Identification of Calcium Sulphoaluminate Formation between Alunite and Limestone
1
Mineral Resources Research Division, Korea Institute of Geoscience & Mineral Resources, 30 Gajeong-dong, Yuseong-gu, Daejeon 305-350, Korea
2
Department of Energy Resources Engineering, Seoul National University, 599 Gwanak-ro, Gwanak-gu, Seoul 151-742, Korea
*
Author to whom correspondence should be addressed.
Sensors 2009, 9(7), 5059-5067; https://doi.org/10.3390/s90705059
Submission received: 31 May 2009
/
Revised: 10 June 2009
/
Accepted: 10 June 2009
/
Published: 25 June 2009
(This article belongs to the Section Chemical Sensors)
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<p>X-ray diffraction patterns of sintered products of mixtures of K<sub>2</sub>SO<sub>4</sub>-3CaO-3Al<sub>2</sub>O<sub>3</sub>-3CaSO<sub>4</sub> at various temperatures in air.</p> ">
<p>X-ray diffraction patterns of sintered products of mixtures of K<sub>2</sub>SO<sub>4</sub>-nCaO-3Al<sub>2</sub>O<sub>3</sub>-3CaSO<sub>4</sub> with various amounts of CaO in air (sintering temp.: 1,200 °C, sintering time: 2 hrs).</p> ">
<p>X-ray diffraction patterns of sintered products of mixtures of K<sub>2</sub>SO<sub>4</sub>-3CaO-3Al<sub>2</sub>O<sub>3</sub>-nCaSO<sub>4</sub> with various amounts of CaSO<sub>4</sub> in air (sintering temp.: 1,200 °C, sintering time: 2 hrs).</p> ">
<p>X-ray diffraction patterns of sintered products of mixtures of K<sub>2</sub>SO<sub>4</sub>-3CaO-3Al<sub>2</sub>O<sub>3</sub>-3CaSO<sub>4</sub>-nSiO<sub>2</sub> with various amounts of SiO<sub>2</sub> in air (sintering temp.: 1,200 °C, sintering time: 2 hrs).</p> ">
<p>X-ray diffraction patterns of sintered products of mixtures of K<sub>2</sub>SO<sub>4</sub>-[(3+m)CaO]-3Al<sub>2</sub>O<sub>3</sub>-3CaSO<sub>4</sub>-nSiO<sub>2</sub> with various amounts of CaO and SiO<sub>2</sub> in air (sintering temp.: 1,200 °C, sintering time: 2 hrs).</p> ">
Versions Notes
<p>X-ray diffraction patterns of sintered products of mixtures of K<sub>2</sub>SO<sub>4</sub>-3CaO-3Al<sub>2</sub>O<sub>3</sub>-3CaSO<sub>4</sub> at various temperatures in air.</p> ">
<p>X-ray diffraction patterns of sintered products of mixtures of K<sub>2</sub>SO<sub>4</sub>-nCaO-3Al<sub>2</sub>O<sub>3</sub>-3CaSO<sub>4</sub> with various amounts of CaO in air (sintering temp.: 1,200 °C, sintering time: 2 hrs).</p> ">
<p>X-ray diffraction patterns of sintered products of mixtures of K<sub>2</sub>SO<sub>4</sub>-3CaO-3Al<sub>2</sub>O<sub>3</sub>-nCaSO<sub>4</sub> with various amounts of CaSO<sub>4</sub> in air (sintering temp.: 1,200 °C, sintering time: 2 hrs).</p> ">
<p>X-ray diffraction patterns of sintered products of mixtures of K<sub>2</sub>SO<sub>4</sub>-3CaO-3Al<sub>2</sub>O<sub>3</sub>-3CaSO<sub>4</sub>-nSiO<sub>2</sub> with various amounts of SiO<sub>2</sub> in air (sintering temp.: 1,200 °C, sintering time: 2 hrs).</p> ">
<p>X-ray diffraction patterns of sintered products of mixtures of K<sub>2</sub>SO<sub>4</sub>-[(3+m)CaO]-3Al<sub>2</sub>O<sub>3</sub>-3CaSO<sub>4</sub>-nSiO<sub>2</sub> with various amounts of CaO and SiO<sub>2</sub> in air (sintering temp.: 1,200 °C, sintering time: 2 hrs).</p> ">
Abstract
:This study was carried out to identify the conditions of formation of calcium sulphoaluminate (3CaO·3Al2O3·CaSO4) by the sintering of a limestone (CaCO3) and alunite [K2SO4·Al2(SO4)3·4Al(OH)3] mixture with the following reagents: K2SO4, CaCO3, Al(OH)3, CaSO4·2H2O, and SiO2. When K2SO4, CaCO3, Al(OH)3, CaSO4·2H2O were mixed in molar ratios of 1:3:6:3 and sintered at 1,200∼1,300 °C, only 3CaO·3Al2O3·CaSO4 and calcium langbeinite (2CaSO4·K2SO4) were generated. With an amount of CaO that is less than the stoichiometric molar ratio, 3CaO·3Al2O3·CaSO4 was formed and anhydrite (CaSO4) did not react and remained behind. With the amount of CaSO4 that is less than the stoichiometric molar ratio, the amounts of 3CaO·3Al2O3·CaSO4 and 2CaSO4·K2SO4 decreased, and that of CaO·Al2O3 increased. In the K2SO4-CaO-Al2O3-CaSO4-SiO2 system, to stabilize the formation of 3CaO·3Al2O3·CaSO4, 2CaSO4·K2SO4, and β-2CaO·SiO2, the molar ratios of CaO: Al2O3: CaSO4 must be kept at 3:3:1 and that of CaO/SiO2, over 2.0; otherwise, the generated amount of 3CaO·3Al2O3·CaSO4 decreased and that of gehlenite (2CaO·Al2O3·SiO2) with no hydration increased quantitatively. Therefore, if all SO3(g) generated by the thermal decomposition of alunite reacts with CaCO3 (or CaO, the thermal decomposition product of limestone) to form CaSO4 in an alunite- limestone system, 1 mol of pure alunite reacts with 6 mol of limestone to form 1 mol of 3CaO·3Al2O3·CaSO4 and 1 mol of 2CaSO4·K2SO4.
1. Introduction
Cement has been prepared using alunite [1], and a type of special cement containing calcium aluminate, anhydrite, and potassium sulfate has been prepared using anhydrite formed by the reaction between SO3(g) that evolves from alunite and limestone via the following reaction:
Choi et al. [2] synthesized a calcium sulphoaluminate clinker consisting of 3CaO·3Al2O3·CaSO4, CaO and CaSO4 through the sintering for 2 hrs at a temperature of 1,200 °C of alunite, limestone and an anhydrite mixture at a weight ratio of 1:13:5. Their research results showed that alunite could be used in the preparation of a 3CaO·3Al2O3·CaSO4 clinker provided that adequate mixing conditions are provided, despite that the expansion is relatively small compared to that of a clinker synthesized from reagents. However, the exact formation conditions of 3CaO·3Al2O3·CaSO4 in the sintering state were not discussed. In addition, Han et al. [3,4] synthesized a clinker containing calcium fluoroaluminate (C11A7·CaF2) from domestic alunite and investigated its characteristics in an effort to develop a type of fast-hardening cement.
The authors [5] carried out an investigation of the conditions under which 3CaO·3Al2O3·CaSO4 is formed when mixtures of alunite and limestone are sintered. It was concluded that calcium langbeinite (2CaSO4·K2SO4) forms from 700 °C and that calcium sulphoaluminate forms from 800 °C. Both are stable up to 1,300 °C, as shown in the equation below:
However, when alunite or limestone is incorporated in SiO2 so as to enable the formation of calcium sulphoaluminate, the molar ratios of CaO/alunite and CaO/SiO2 must be kept over 6.0 and 2.0, respectively. A clinker composed of calcium sulphoaluminate and calcium langbeinite was transformed into ettringite(3CaO·Al2O3·3CaSO4·32H2O) in water as calcium langbeinite is transformed into CaSO4·2H2O(s) and K2SO4 (aq) in water.
In the present study, the formation of 3CaO·3Al2O3·CaSO4 is identified in a K2SO4-CaO-Al2O3-CaSO4-SiO2 system using reagents of various types in a detailed investigation of the formation conditions of this species through the sintering of a mixture of alunite and limestone.
2. Experimental
The reagents listed in Table 1 were used to investigate the reaction products arising from the K2SO4-CaO-Al2O3-CaSO4-SiO2 system. K2SO4 and Al(OH)3 were used in substitution for the components of alunite; calcium carbonate (CaCO3) substituted for limestone, and CaSO4·2H2O, substituted for anhydrite (CaSO4), which is formed by the sintering reaction between alunite and limestone.
The mixture of reagents were sintered in a programmable electric furnace (Barnstead /Thermolyne F46120 CM High-Temperature Furnace : 240 V, 40 A, 2,500 Watt, 50/60 Hz, 1 Phase) below 1,300 °C in an air atmosphere. The mineral phases of the manufactured clinker were then analyzed by XRD(PW-1700, Philips, 30kV, 25mA, Cu target, Ni filter, at a scanning rate of 2°/min). After the prepared clinker was finely milled with a laboratory ball mill, the mineral phases of the crushed clinker were analyzed by XRD.
3. Results and Discussion
Alunite (K2SO4·Al2(SO4)3·4Al(OH)) is transformed into KAl(SO4)2 and Al2O3 by dehydration at 500∼580 °C and KAl(SO4)2, K2SO4 and Al2O3 by desulphurization at 700∼780 °C via the reaction of K2SO4·Al2(SO4)3·4Al(OH)3 → K2SO4 + 2Al2O3 + 3SO3(g) + 6H2O(g), regardless of the partial pressure of CO2(g). However, limestone decomposes from 650 °C in air and from 900 °C in a CO2(g) saturated atmosphere [6].
When the mixture of alunite and limestone is sintered in air and in a CO2(g) saturated atmosphere, the rate of formation of anhydrite is relatively low, at 76.0% and 67.0%, respectively, at a CaCO3/alunite stoichiometric molar ratio of 3. However, the rate of formation increases as the molar ratio of CaCO3/alunite (particle size, 37∼44 μm) exceeds 6, showing rates of more than 99.0% and 95.0% in air and in a CO2(g) saturated atmosphere, respectively [7].
As shown in the results of aforementioned experiment, if alunite and limestone are mixed and sintered in air, most of the generated SO3 reacts with limestone to form anhydrite (CaSO4). Additionally, ignoring impurities such as Fe2O3, TiO2, and P2O5 included in the alunite, because alunite ore is composed of alunite, quartz(SiO2), and the aluminum silicate minerals of kaolinite, dickite, and pyrophyllite, the alunite and limestone mixture can be said to have five components, as does K2SO4-CaO-Al2O3-CaSO4-SiO2.
If 1 mol if pure alunite is heated to temperatures that exceed 800 °C, it is pyrolyzed as K2SO4·Al2(SO4)3·4Al(OH)3 → K2SO4 + 3Al2O3 + 3SO3 + 6H2O. Therefore, to formulate SO3(g) of 3 mol into anhydrite, 3 mol of CaCO3 is required, and to change 3 mol of Al2O3 into 3CaO·3Al2O3·CaSO4, 3 additional mol of CaCO3 and 1 mol of CaSO4 will be needed. Therefore, to change all of the Al2O3 in alunite into 3CaO·3Al2O3·CaSO4, and to generate SO3(g) by the thermal decomposition of alunite into anhydrite, theoretically, pure alunite and limestone should be mixed at a molar rate of 1:6. This mixture will be composed of five component systems as in K2SO4-CaO-Al2O3-CaSO4.
The present study aims to determine the mineral phases of a clinker generated in the K2SO4-CaO-Al2O3-CaSO4 and the K2SO4-CaO-Al2O3-CaSO4-SiO2 systems, using several types of reagents, including K2SO4, Al(OH)3, SiO2, CaSO4·2H2O, and CaCO3.
Figure 1 shows X-ray diffraction patterns of the materials generated, when a compound consisting of K2SO4-3CaO-3Al2O3-3CaSO4 was sintered at 1,100 °C, 1,200 °C, and 1,300 °C, respectively, for 2 hours. As shown in this figure, 3CaO·3Al2O3·CaSO4 and 2CaSO4·K2SO4 is formed, but CaSO4 does not react and remains at 1,100 °C. Meanwhile, at temperatures in excess of 1,200 °C 3CaO·3Al2O3·CaSO4 and 2CaSO4·K2SO4 were mainly generated. Accordingly, 1 mol of pure alunite reacts with 6 mol of limestone to form 1 mol of 3CaO·3Al2O3·CaSO4 and 1 mol of 2CaSO4·K2SO4 as follows; K2SO4·Al2(SO4)3·4Al(OH)3 + 6CaCO3 → 2CaSO4·K2SO4 + 3CaO·3Al2O3·CaSO4 + 6H2O(g) + 6CO2(g).
Figure 2 displays the materials generated from K2SO4-nCaO-3Al2O3-3CaSO4 with various amounts of CaO sintered at 1,200 °C for two hours, as determined via an XRD analysis.
When it CaO is included in at an amount of 3 mol, 3CaO·3Al2O3·CaSO4 and 2CaSO4·K2SO4 are mainly generated. However, it was found that as the amount of CaO is increased from 3 mol to 5 mol, CaO does not participate in the formation reaction of 3CaO·3Al2O3·CaSO4. Thus, it can be said that 3CaO·3Al2O3·CaSO4 and 2CaSO4·K2SO4 are generated stably when CaO is 3 mol in the K2SO4-nCaO-3Al2O3-3CaSO4 system.
According to Fukuda [8] 3CaO·3Al2O3·CaSO4 is the only compound in the CaO-Al2O3-SO3 system. This line of research was started in 1962 by Halstead, et al. [9] with Ca2+ and SO42− ions in a three-dimensional crystal structure sharing the angular point of a AlO4 tetrahedron; an Al3+ ion is coordinated with four O2− ions, a Ca2+ ion is surrounded asymmetrically by O2− ions, and an isolated SO42− ion is characterized by its ability to readily react with water. Kondo [10] discovered that these ions become hardened in water. In general, they are produced by re-sintering after producing 3CaO·Al2O3 and regulating the mixture ratio of 3CaO·Al2O3, CaSO4·2H2O and Ca(OH)2 and by sintering a mixture of CaCO3, Al2O3, and CaSO4·2H2O.
2CaSO4·K2SO4 is easily generated in the CaO-Al2O3-SiO2-Fe2O3-MgO-CaSO4-K2SO4 system and has a considerable influence on the condensation time and the hardening characteristics of cements. Known as a water-soluble alkali, as 2CaSO4·K2SO4 can be easily separated from the liquid state of a clinker oxide and is said to become K2SO4·CaSO4·H2O(syngenite) and CaSO4·2H2O upon exposure to water [11].
Figure 3 shows the materials generated from the K2SO4-3CaO-3Al2O3-nCaSO4 system sintered at 1,200 °C for two hours with varying amounts of anhydrite, as determined via an XRD analysis.
As shown in this figure, when anhydrite is included in an amount of 3 mol, 3CaO·3Al2O3·CaSO4 and 2CaSO4·K2SO4 are generated. However, as the amount of anhydrite is decreased from 3 mol to 1 mol, it was observed that the K2SO4 that did not react with CaO·Al2O3 remained. As the amount of anhydrite is increased from 3 mol to 5 mol, only the diffraction strength of the CaSO4 that does not react increases. Thus, it can be said that an amount of CaSO4 in excess of the stoichiometric molar ratio is necessary to generate 3CaO·3Al2O3·CaSO4 stably.
As noted above, 3CaO·3Al2O3·CaSO4 and 2CaSO4·K2SO4 were mainly generated in the K2SO4-3CaO-3Al2O3-3CaSO4 system. However, because alunite from nature has impurities of SiO2 and aluminum silicate minerals such as kaolinite, dickite, and pyrophyllite, the alunite and limestone mixture is believed to be comprised of a K2SO4-CaO-Al2O3-CaSO4-SiO2 system to which SiO2 is added.
Figures 4 and 5 show, by XRD analysis, the materials generated from the K2SO4-3CaO-3Al2O3-3CaSO4-nSiO2 system and the K2SO4-(3+m)CaO-3Al2O3-3CaSO4-nSiO2 system, respectively, sintered at 1,200 °C for 2 hours, with various amounts of CaO (3 + m : mol number) and SiO2(n: mol number). In Figure 4, when there is no SiO2 in the mixture, the result is identical to that obtained when 3 mol of CaO is used (Figure 2). It is expected that 3CaO·3Al2O3·CaSO4 and 2CaSO4·K2SO4 will be generated. However, as the amount of SiO2 is increased from 1 mol to 5 mol, the amount of 3CaO·3Al2O3·CaSO4 generated is reduced, because gehlenite (2CaO·Al2O3·SiO2) and wollastonite (α-CaO·SiO2), which do not react with water, are generated. In addition, as shown in Figure 5, when the mol rate of CaO/alunite is less than 6 (m less than 3), and that of CaO/SiO2 is less than 2, the synthetic clinker contained 2CaO·Al2O3·SiO2 and CaSO4; these compounds do not participate in the formation reaction of 3CaO·3Al2O3·CaSO4 because 3CaO·3Al2O3·CaSO4 is the only compound in the CaO-Al2O3-SO3 system as noted above[8] and CaO and Al2O3 participate preferentially in the formation reaction of 2CaO·Al2O3·SiO2. Accordingly, if all SO3(g) generated by thermal decomposition of alunite reacts with CaCO3 (or CaO, the thermal decomposition product of limestone) to form CaSO4 in the alunite-limestone system, when the molar ratios of CaO/alunite exceed 6 and that of CaO/SiO2 exceeds 2, 3CaO·3Al2O3·CaSO4, 2CaSO4·K2SO4 and β-2CaO·SiO2 are generated stably.
4. Conclusions
This study investigated the formation characteristics of calcium sulphoaluminate (4CaO·3Al2O3·SO3) in a K2SO4-CaO-Al2O3-CaSO4-SiO2 system using reagents of various types in an effort to identify the formation conditions of 3CaO·3Al2O3·CaSO4 by the sintering of a mixture of alunite and limestone. In experiments with reagents for the mineral phases generated from the compound system (the K2SO4-CaO-Al2O3-CaSO4-SiO2 system), if all SO3(g) from alunite reacts with limestone to form anhydrite, it was found that 1 mol of pure alunite reacts with 6mol of limestone to form 1 mol of 3CaO·3Al2O3·CaSO4 and 1 mol of 2CaSO4·K2SO4, as of 3CaO·3Al2O3·CaSO4 and 2CaSO4·K2SO4 are generated stably at a component ratio of K2SO4-3CaO-3Al2O3-3CaSO4. Over-mixing of CaO and CaSO4 has a slight effect on the generation of 3CaO·3Al2O3·CaSO4. However, it is thought that under-mixing will have a substantial effect on the mineral phase of the clinker and on the amount of 3CaO·3Al2O3·CaSO4 that is generated. Moreover, if the impurities of SiO2 are incorporated in the alunite and limestone, the molar ratio of CaO/alunite must exceed 6 and that of CaO/SiO2 must exceed 2 in order to ensure the stable formation of calcium sulphoaluminate, calcium langbeinite, and the β-2CaO·SiO2 phases. Otherwise, the amount of gehlenite(2CaO·Al2O3·SiO2), which does not react with water, may be increased.
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Figure 1.
X-ray diffraction patterns of sintered products of mixtures of K2SO4-3CaO-3Al2O3-3CaSO4 at various temperatures in air.
Figure 1.
X-ray diffraction patterns of sintered products of mixtures of K2SO4-3CaO-3Al2O3-3CaSO4 at various temperatures in air.
Figure 2.
X-ray diffraction patterns of sintered products of mixtures of K2SO4-nCaO-3Al2O3-3CaSO4 with various amounts of CaO in air (sintering temp.: 1,200 °C, sintering time: 2 hrs).
Figure 2.
X-ray diffraction patterns of sintered products of mixtures of K2SO4-nCaO-3Al2O3-3CaSO4 with various amounts of CaO in air (sintering temp.: 1,200 °C, sintering time: 2 hrs).
Figure 3.
X-ray diffraction patterns of sintered products of mixtures of K2SO4-3CaO-3Al2O3-nCaSO4 with various amounts of CaSO4 in air (sintering temp.: 1,200 °C, sintering time: 2 hrs).
Figure 3.
X-ray diffraction patterns of sintered products of mixtures of K2SO4-3CaO-3Al2O3-nCaSO4 with various amounts of CaSO4 in air (sintering temp.: 1,200 °C, sintering time: 2 hrs).
Figure 4.
X-ray diffraction patterns of sintered products of mixtures of K2SO4-3CaO-3Al2O3-3CaSO4-nSiO2 with various amounts of SiO2 in air (sintering temp.: 1,200 °C, sintering time: 2 hrs).
Figure 4.
X-ray diffraction patterns of sintered products of mixtures of K2SO4-3CaO-3Al2O3-3CaSO4-nSiO2 with various amounts of SiO2 in air (sintering temp.: 1,200 °C, sintering time: 2 hrs).
Figure 5.
X-ray diffraction patterns of sintered products of mixtures of K2SO4-[(3+m)CaO]-3Al2O3-3CaSO4-nSiO2 with various amounts of CaO and SiO2 in air (sintering temp.: 1,200 °C, sintering time: 2 hrs).
Figure 5.
X-ray diffraction patterns of sintered products of mixtures of K2SO4-[(3+m)CaO]-3Al2O3-3CaSO4-nSiO2 with various amounts of CaO and SiO2 in air (sintering temp.: 1,200 °C, sintering time: 2 hrs).
| Reagents | Chemical formula | Purity | Manufacturer |
|---|---|---|---|
| Potassium Sulfate | K2SO4 | First grade | Ducksan Pharmaceutical Co., Ltd |
| Aluminum Hydroxide | Al(OH)3 | First grade | Shinyo Pure Chemical Co., Ltd |
| Calcium Carbonate | CaCO3 | min 98.0% | Kanto Chemical Co., Inc. |
| Gypsum | CaSO4·2H2O | Extra pure | Junsei Chemical Co., Ltd. |
| Silicate Dioxide | SiO2 | Extra pure | Junsei Chemical Co., Ltd. |
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Kim, H.-S.; Han, G.-C.; Ahn, J.-W.; Cho, K.-H.; Cho, H.-C. Identification of Calcium Sulphoaluminate Formation between Alunite and Limestone. Sensors 2009, 9, 5059-5067. https://doi.org/10.3390/s90705059
AMA Style
Kim H-S, Han G-C, Ahn J-W, Cho K-H, Cho H-C. Identification of Calcium Sulphoaluminate Formation between Alunite and Limestone. Sensors. 2009; 9(7):5059-5067. https://doi.org/10.3390/s90705059
Chicago/Turabian StyleKim, Hyung-Seok, Gi-Chun Han, Ji-Whan Ahn, Kye-Hong Cho, and Hee-Chan Cho. 2009. "Identification of Calcium Sulphoaluminate Formation between Alunite and Limestone" Sensors 9, no. 7: 5059-5067. https://doi.org/10.3390/s90705059
APA StyleKim, H.-S., Han, G.-C., Ahn, J.-W., Cho, K.-H., & Cho, H.-C. (2009). Identification of Calcium Sulphoaluminate Formation between Alunite and Limestone. Sensors, 9(7), 5059-5067. https://doi.org/10.3390/s90705059
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