1 Introduction

Despite recent emergence of natural gas, nuclear, solar, and wind power, coal remains an important energy source to the United States and the world. For example, in 2018, 27.4% of the United States energy demand was met by burning coal, while for the world the number was even higher, about 40%. According to proven reserves, the world has about 150 years’ worth of energy from coal combustion, but only 50 years’ worth of energy from oil or natural gas. Furthermore, the United States owns 28% of the world’s coal reserves compared to only 2.3% of the world’s oil reserves. Despite this reserve of coal, the production of coal has been decreasing since 2013 due to the rise of natural gas combined cycle generators, fracking, and concerns over atmospheric and local air pollution. (EIA International Energy Outlook 2017, 2018).

Raw coal contains a high percentage (about 80 wt%) of carbon which is combusted to produce CO2 and heat in the power plant; but it also contains harmful components such as sulfur, chlorine, mercury, and heavy metals. When combusted, the harmful components accumulate as bottom ash in the boiler or are swept away in flue gas as fly-ash particles and/or noxious gases. Bottom ash can present problems for combustion due to slagging and also pose safe disposal problems. Stringent air quality standards set by the EPA and MATS compliance have placed restrictions on the particulates, sulfur, and NOx emissions of coal fired power plants due to the realization that serious local and global health concerns can arise from their unabated release. Particulate matter is separated from flue gas using electrostatic filters. Limiting NOx production is achieved by looping of reaction gases and effective flame control. The three types of sulfur present in coal-organic, pyritic, and sulfides are oxidized to form sulfur dioxide which is toxic to humans if released to the atmosphere and corrosive to plant equipment. Emission of other highly active molecules, such as chlorine and mercury, also contributes to deterioration of the atmospheric environment. Wet flue gas desulphurization (WFGD) units have become the industry standard to limit the sulfur dioxide emissions, with state of the art installations capturing 90%–95% of sulfur and a variable amount of chlorine and mercury. In WFGD, flue gas is passed through concentrated aqueous lime solutions that adsorb SOx vapors. The resultant slurry can be used to form calcium sulfate dehydrate (i.e., gypsum) but will mostly accumulate as solid waste as elemental sulfur or calcium sulfate. Separating particulates and sulfur from flue gas requires the processing of large volumes of flue gas and leads to a significant thermal load on the plants. Treatment of waste in air, water, and solids is a concerning issue that has large impacts and costs that are hard to calculate. Improper solid and liquid waste management can lead to failures in the short term requiring remediation efforts, but the continued air pollution has become a top international concern for the long term. The future of allowable and untaxable air pollution is unclear. Thus, current combustion of raw coal leads to a plethora of issues concerning environmental safety, materials handling, and combustion efficiency.

Pre-combustion extractions of raw coal have been an intensive area of research for some time with a few promising methods for removing all of the sulfur and ash content reported recently, as summarized in Table 1. The beneficiation methods are classified as biological, physical, or chemical. Beneficiation using microbes is slow, costly, and difficult to maintain or scale up. While physical remediation of coal is not suitable for chemically bonded minerals and requires energy intensive grinding, industrial implementations of physical coal cleaning methods can be found because of their ease of scalability.

Table 1 Current sulfur removal technologies for coal beneficiation
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Chemical beneficiation of raw coal is considered as the most promising method to effectively remove all sulfur forms. Acids and alkaline solutions can be used sequentially and in various mixtures to produce coal with both low ash and low sulfur. Some commercial ash-free coal methods requiring heated oil as solvent may exist, but the process is not economically feasible. Most of these extraction schemes are inspired from high-value materials; unfortunately, coal is a low-value commodity and these methods which call for even dilute acids and microwave radiation cannot be performed economically on an industrial scale. In addition, the residual acids and caustics in the coal, even in small amounts, will be combusted upon use, which creates new environmental challenges. Furthermore, the hydrocarbon bonds should not be broken down so as to retain heating value. While hydrothermal extractions have been used for clean coal, they usually decrease the heating value by a considerable amount due to organic dissolution and fractionation into gas and liquid phase (Timpe et al. 2001). Recently, a research group did show that carbonic acid could be used to enhance aqueous extraction of coal by bubbling CO2 through stagnant hot water, but the experimental temperatures and pressures were very mild (Gao et al. 2017; Ding et al. 2019).

Inspired by previous successful extraction efforts but keeping in mind the necessary thermo-economic restrictions for scale up on coal, we propose an extraction using supercritical mixtures of water and carbon dioxide. The mixture will form in situ carbonic acid capable of leaching heteroatoms from coal but also will be finely tunable to prevent loss of hydrocarbon heating value. Also, supercritical extractions have the benefit of simple separation upon completion of extraction using fractionation at decreasing pressures. Power plants would be able to use carbon dioxide generated from combustion, otherwise emitted, and use waste heat to perform economical and environmentally protective extractions on raw coal. Because sulfur comprises the majority of hazardous aerosolized pollutants by mass, sulfur is studied as a model heteroatom before and after extraction in this work.

1.1 Supercritical fluid extraction

Supercritical fluid extractions have several benefits including enhanced mass transport, ease of separation and recycle, wide range of extractive capability and tunability, and better inherent safety. A fluid is supercritical when it is compressed beyond its critical pressure and heated beyond its critical temperature, and the fluid density can be adjusted by changing pressure and temperature. The diffusivity of the supercritical fluids is higher than that of liquid solvents, and can be easily varied. For typical conditions, diffusivity in supercritical fluids is of the order of 10−3 cm2/s as compared to 10−1 for gases and 10−5 for liquids. The viscosity of typical supercritical fluids is of the order of 10−4 g/(cm s) which is similar to that of gases and about 100 fold lower than that of liquids. The combination of the high diffusivity and low viscosity provide rapid equilibration of the fluid to the mixture to be extracted, hence extraction can be reached close to the thermodynamic limits. In addition, the supercritical temperature can be manipulated by changing the pressure, which can be done to ensure that the fluid mix is supercritical at the intended extraction temperature.

For many extraction applications in food and pharmaceutical industries, carbon dioxide is the supercritical fluid of choice because it is non-flammable, non-toxic, inexpensive, and has mild critical temperature (31.1 °C and 74 bar). Hence, much of the attention has been given to supercritical carbon dioxide for practical extraction applications. However, scCO2 is too mild for extraction of hard minerals from materials such as coal.

One the other hand, water is supercritical at > 374 °C temperature and > 221 bar pressure. Supercritical water has liquid-like density and gas-like transport properties, and behaves very differently than it does at room temperature. For example, it is highly non-polar, permitting complete solubilization of the most organic compounds and gases. The resulting single-phase mixture does not have many of the conventional transport limitations that are encountered in multi-phase reactors. The physiochemical properties of water, such as viscosity, ion product, density, and heat capacity, also change dramatically in the supercritical region with only a small change in the temperature or pressure, resulting in a substantial increase in the rates of chemical reactions (Gupta 2005). For example, Fig. 1 shows how density, dielectric constant and ionic product of water vary with temperature at 240 bar.

Fig. 1
figure 1

Physical properties of water versus temperature, at 240 bar. Dielectric constants of typical organic solvents at room temperature are also indicated (Kritzer and Dinjus 2001)

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From Fig. 1, it is interesting to see that the dielectric behavior of 200 °C water is similar to that of ambient methanol, 300 °C water is similar to ambient acetone, 370 °C water is similar to methylene chloride, and 500 °C water is similar to ambient hexane (Gupta 2005). Hence, for our application of coal beneficiation, subcritical conditions (e.g., 300 °C) may provide a conducive solvent atmosphere where various ionic species are effectively solubilized in the fluid and removed.

1.2 Combination of supercritical water and carbon dioxide (ScWC)

The CO2–H2O ratio can be used to fine-tune the extraction efficiency. Ionization provided by the formed carbonic acid along with the high thermal energy can cause reaction of the inorganic content, and the products are then solubilized and efficiently carried away by the high density of the fluid. As shown in Fig. 2, the CO2–H2O ratio can also be used to tune the critical point of the mixture. With increasing pressure and carbon dioxide mass percent, the critical temperature of the mixture decreases from 623 K at 15% carbon dioxide concentration and low pressure to about 545 K at carbon dioxide concentration above 35% and pressure above 100 MPa. Dew point and bubble point lines indicate that carbon dioxide and water will be well miscible and soluble at temperatures above 530 K.

Fig. 2
figure 2

Pressure-mole fraction phase diagram of the CO2–H2O system at temperatures of 423–623 K and pressures up to 200 MPa. The isotherms on the left of the critical line stand for the bubble point lines of CO2 saturated water, and the isotherms on the right of the critical line stand are dew point lines of the H2O saturated supercritical CO2. (Zhao and Lvov 2016)

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2 Experimental work

2.1 Materials

Supercritical fluid grade CO2 and deionized water and their mixtures were used as extraction fluids. The pulverized bituminous coal with particle size 250–1250 micron was obtained from Rosebud Mining Company (Kittanning, PA) identified as Clymer Blend CPA#101315. Nanopure filtered water was used for all testing. High purity SFE grade CO2 tank with dip tube was provided by Airgas. Coal standard 2683c was acquired from NIST. For analytical work, 70% environmental grade nitric acid from GFS Chemicals was used for ICP-OES. Boric acid was purchased from the American Borate Company, and pure sodium sulfate and sodium hydroxide were purchased from Sigma Aldrich.

2.2 Analytical techniques

For elemental analysis of solids, Inductively Coupled Plasma Mass Spectroscopy of coal pellets was performed on an Agilent ICP-MS. A 1550 W laser (8 J/cm2) would be focused on the pellet and used to ablate and ionize the pellet surface at low pressure in the presence of plasma gas. Ions are swept by nebulizer gas into the spectroscopy unit and produce counts for each element. A laser spot size of 75 microns was used to ablate 5 mm of pellet to 7.0 mm depth while rastering at 75 micron/s. Line length could be adjusted to obtain an appropriate number of counts to build calibration curves. The experimental error in the sulfur analysis is expected to be 5%.

For validation and additional testing, samples were also sent to Standard Laboratories, Inc. (South Charleston, WV) for analysis specialized to coal samples.

A Hitachi SU-70 FE-SEM was used to obtain images and EDS spectra. Raman shift and XRD and BET were used as well to understand physical and chemical changes to the carbon structure.

2.3 Coal extraction apparatus

A semi-continuous coal extractor was designed and built as shown in Fig. 3, in which coal powder is packed in the extraction vessel and the extraction fluid is pumped continuously.

Fig. 3
figure 3

Schematic of the semi-continuous supercritical H2O–CO2 (ScWC) extraction of coal

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A high-pressure hydrothermal reactor (model XHTC400 USP-1200) from Columbia International was used as a flow vessel to extract coal solids. The vessel volume is 250 mL and material of construction is S316 stainless steel. The vessel itself is rated to a maximum continuous working temperature of 400 °C, maximum temperature of 450 °C, and a maximum working pressure of 200 bar. A Supercritical 24 constant flow/constant pressure dual-piston pump was used to pressurize the vessel with CO2. An Eldex 1SMP pump (0-5 mL/min, < 200 bar) was used to pump water. The two streams meet at a tee joint that immediately feeds to a check valve at the vessel inlet. The vessel was heated with a Rama 1000 W heating band controlled by a temperature controller. A Swagelok KPB1P0A422P20000 backpressure regulator was used to control the pressure of the outlet. Gas exiting from the regulator was fed to room temperature separator to allow aqueous suspension leachate to separate from gaseous CO2.

In a typical extraction, the cooling/chilling unit on the Supercritical 24 pump were turned on and allowed to cool for 20 min. The vessel was loaded with about 10–50 g of pulverized coal and covered with porous glass wool to suppress carryover of the coal particles by the extraction fluid. The vessel was tightened and the backpressure regulator left slightly open. If the extraction called for water, the Eldex pump would be then be primed, turned off, and connected to the vessel inlet. The CO2 tank was then opened and the pump turned on. The regulator was then closed all the way and checked for zero outlet flow. The vessel was allowed to fully pressurize to 153 bar with only CO2 over the course of about 25 min at which point the backpressure regulator was opened and a steady flow established. The temperature controller was then turned on and set to 75 °C. If the extraction called for water, the Eldex pump would also be turned on. Once the vessel reached about 50 °C, the setpoint was increased to 175 °C and then again to desired set point. Heating to desired set temperature would take about 25 min. Extraction time is then considered to be time zero once the vessel has reached the desired temperature. Upon completion of an extraction, both pumps and the heating would be turned off and the CO2 tank closed. The regulator was loosened to completely depressurize the vessel and then closed to allow the evacuated vessel to cool overnight. Usually, the vessel temperature would increase past reaction temperature at the beginning of cooling as incoming fluid was shut off and no longer provided a heat duty. Coal solids were weighed before and after extraction. Other than solids embedded in the glass wool used a filter, total coal mass did not seem to change during extraction. Liquid and solid samples would be collected the next day and stored for analysis.

Typical temperature and pressure profiles of the reactor versus time are shown in the Fig. 4.

Fig. 4
figure 4

Temperature (a) and pressure (b) profiles for a typical experiment. Data for experiment E102219 for which the extraction is considered to start at 143 min timescale

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Extracted and raw coals were dried at 80 °C in a vacuum oven for 12 h. The entire portion would then be ground with a mortar and pestle and mixed together. A roughly 100 mg portion of that coal mixture would then be dried in a vacuum oven at 80 °C and − 100 psi/g for two hours to ensure moisture removal. Approximately 32 mg coal and 593 mg boric acid were then weighed, mixed, and ground together with a high-energy ball mill. An 11 mm die was used to press pellets at 3 tons of applied force for 2 min. Pellets were fashioned with various amounts of a NIST coal standard (sulfur, 2 wt%) in order to create a calibration curve. The pellets were then taken for sulfur analysis using ICP-MS with laser ablation.

3 Results and discussion

3.1 Results

The coal feedstock was analyzed independently by Standard Laboratories using prescribed ASTM methods. The analysis is shown in the Table 2. It showed a 1.14 wt% sulfur content using ASTM D2492. Our in-house ICP-MS analysis gave a similar sulfur content of 1.15 wt%, but due to high variation, the coal was mixed more thoroughly and a raw value of 1.37 wt% was obtained thereafter.

Table 2 Analysis of the feedstock coal
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A total of 17 extraction runs were carried out using the above bituminous coal at a constant pressure of 143 bar with varying extraction time, temperature, water flow rate and CO2 flow rate, as shown in Table 3. The sulfur content was tracked by ICP-MS analysis in the extracted coal as a measure of extraction effectiveness. Standard Labs results are also presented when available.

Table 3 Master list of coal extraction experiments conducted
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Experiments were performed at various temperatures with CO2 flow, H2O flow (hydrothermal), and combined flow (ScWC) in order to asses the effectiveness of supercritical carbon dioxide as solvent and to compare combined flow extraction to more typical hydrothermal extractions. Because fluid characteristics can vary complexly with CO2–H2O ratio, a variety of temperatures were explored ranging from 200 to 400  °C, and sulfur remaining was used as a measure of effectiveness. The coal mass was varied slightly as we came to understand the amount needed for analysis but changes are negligible. The fluid path of our vessel does not directly cross through the loaded solids, so it is likely that the solvent to coal ratios are all higher than necessary. Further testing will be need to understand the mass transfer characteristics in a well design flow path. For the same reason, in the present study, the differences in time are not as important as changes in temperature and fluid composition.

Solids recovered after extraction were usually within 2% of the mass loaded after accounting for loss of moisture, except for extractions with pure water at temperatures around 350 °C where about 10% of the mass was lost. The exact masses recovered were difficult to obtain as some coal particles entangle in the glass wool used as filter.

Data in Fig. 5 shows that carbon dioxide, ScWC, and hydrothermal extraction are all similarly capable of extracting 50% sulfur. Extraction with carbon dioxide was most effective at 350 °C, while extraction with water seemed to be most effective around 300 °C where the ionic concentration was highest. As expected, the hydrothermal extraction was more aggressive at lower temperatures than the carbon dioxide, and the mixture was somewhere in between. Combined flow may provide a synergy that increases extraction but more accurate assessment of the raw coal would be necessary. ScWC, or combined flow, does seem to inhibit organic dissolution that would be expected and was seen from strictly hydrothermal extraction. Although a limited testing was done with flowrate, increasing the flowrate of carbon dioxide extraction at 350 °C from 5.82 to 11.64 g/min did result in reducing sulfur content from 0.92 wt% to 0.73 wt%.

Fig. 5
figure 5

Sulfur remaining in coal after extraction using hydrothermal, ScWC, and CO2

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While we studied only a single-step desulfurization reactions, analysis of the sulfur forms indicated that extraction with pure carbon dioxide at 200 °C caused pyritic sulfur to be transformed into sulfates that may be easily washed out with warm water. While raw coal contained only 0.02% sulfate and 0.50% pyritic sulfur, E120218 contained 0.16% sulfate and 0.28% pyritic sulfur.

In the case of the combined and hydrothermal extractions at 395 °C, the powder coal feedstock turned into a porous-fused mass by a process called hydrothermal carbonization (Fig. 6). Opaque yellow product was typical for all successful extractions. BET analysis showed that solid product surface area was low, with surface area of 14 m2/g and average pore radius of 9.9 Å, probably similar to raw coal, which could not be analyzed due to volatile sulfur content. The coal after the extraction at lower temperatures was not fused.

Fig. 6
figure 6

Products from experiment E102219: a coal and b dissolved minerals

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Extracted coal from E102219 was further sent out for proximate analysis to the Standard Laboratories. The results are compared with the coal feedstock in Table 4. The volatile carbon portion of the raw coal, 25%, had decreased to 12.5% with a corresponding increase in fixed carbon for E102219. Samples E102219 and E062519 both had substantially less carbon ablated during ICP-MS than all other samples. ICP-MS sulfur weight percentages are in accordance with Standard Labs traditional pyrolysis results for selected samples.

Table 4 Proximate analysis of the extracted coal from experiment E102219
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To further understand the characteristics of the extracted coal from E102219 experiment, X-ray diffraction and thermo-gravimetric analyses were carried out and the results are compared to raw coal in Fig. 7.

Fig. 7
figure 7

X-ray diffraction analysis a and thermo-gravimetric analysis b of the extracted (E102219) and raw coals

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XRD spectra for coal contain two main peaks for carbon at 2θ of 25° and 26.5°. Raw coal has a more prominent peak at 25° with a smaller peak at 26.5°. For E102219, the higher intensity indicates a more ordered crystalline structure as compared to raw coal. Also, the peak at 26.5° has become larger than the peak at 25°. The 26.5° peak is associated with synthetic graphite, and the peak at 25° can be attributed to carbon that is not graphitic.

Thermogravimetric analysis was carried out in nitrogen atmosphere and shows the difference in volatility between raw and extracted coal. By 800 °C, the raw sample has lost 23.2% of mass, compared to only 7.7% mass for E1022. Although we extracted only to 395 °C, E102219 is considerably less volatile in the range of 400–800 °C.

Raman spectra for raw sample have higher counts and a more angled baseline due to fluorescence of metals contained in the raw coal (Fig. 8). This fluorescence is not noticed in the extracted sample from E102219, which has a nearly flat baseline and lower noise, indicating a lack of fluorescence generating metals. Two characteristic carbon peaks appear at 1350 and 1600 cm−1. With baseline subtracted, the peak heights and ratios are the same. A slight broadening of the peak at 1350 cm−1 is noticeable with two shoulder peaks becoming more prominent.

Fig. 8
figure 8

Raman shift spectra for raw coal and the extracted coal from E102219

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Thus, the extraction with fluid above the supercritical point of pure water (375 °C) caused hydrothermal carbonization which may be useful for further upgrading carbon once the heteroatoms have been extracted at temperatures between 300 and 350 °C. The presence of carbon dioxide during hydrothermal carbonization may cause volatile carbon content to crosslink in the solid instead of being extracted by the solution. From the proximate analysis, E102219 has retained most of its heating value. Removing the sulfur should decrease the heating value slightly, but crosslinking volatile carbon into fixed carbon would increase the heating value. Importantly, the combined extraction seems to crosslink carbons that would be extracted and lost by hydrothermal extraction. A survey of the extractive reactions involved is presented below.

3.2 Extractive reactions involved

Water molecule dissociates to form hydrogen ion and hydroxyl ion that both participate in further extraction reactions. At room temperature, the ions are in small concentration, and the dissociation increased with temperature up to about 300 °C and then it rapidly drops, as shown in Fig. 1 (Kritzer and Dinjus 2001). Thermal energy promotes the diffusion and reaction of the ions with the elements in the coal matrix.

$${\text{H}}_{2} {\text{O }} \to {\text{H}}^{ + } + {\text{OH}}^{ - }$$

Carbon dioxide dissolve in water to form carbonic acid following the reaction below:

$${\text{CO}}_{2} + {\text{H}}_{2} {\text{O}} \to {\text{H}}_{2} {\text{CO}}_{{3}}$$
$${\text{H}}_{2} {\text{CO}}_{{3}} \to {\text{HCO}}_{{3}}^{ - } + {\text{H}}^{ + }$$
$${\text{HCO}}_{{3}}^{- } + {\text{OH}}^{ - } \to {\text{CO}}_{{3}}^{2 - } + {\text{H}}_{2} {\text{O}}$$

Carbonic acid can then reacts to dissolve metals into solution or to form carbonate salts. (M = Ca, Mg, etc.)

$${\text{CO}}_{{3}}^{2 - } + {\text{M}}^{2 + }_{{\left( {\text{mineral}} \right)}} \to {\text{MCO}}_{{3 \, \left( {\text{s}} \right)}}$$
$${\text{MCO}}_{{3 \, \left( {\text{s}} \right)}} + {\text{ H}}_{2} {\text{CO}}_{{3}} \rightleftharpoons {\text{M}}^{2 + }_{{\left( {\text{aq}} \right)}} + \, 2{\text{HCO}}_{{3}}^{ - }$$
$${\text{MCO}}_{{3 \, \left( {\text{s}} \right)}} + {\text{ heat}} \to {\text{ MO}} + \text{CO}_2$$

The CO2–H2O mixture is acidic which will help to break down complex mineral structure and provide access to metal ions. Many complex reactions have been hypothesized regarding the specific forms of sulfur. Although this paper does not attempt to study these reactions, a comprehensive analysis of the reaction network can further help understand the molecular mechanism involved so that a rational design for industrial level extraction plants can be made.

For pyrite, iron and sulfur can react with various forms of hydrogen, carbonate, and oxygen ions to ultimately form iron, iron sulfates, sulfur dioxide, and hydrogen sulfide. Pyrite can also be converted into sulfate. Reactive sulfur species COS may also be formed, via a network of reactions as

$${\text{FeS}} +\text{H}_2\text{CO}_3 \to {\text{FeCO}_3} + {\text{H}}_{2} {\text{S}}$$
$${\text{SO}}_{2} + {\text{H}}_{2} {\text{O}} \rightleftharpoons {\text{H}}_{2} {\text{SO}}_{3}$$
$${\text{SO}}_{2} + 2{\text{H}}_{2} {\text{O}} \rightleftharpoons {\text{H}}_{2} + {\text{H}}_{2} {\text{SO}}_{4}$$
$$4{\text{SO}}_{2} + 4{\text{H}}_{2} {\text{O}} \rightleftharpoons 3{\text{H}}_{2} {\text{SO}}_{4} + {\text{H}}_{2} {\text{S}}$$
$${\text{H}}_{2} {\text{S}} + {\text{CO}} \to {\text{COS}} + {\text{H}}_{2}$$
$${\text{H}}_{2} {\text{S}} + {\text{CO}}_{2} \to {\text{COS}} + {\text{H}}_{2} {\text{O}}$$

Organic sulfur is found in coal as mercaptans (RSH), disulfides (RS-S-R’), sulfides (R-S-R’), and thiophenes (heterocyclic). Organic sulfur is thus integrated into the carbon structure and difficult to remove. Oxidative ions convert organic sulfur to sulfates which can be dissolved in water or form sulfur dioxide.

$${\text{RSH}} + {\text{H}_2}{\text{O}} \to {\text{ROH}} + {\text{ H}}_{2} {\text{S}}$$
$${\text{RSH }} + {\text{CO}}_{2} \to {\text{ROH}} + {\text{COS}}$$

Interaction of fluid with the coal may also cause lower organics to liquify or gasify to produce carbon dioxide, hydrogen gas, or methane. More complex studies of the reactions involved can be found in other recent studies (Morimoto et al. 2008; Tian et al. 2016; Zhang et al. 2018).

3.3 Industrial application

The proposed supercritical water-carbon dioxide (ScWC) extraction technology has potential to help industry in mitigating hazardous aerosol pollutant emission, reducing the need to treat flue gas, and increasing the use of flue gas streams. Successfully removing sulfur and other hazardous molecules from the raw coal before combustion would eliminate pollution of ash, limestone slurry, and air. While many post combustion efforts prove to trade one form of pollution for another, our proposed pre-combustion extraction process seeks to reduce waste in all three phases. In the traditional combustion, treating the flue gas instead of raw coal results in a substantial volume of gas to be processed. This also hinders the ability to further harvest thermal energy from the stream; small improvements in the thermal efficiency of large power plants can have drastic overall economic effects. Pollutant-free flue gas stream may also allow for direct compression of carbon dioxide for sequestration and use. The proposed process has potential to provide new synergy with oxyfuel combustion, Brayton cycle, and enhanced oil recovery technologies. The presence of sulfur and mercury is the main reason for coal processing for power generation to become an expensive proposition. Removing them pre-combustion also offers the potential to use coal for other beneficiated products where these two elements are not desired in the products. Again, the use of CO2 and H2O mixture has potential for industrial applications in the power plants as both CO2 and H2O are available on site.

4 Conclusion

Supercritical water-CO2 (ScWC) and supercritical CO2 extractions are proposed for cleaning of coal before combustion. The coal beneficiation is demonstrated in 200–400 °C range at 143 bar using a semi-continuous process without needing any mineral acid or organic solvents by studying the sulfur removal. Carbon dioxide extraction at 350 °C is effective similar to the typical hydrothermal extraction which was most effective at 290 °C. Extraction with carbon dioxide caused more difficult-to-remove pyritic and organic sulfurs to become sulfate by 200 °C. Extracted solids contained about 50% less sulfur than raw coal for 1-h extractions using CO2 at 350 °C, water at 290 °C or combined H2O–CO2 at 320 °C. While hydrothermal extraction slightly decreased the mass of coal recovered (about 10%), ScWC extraction cause any loss of carbon content. Thus, the extractive strength of the fluid can be tuned by adjusting the temperature and H2O/CO2 flow ratio. Extraction with pure water above the supercritical point of pure water caused hydrothermal carbonization of coal solids where volatile carbons were crosslinked into fixed carbons. Carbonization caused the coal mass to fuse upon drying and may be interesting for further carbon upgrading, but should be avoided for coal meant to be combusted. Hence, it is preferable to operate at 320 °C or below to obtain a free-flowing extracted coal.