Hyperspectral Mapping of Surface Mineralogy in the Lake Magadi Area in Kenya
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CASE STUDY Methane Recovery at Non-Coal Mines
CASE STUDY Methane Recovery at Non-coal Mines Background Existing methane recovery projects at non-coal mines reduce greenhouse gas (GHG) emissions by up to 3 million tons of carbon dioxide equivalent (CO₂e). Although methane emissions are generally associated with coal mines, methane is also found in salt, potash, trona, diamond, gold, base metals, and lead mines throughout the world. Many of these deposits are located adjacent to hydrocarbon (e.g., coal and oil) deposits where methane originates. Consequently, during the process of mining non-coal deposits, methane may be released. Overview of Methane Recovery Projects Beatrix Gold Mine, South Africa Promethium Carbon, a carbon and climate change advisory firm, has developed a project to capture and use methane from the Beatrix Gold Mine in Free State, South Africa (see box). Project Specifications: Beatrix Gold Mine Name Capture and Utilization of Methane at the Gold Fields–owned Beatrix Mine in South Africa Site Free State Province, South Africa Owner Gold Fields Ltd., Exxaro On-site Pty Ltd. Dates of Operation May 2011–present Equipment Phase 1 • GE Roots Blowers • Trolex gas monitoring systems • Flame arrestor • 23 burner flare Equipment Phase 2 Addition of internal combustion engines End-use Phase 1 Destruction through flaring End-use Phase 2 4 MW power generation Emission Reductions 1.7 million tons CO²e expected over CDM project lifetime (through 2016) Commissioning of Flare at Beatrix Gold Mine (Photo courtesy of Gold Fields Ltd.) CASE STUDY Methane Recovery at Non-coal Mines ABUTEC Mine Gas Incinerator at Green River Trona Mine (Photo courtesy of Solvay Chemicals, Inc.) Green River Trona Mine, United States Project Specifications: Green River Trona Mine Trona is an evaporite mineral mined in the United States Name Green River Trona Mine Methane as the primary source of sodium carbonate, or soda ash. -
Trona Na3(CO3)(HCO3) • 2H2O C 2001-2005 Mineral Data Publishing, Version 1
Trona Na3(CO3)(HCO3) • 2H2O c 2001-2005 Mineral Data Publishing, version 1 Crystal Data: Monoclinic. Point Group: 2/m. Crystals are dominated by {001}, {100}, flattened on {001} and elongated on [010], with minor {201}, {301}, {211}, {211}, {411},to 10 cm; may be fibrous or columnar massive, as rosettelike aggregates. Physical Properties: Cleavage: {100}, perfect; {211} and {001}, interrupted. Fracture: Uneven to subconchoidal. Hardness = 2.5–3 D(meas.) = 2.11 D(calc.) = 2.124 Soluble in H2O, alkaline taste; may fluoresce under SW UV. Optical Properties: Translucent. Color: Colorless, gray, pale yellow, brown; colorless in transmitted light. Luster: Vitreous. Optical Class: Biaxial (–). Orientation: X = b; Z ∧ c =83◦. Dispersion: r< v; strong. α = 1.412–1.417 β = 1.492–1.494 γ = 1.540–1.543 2V(meas.) = 76◦160 2V(calc.) = 74◦ Cell Data: Space Group: I2/a. a = 20.4218(9) b = 3.4913(1) c = 10.3326(6) β = 106.452(4)◦ Z=4 X-ray Powder Pattern: Sweetwater Co., Wyoming, USA. 2.647 (100), 3.071 (80), 4.892 (55), 9.77 (45), 2.444 (30), 2.254 (30), 2.029 (30) Chemistry: (1) (2) CO2 38.13 38.94 SO3 0.70 Na2O 41.00 41.13 Cl 0.19 H2O 20.07 19.93 insol. 0.02 −O=Cl2 0.04 Total 100.07 100.00 • (1) Owens Lake, California, USA; average of several analyses. (2) Na3(CO3)(HCO3) 2H2O. Occurrence: Deposited from saline lakes and along river banks as efflorescences in arid climates; rarely from fumarolic action. Association: Natron, thermonatrite, halite, glauberite, th´enardite,mirabilite, gypsum (alkali lakes); shortite, northupite, bradleyite, pirssonite (Green River Formation, Wyoming, USA). -
Remarks on Different Methods for Analyzing Trona and Soda Samples
REMARKS ON DIFFERENT METHODS FOR ANALYZING TRONA AND SODA SAMPLES Gülay ATAMAN*; Süheyla TUNCER* and Nurgün GÜNGÖR* ABSTRACT. — Trona is one of the natural forms of sodium carbonate minerals. It is well known as «sesque carbonate», «urao» or «trona» in the chemical literature, and the chemical formula of the compound is [Na2CO3.NaHCO3.2H2O]. The aim of this work is to adapt the standard methods for the analysis of trona samples, considering the inter- ferences arising from silicates and other minerals found together with trona samples. In order to reduce the experimen- tal errors, the analyses used for the determination of trona samples have been revised. The experimental results using potentiometric titration, AgNO3 external indicator and BaCl2 titration methods have been compared to theoretical results using statistical evaluations. 95 % confidence level, which is commonly used by analytical chemists, was employed as the basis of evaluation, R values, Student's t calculated at 95 % confidence level of 7 trona samples from Beypazarı, Student's t tabulated for the percentages of Na2CO3, were found to be 0.008 in BaCl2 method, 3.25 for AgNO3 external indicator method and 3.26 for potentiometric method; for the percentages of NaHCO3 the same values are 0.59 for BaCl2 method, 2.83 for AgNO3 external indicator method and 3.59 for potentiometric method. Systematic error is indicated when R> 1. In addi- tion to quantitative analysis of trona samples, qualitative XRD analyses have been routinely performed for each sample and the results were found to be in good agreement. INTRODUCTION Trona is a naturally occuring from of sodium carbonate minerals. -
Rocks and Minerals Make up Your World
Rocks and Minerals Make up Your World Rock and Mineral 10-Specimen Kit Companion Book Presented in Partnership by This mineral kit was also made possible through the generosity of the mining companies who supplied the minerals. If you have any questions or comments about this kit please contact the SME Pittsburgh Section Chair at www.smepittsburgh.org. For more information about mining, visit the following web sites: www.smepittsburgh.org or www.cdc.gov/niosh/mining Updated August 2011 CONTENTS Click on any section name to jump directly to that section. If you want to come back to the contents page, you can click the page number at the bottom of any page. INTRODUCTION 3 MINERAL IDENTIFICATION 5 PHYSICAL PROPERTIES 6 FUELS 10 BITUMINOUS COAL 12 ANTHRACITE COAL 13 BASE METAL ORES 14 IRON ORE 15 COPPER ORE 16 PRECIOUS METAL ORE 17 GOLD ORE 18 ROCKS AND INDUSTRIAL MINERALS 19 GYPSUM 21 LIMESTONE 22 MARBLE 23 SALT 24 ZEOLITE 25 INTRODUCTION The effect rocks and minerals have on our daily lives is not always obvious, but this book will help explain how essential they really are. If you don’t think you come in contact with minerals every day, think about these facts below and see if you change your mind. • Every American (including you!) uses an average of 43,000 pounds of newly mined materials each year. • Coal produces over half of U.S. electricity, and every year you use 3.7 tons of coal. • When you talk on a land-line telephone you’re holding as many as 42 different minerals, including aluminum, beryllium, coal, copper, gold, iron, limestone, silica, silver, talc, and wollastonite. -
Ulexite Nacab5o6(OH)6 • 5H2O C 2001-2005 Mineral Data Publishing, Version 1 Crystal Data: Triclinic
Ulexite NaCaB5O6(OH)6 • 5H2O c 2001-2005 Mineral Data Publishing, version 1 Crystal Data: Triclinic. Point Group: 1. Rare as measurable crystals, which may have many forms; typically elongated to acicular along [001], to 5 cm, then forming fibrous cottonball-like masses; in compact parallel fibrous veins, and radiating and compact nodular groups. Twinning: Polysynthetic on {010} and {100}; possibly also on {340}, {230}, and others. Physical Properties: Cleavage: On {010}, perfect; on {110}, good; on {110}, poor. Fracture: Uneven across fiber groups. Tenacity: Brittle. Hardness = 2.5 D(meas.) = 1.955 D(calc.) = 1.955 Slightly soluble in H2O; parallel fibrous masses can act as fiber optical light pipes; may fluoresce yellow, greenish yellow, cream, white under SW and LW UV. Optical Properties: Transparent to opaque. Color: Colorless; white in aggregates, gray if included with clays. Luster: Vitreous; silky or satiny in fibrous aggregates. Optical Class: Biaxial (+). Orientation: X (11.5◦,81◦); Y (100◦,21.5◦); Z (107◦,70◦) [with c (0◦,0◦) and b∗ (0◦,90◦) using (φ,ρ)]. α = 1.491–1.496 β = 1.504–1.506 γ = 1.519–1.520 2V(meas.) = 73◦–78◦ Cell Data: Space Group: P 1. a = 8.816(3) b = 12.870(7) c = 6.678(1) α =90.36(2)◦ β = 109.05(2)◦ γ = 104.98(4)◦ Z=2 X-ray Powder Pattern: Jenifer mine, Boron, California, USA. 12.2 (100), 7.75 (80), 6.00 (30), 4.16 (30), 8.03 (15), 4.33 (15), 3.10 (15b) Chemistry: (1) (2) B2O3 43.07 42.95 CaO 13.92 13.84 Na2O 7.78 7.65 H2O 35.34 35.56 Total 100.11 100.00 • (1) Suckow mine, Boron, California, USA. -
PERIDOT from TANZANIA by Carol M
PERIDOT FROM TANZANIA By Carol M. Stockton and D. Vincent Manson Peridot from a new locality, Tanzania, is described Duplex I1 refractometer and sodium light, approx- and compared with 13 other peridots from various imate a = 1.650, B = 1.658, and -y = 1.684, indi- localities in terms of color and chemical com- cating a biaxial positive optic character. The position. The Tanzanian specimen is lower in iron specific gravity, measured hydrostatically, is ap- content than all but the Norwegian peridots and is proximately 3.25. very similar to material from Zabargad, Egypt. A gem-quality enstatite that came from the same area CHEMISTRY in East Africa and with which Tanzanian peridot has been confused is also described. The Tanzanian peridot was analyzed using a MAC electron microprobe at an operating voltage of 15 KeV and beam current of 0.05 PA. The standards used were periclase for MgO, kyanite for Ala, quartz for SiOz, wollastonite for CaO, rutile for In September 1982, Dr. Horst Krupp, of Idar- TiOa, chromic oxide for CraOg, almandine-spes- Oberstein, sent GIA's Department of Research a sartine garnet for MnO, fayalite for FeO, and nickel sample of peridot for study. The stone was from oxide for NiO. The data were corrected using the a parcel that supposedly contained enstatite pur- Ultimate correction program (Chodos et al., 1973). chased from the Tanzanian State Gem Corpora- For purposes of comparison, we also selected tion, the source of a previous lot of enstatite that and analyzed peridots from major known locali- Dr. Krupp had already cut and marketed. -
Olivine – Peridot 橄欖石 Prof
Olivine – Peridot 橄欖石 Prof. Dr H.A. Hänni, FGA, SSEF Research Associate Email: [email protected] Fig. 1 Peridots rough and cut, from various locations. Photo © H.A.Hänni 作者述了寶石級橄欖石的特性,它歸屬於橄欖石 類礦物,它有三種成因,化學成的改變而引致顏 色、折射率和比重的變異,並簡報其內含物、人工 合成方法和產地,以及作為首飾時應注意的地方。 Peridot is a widely appreciated green gemstone (Fig. 1). It belongs to the Olivine group, which also includes the major minerals forsterite Mg2SiO4, fayalite Fe2SiO4 and tephroite Mn2SiO4. Olivines are the main constituents of maic and ultramaic rocks that are formed in the earth’s mantle. Olivine-basalt rocks bring the crystals to the surface, where they are found e.g. in extended basalt layers such as in China (Hebei province) (Fig. 2), and the Fig. 3 A Pallasite, an iron-nickel matrix with olivine crystals. Photo © H.A.Hänni USA (Arizona). Another genetic type of olivines is found in rocks formed by metamorphism like in Myanmar or Pakistan. Olivines are also the main constituents of rare pallasites, nickel-iron meteorites, with large inclusions of olivine (Fig. 3). Synthetic forsterites with dopants are used for laser technology applications. Gemstone olivine is called peridot, and also chrysolite. It is represented by a solid mixture between the Mg member forsterite (fo) and the Fe member fayalite (fa), with high fo and low fa concentrations. Occasional Fig. 2 An olivine-basalt rock sample with olivine grain contributions of Mn, Ni or Cr are always very small, but clusters and a larger olivine crystal from Zhangjikou- inluence the colour of the stone. Forsterite and fayalite Xuanhua, Hebei Province, China. are a solid solution series just as pyrope and almandine Photo © H.A.Hänni garnets. -
Forsterite Dissolution and Magnesite Precipitation at Conditions Relevant for Deep Saline Aquifer Storage and Sequestration of Carbon Dioxide
Chemical Geology 217 (2005) 257–276 www.elsevier.com/locate/chemgeo Forsterite dissolution and magnesite precipitation at conditions relevant for deep saline aquifer storage and sequestration of carbon dioxide Daniel E. Giammara,T, Robert G. Bruant Jr.b, Catherine A. Petersb aDepartment of Civil Engineering and Environmental Engineering Science Program, Washington University, St. Louis, MO 63130, United States bProgram in Environmental Engineering and Water Resources, Department of Civil and Environmental Engineering, Princeton University, Princeton, NJ 08544, United States Received 30 April 2003; accepted 10 December 2004 Abstract The products of forsterite dissolution and the conditions favorable for magnesite precipitation have been investigated in experiments conducted at temperature and pressure conditions relevant to geologic carbon sequestration in deep saline aquifers. Although forsterite is not a common mineral in deep saline aquifers, the experiments offer insights into the effects of relevant temperatures and PCO2 levels on silicate mineral dissolution and subsequent carbonate precipitation. Mineral suspensions and aqueous solutions were reacted at 30 8C and 95 8C in batch reactors, and at each temperature experiments were conducted with headspaces containing fixed PCO2 values of 1 and 100 bar. Reaction products and progress were determined by elemental analysis of the dissolved phase, geochemical modeling, and analysis of the solid phase using scanning electron microscopy, infrared spectroscopy, and X-ray diffraction. The extent of forsterite dissolution increased with both increasing temperature and PCO2. The release of Mg and Si from forsterite was stoichiometric, but the Si concentration was ultimately controlled by the solubility of amorphous silica. During forsterite dissolution initiated in deionized water, the aqueous solution reached supersaturated conditions with respect to magnesite; however, magnesite precipitation was not observed for reaction times of nearly four weeks. -
12.109 Lecture Notes September 29, 2005 Thermodynamics II Phase
12.109 Lecture Notes September 29, 2005 Thermodynamics II Phase diagrams and exchange reactions Handouts: using phase diagrams, from 12.104, Thermometry and Barometry Fractional crystallization vs. equilibrium crystallization Perfect equilibrium – constant bulk composition, crystals + melt react, reactions go to equilibrium Perfect fractional – situation where reaction between phases is incomplete, melt entirely removed, etc. Because earth is not in equilibrium, we have interesting geology! Binary system = 2 component system Example: albite (Ab) and anorthite (An) solid solution Phase diagrams show the equilibrium case. Fractional crystallization would result in zoned crystal growth: The exchange of ions happens by solid state diffusion. If the crystal grows faster than ions can diffuse through it, the outer layers form with different compositions, thus we have a chemically zoned crystal. Olivine and plagioclase commonly grow this way. In crossed polarized light, you can see gradual extinction from the center, out to the edges of the crystal. This is also sometimes visible in clinopyroxene. Fractional crystallization preserves the original composition. The center zone has the composition of the crystal from the liquidus. The liquidus composition reveals the temperature of the liquid when it arrived at the final crystallization. Solvus, or miscibility gap – in system with solid solution, region of immiscibility (inability to mix) In Na-K feldspars, perthite results from unmixing of a single crystalline phase two coexisting phases with different compositions and same crystal structure As T goes down, two phases separate out (spinoidal decomposition) Feldspar system, see Bowen and Tuttle Thermometry and Barometry Thermobarometer Igneous and metamorphic rocks Uses composition of coexisting minerals to tell us something about T + P Liquidus minerals record temperature (if you can preserve the composition of the liquidus mineral. -
Geological Mapping and Characterization of Possible Primary Input Materials for the Mineral Sequestration of Carbon Dioxide in Europe
minerals Article Geological Mapping and Characterization of Possible Primary Input Materials for the Mineral Sequestration of Carbon Dioxide in Europe Dario Kremer 1,*, Simon Etzold 2,*, Judith Boldt 3, Peter Blaum 4, Klaus M. Hahn 1, Hermann Wotruba 1 and Rainer Telle 2 1 AMR Unit of Mineral Processing, RWTH Aachen University, Lochnerstrasse 4-20, 52064 Aachen, Germany 2 Department of Ceramics and Refractory Materials, GHI - Institute of Mineral Engineering, RWTH Aachen University, Mauerstrasse 5, 52064 Aachen, Germany 3 HeidelbergCement AG-Global Geology, Oberklamweg 2-4, 69181 Leimen, Germany 4 HeidelbergCement AG-Global R&D, Oberklamweg 2-4, 69181 Leimen, Germany * Correspondence: [email protected] (D.K.); [email protected] (S.E.); Tel.: +49-241-80-96681(D.K.); +49-241-80-98343 (S.E.) Received: 19 June 2019; Accepted: 10 August 2019; Published: 13 August 2019 Abstract: This work investigates the possible mineral input materials for the process of mineral sequestration through the carbonation of magnesium or calcium silicates under high pressure and high temperatures in an autoclave. The choice of input materials that are covered by this study represents more than 50% of the global peridotite production. Reaction products are amorphous silica and magnesite or calcite, respectively. Potential sources of magnesium silicate containing materials in Europe have been investigated in regards to their availability and capability for the process and their harmlessness concerning asbestos content. Therefore, characterization by X-ray fluorescence (XRF), X-ray diffraction (XRD), and QEMSCAN® was performed to gather information before the selection of specific material for the mineral sequestration. The objective of the following carbonation is the storage of a maximum amount of CO2 and the utilization of products as pozzolanic material or as fillers for the cement industry, which substantially contributes to anthropogenic CO2 emissions. -
Quantitative Redox Control and Measurement in Hydrothermal Experiments
Fluid-Mineral Interactions: A Tribute to H. P. Eugster © The Geochemical Society, Special Publication No.2, 1990 Editors: R. J. Spencer and I-Ming Chou Quantitative redox control and measurement in hydrothermal experiments I-MING CHOU and GARY L. CYGAN 959 National Center, U.S. Geological Survey, Reston, Virginia 22092, U.S.A. Abstract-In situ redox measurements have been made in sealed Au capsules containing the assemblage Co-CoO-H20 by using hydrogen-fugacity sensors at 2 kbar pressure with three different pressure media, Ar, CH4 and H20, and between 500 and 800°C. Results show that equilibrium redox states can be achieved and maintained under Ar or CH4 external pressure, but they cannot be achieved and maintained at temperatures above 600°C under H20 external pressure. The conventional as- sumption that equilibrium redox condition is achieved at a fixed P- T condition in the presence of a redox buffer assemblage is therefore not necessarily valid, mainly due to the slow kinetics of the buffer reaction and/or the high rate of hydrogen leakage through the buffer container. The inconsistent equilibrium phase boundaries for the assemblage annite-sanidine-magnetite-fluid reported in the literature can be explained by the inadequate redox control in some of the earlier experiments. The attainment of redox equilibrium in hydrothermal experiments should be confirmed by the inclusion of a hydrogen-fugacity sensor in each experiment where the redox state is either quantitatively or semiquantitatively controlled. INTRODUCfION this assumption is not always valid. Therefore, some of the published data on the mineral stability re- THE PIONEERINGWORKOF EUGSTER (1957) on the lations in P- T-f O or P- T-JH2 space obtained by solid oxygen buffer technique provides a convenient 2 using the oxygen-buffer technique may not be re- way to control redox states in hydrothermal exper- liable, as indicated, for example, by the recent data iments. -
CRYSTAL STRUCTURES of NATURAL OLIVINES J. D. Brnmt
THE AMERICAN MINERALOGISI', VOL 53, MAY_JUNE, 1968 CRYSTAL STRUCTURES OF NATURAL OLIVINES J. D. Brnmt, G.V. Grnns2,P. B. MoonE, ANDJ. V. SurrH, Departmentof the GeophysicalSciences, (Jn'ittersity of Chicago Chicago,Illinois 60637,U.S.A. Ansrnncr Atomic parameters were obtained by 3D least-squares X-ray difiraction analysis of forsterite (Mgo go,Feo1s), plutonic hyalosiderite (Mgo u:u,Feonso,Mrio ooo,CzIo oor), dike hortonolite (Mgo as,Feoas,Mno or,Cao or), and fayalite (Feo gz,Mgoor,Mns ,r). The closeness in value of the isotropic temperature factors calculated for the M sites indicates substitutional disorder of the Mg and Fe atoms in all four structures. Poiyhedra distortions are closely similar in all four structures showing that they depend on the struc- ture type rather than on the Mg, Fe substitution. Simple electrostatic rules allied with papk- ing considerations permit qualitative explanation of the structural distortions. The M(l) octahedron has six short shared edges to give a distorted and elongated trigonal antiprism. The M(2) octahedron has a triangle of three short shared edges. Metal-oxygen distances tend to compensate e.g., the longest Si-O distance and the shortest (MS,Fe)-O distance go to the same oxygen. INrnorucrroN The type structure of olivine was determined by Bragg and Brown (1926) on a forsterite crystal with composition Mgo noFeo.ro.Three- dimensionalrefinement of another forsterite crystal by Belov, Belova, Andrianova, and Smirnova (1951) yielded Si-O and M-O distancesfar outside the usual ranges for silicates. More recently Hanke a\d Zemarn (1963) determined the atomic parameters of forsterite from a two-di- mensionalanalysis, and Born (1964) followed this by showing that the observedposition ol M(2) falls on the maximum of the total attractive plus repulsiveenergy for half-ionizedatoms.