of volatile elements into the vapor (Figure 8).Table 5
Comparison of measured and modeled geothermal fluids at Krafla. Concentrations are in ppm.
Subcritical fluid
Supercritical fluid
Experimenta
Kraflab
Experiment w37a
Experiment w17a
IDDP-1c
Modelc
t (°C)
260
295
420
400
440
SiO2
453±121
659
2.4±1.4
2.9±1.3
6.0
3.2
B
3.41±0.05
1.23
3.30±0.46
1.39±0.06
1.41
1.39
Na
181±18
178
0.13±0.04
0.99±0.46
0.51
168
K
21.1±9.1
40.9
0.04±0.02
0.23±0.04
0.12
31.8
Ca
1.91±0.76
1.18
0.04±0.03
0.10±0.05
0.16
0.0002
Mg
0.009±0.013
0.001
0.003±0.001
0.026±0.008
0.024
0.000001
Fe
0.044±0.036
0.036
0.04±0.01
0.12±0.06
5.25
0.004
Al
6.20±0.79
1.27
0.04±0.02
0.08±0.04
0.054
0.001
Cl
44.8±1.6
112
0.41±0.06
1.99±0.44
105
109
CO2
76.9±12.5
858
87±104
60.5±34.2
1637
1628
SO4
157±29
127
0.37±0.07
0.84±0.57
32.7
4.13
H2S
37.3±9.6
266
13.9±6.5
25.1±10.2
630
395
aAn average from the experimental runs (Table 3). bFrom Kaasalainen and Stefánsson [64]. cFrom Heřmanská et al. [31].


## 4.4. Mechanism of Boiling in Cracks and Implications for Exploitation of Supercritical Resources

Our experiments suggest that quartz and other silicates such as feldspar and wollastonite are the dominant secondary mineral phases that precipitate upon conductive boiling of subcritical fluids to form supercritical fluids. Boiling of 1 kg of subcritical fluids from Krafla has been modeled to produce ~50 cm3 of silica [31], and using such results, the time required for complete closure of cracks by secondary mineral formation can be calculated (Figure 9). The permeability in volcanic geothermal systems like Krafla has been shown to range typically from 10-14 to 10-16 m2, which can be equated to a single crack with a width of up to 0.05 mm cutting each cubic meter in the system [51–53]. Based on an average fluid mass flux of 10-5 kg m-2 s-1 [54], conductive boiling of a subcritical fluid to supercritical conditions could lead to the complete closure of a 0.01 to 0.05 mm wide crack over a time period as short as a few hours or as long as ~140 years (Figure 9). These calculated time scales are in line with previous findings on permeability reduction in geothermal systems [25, 30, 32, 55–58]. However, the calculations should be considered as a simplification of real conditions. Mineral deposition was assumed to be immediate and independent of fluid flow, and possible reduced fluid flow upon decreased permeability associated with the mineral deposition was not considered. Formation of supercritical fluids may thus contribute to silica deposits, for example, as observed at the IDDP-1 well orifices [16]. However, such scaling will not occur during the supercritical fluid condensation as supercritical fluids exhibit low concentrations in mineral-forming elements (Figure 7).Figure 9
Mechanism of conductive boiling of subcritical fluids in cracks near the brittle-ductile transition (BDT). (a) Conductive boiling of a subcritical fluid to supercritical conditions along a single crack. (b) Volumes of secondary minerals (from Heřmanská et al. [31]) formed upon conductive boiling as a function of specific enthalpy along a crack. (c) Time for closure of a crack with a width of 0.05 mm as a function of specific enthalpy and fluid mass flux. Values for the range of fluid mass flux are taken from Norton and Knight [54]. (d) Time for closure of a crack with variable width based on permeability values of Norton and Knapp [53], Lamur et al. [51], and Watanabe et al., [52] using an average fluid mass flux of 10-5 kg m-2 s-1 [54]. Closure of the crack accelerates as soon as quartz starts to precipitate.


## 5. Conclusions

The chemical and mineralogical changes associated with supercritical fluid formation by conductive heating and boiling of subcritical geothermal fluids were studied experimentally. Our results showed that the chemical composition of geothermal fluids at subcritical temperatures is controlled by near-equilibrium between the geothermal fluids and secondary minerals, except for mobile elements like Cl, which is in line with previous studies [35–39]. Upon conductive heating and boiling of such fluids to form supercritical fluids having a temperature >400°C, rock-forming elements like Si, Na, K, Ca, Mg, and Cl are quantitatively deposited into silicate, aluminum silicate, and salt deposits. In contrast, volatile element concentrations like CO2, H2S, and B remained unchanged. The observed concentrations of the nonvolatile elements are similar to those predicted from the solubility of quartz (SiO2) and salts (NaCl, KCl, and CaCl2) suggesting that reactions between these solids and the fluid influence and even control the elemental concentrations in the supercritical fluid. Similar concentration trends were observed for the IDDP-1 supercritical and subcritical geothermal fluids at Krafla, Iceland, and have been predicted from geochemical modeling [31]. The experimental results further support findings that the supercritical IDDP-1 fluids likely form by conductive heating of subcritical geothermal fluids of meteoric origin, with minor input of magmatic gases [31, 48, 50]. Such fluids may be suitable for power production.



---

*Source: 6023534-2019-08-05.xml*