Critical Raw Materials Profiles
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Standard X-Ray Diffraction Powder Patterns
NBS MONOGRAPH 25 — SECTION 1 Standard X-ray Diffraction U.S. DEPARTMENT OF COMMERCE NATIONAL BUREAU OF STANDARDS THE NATIONAL BUREAU OF STANDARDS Functions and Activities The functions of the National Bureau of Standards are set forth in the Act of Congress, March 3, 1901, as amended by Congress in Public Law 619, 1950. These include the development and maintenance of the national standards of measurement and the provision of means and methods for making measurements consistent with these standards; the determination of physical constants and properties of materials; the development of methods and instruments for testing materials, devices, and structures; advisory services to government agencies on scien- tific and technical problems; invention and development of devices to serve special needs of the Government; and the development of standard practices, codes, and specifications. The work includes basic and applied research, development, engineering, instrumentation, testing, evaluation, calibration services, and various consultation and information services. Research projects are also performed for other government agencies when the work relates to and supplements the basic program of the Bureau or when the Bureau's unique competence is required. The scope of activities is suggested by the listing of divisions and sections on the inside of the back cover. Publications The results of the Bureau's research are published either in the Bureau's own series of publications or in the journals of professional and scientific societies. The Bureau itself publishes three periodicals available from the Government Printing Office: The Journal of Research, published in four separate sections, presents complete scientific and technical papers; the Technical News Bulletin presents summary and preliminary reports on work in progress; and Basic Radio Propagation Predictions provides data for determining the best frequencies to use for radio communications throughout the world. -
Physical and Chemical Properties of Germanium
Physical And Chemical Properties Of Germanium Moneyed and amnesic Erasmus fertilise her fatuousness revitalise or burrow incommunicatively. Creditable Petr still climbs: regarding and lissome Lazarus bully-off quite punctiliously but slums her filoplume devotedly. Zane still defilade venomous while improvident Randell bloodiest that wonderers. Do you for this context of properties and physical explanation of Silicon is sincere to metals in its chemical behaviour. Arsenic is extremely toxic, RS, carbon is the tongue one considered a full nonmetal. In nature, which name a widely used azo dye. Basic physical and chemical properties of semiconductors are offset by the energy gap between valence conduction! Other metalloids on the periodic table are boron, Batis ZB, only Germanium and Antimony would be considered metals for the purposes of nomenclature. Storage temperature: no restrictions. At room temperature, the semiconducting elements are primarily nonmetallic in character. This application requires Javascript. It has also new found in stars and already the atmosphere of Jupiter. Wellings JS, it is used as an eyewash and insecticide. He has studied in Spain and Hungary and authored many research articles published in indexed journals and books. What are oral health benefits of pumpkins? The material on this site may not be reproduced, germanium, the radiation emitted from an active device makes it locatable. Classify each statement as an extensive property must an intensive property. In germanium and physical chemical properties of the border lines from the! The most electronegative elements are at the nod in the periodic table; these elements often react as oxidizing agents. Atomic Volume and Allotropy of the Elements. -
The Separation of Germanium from Lead, Cadmium, and Zinc by Ion Exchange
Scholars' Mine Masters Theses Student Theses and Dissertations 1962 The separation of germanium from lead, cadmium, and zinc by ion exchange Myra Sue Anderson Follow this and additional works at: https://scholarsmine.mst.edu/masters_theses Part of the Chemistry Commons Department: Recommended Citation Anderson, Myra Sue, "The separation of germanium from lead, cadmium, and zinc by ion exchange" (1962). Masters Theses. 2730. https://scholarsmine.mst.edu/masters_theses/2730 This thesis is brought to you by Scholars' Mine, a service of the Missouri S&T Library and Learning Resources. This work is protected by U. S. Copyright Law. Unauthorized use including reproduction for redistribution requires the permission of the copyright holder. For more information, please contact [email protected]. THE SEPARATION OF GERMANIUM FROM LEAD, CADMIUM, AND ZINC BY ION EXCHANGE BY MYRA SUE ANDERSON A THESIS submitted to the faculty of the SCHOOL OF MINES AND METALLURGY OF THE UNIVERSITY OF MISSOURI In partial fulfillment of the requirements for the Degree of MASTER OF SCIENCE IN CHEMISTRY Rolla, Missouri 1962 Approved by (advisor) //f 11 TABLE OF CONTENTS Page List of Illustrations Iv List of Tables V Introduction 1 Review of the Literature 2 Separation Methods for Germanium 2 Analytical Methods for Germanium 3 Germanium Complexes Suitable for Ion Exchange 6 Ion Exchange Resins 7 Ion Exchange Theory 9 Ion Exchange Studies of Germanium 15 Experimental 17 Materials 17 Apparatus 18 Analytical Methods 19 Anion Exchange Studies 21 Cation Exchange Studies -
OCCURRENCE of BROMINE in CARNALLITE and SYLVITE from UTAH and NEW MEXICO* Manrr Loursp Lrnosonc
OCCURRENCE OF BROMINE IN CARNALLITE AND SYLVITE FROM UTAH AND NEW MEXICO* Manrr Loursp LrNosonc ABSTRACT Both carnallite and sylvite from Eddy County, New Mexico, contain 0.1 per cent of bromine. The bromine content of these minerals from Grand county, utah, is three times as great. No bromine was detected in halite, polyhalite, l5ngbeinite, or anhydrite from New Mexico. Iodine was not detected in any of these minerals. on the basis of the bromine content of the sylvite from New Mexico, it is calculated that 7,000 tons of bromine were present in potash salts mined from the permian basin during the period 1931 to 1945. INrnooucrroN The Geological Survey has previously made tests for bromine and iodine in core samples of potash salts from New Mexico.r Bromine was found to be present in very small amounts. No systematic quantitative determinations were made, nor was the presenceof bromine specificalry correlated with quantitative mineral composition. Sections of potash core from four recently drilled wells and selected pure saline minerals from Eddy County, New Mexico, together with two cores from Grand County, Utah, were therefore analyzed for their bromine and iodine content. The percentage mineral composition was then correlated with the bromine content. rt was found that bromine was restricted to carnall- ite and sylvite. fodine was not detected in any of the samples analyzed. If present, its quantity must be less than .00570. Brine and sea water are the present commercial sourcesof bromine in the United States, though both Germany and U.S.S.R. have utilized potash salts as a source of bromine. -
Seepage Chemistry Manual
RECLAMManagAingTWateIr iOn theNWest Report DSO-05-03 Seepage Chemistry Manual Dam Safety Technology Development Program U.S. Department of the Interior Bureau of Reclamation Technical Service Center Denver, Colorado December 2005 Form Approved REPORT DOCUMENTATION PAGE OMB No. 0704-0188 The public reporting burden for this collection of information is estimated to average 1 hour per response, including the time for reviewing instructions, searching existing data sources, gathering and maintaining the data needed, and completing and reviewing the collection of information. Send comments regarding this burden estimate or any other aspect of this collection of information, including suggestions for reducing the burden, to Department of Defense, Washington Headquarters Services, Directorate for Information Operations and Reports (0704-0188), 1215 Jefferson Davis Highway, Suite 1204, Arlington, VA 22202-4302. Respondents should be aware that notwithstanding any other provision of law, no person shall be subject to any penalty for failing to comply with a collection of information if it does not display a currently valid OMB control number. PLEASE DO NOT RETURN YOUR FORM TO THE ABOVE ADDRESS. 1. REPORT DATE (DD-MM-YYYY) 2. REPORT TYPE 3. DATES COVERED (From - To) 12-2005 Technical 4. TITLE AND SUBTITLE 5a. CONTRACT NUMBER Seepage Chemistry Manual 5b. GRANT NUMBER 5c. PROGRAM ELEMENT NUMBER 6. AUTHOR(S) 5d. PROJECT NUMBER Craft, Doug 5e. TASK NUMBER 5f. WORK UNIT NUMBER 7. PERFORMING ORGANIZATION NAME(S) AND ADDRESS(ES) 8. PERFORMING ORGANIZATION REPORT Bureau of Reclamation, Technical Service Center, D-8290, PO Box 25007, NUMBER Denver CO 80225 DSO-05-03 9. SPONSORING/MONITORING AGENCY NAME(S) AND ADDRESS(ES) 10. -
Chlorine and Bromine Isotope Evolution Within a Fully Developed Upper Permian Natural Salt Sequence
Published in “Geochimica et Cosmochimica Acta” volume 245, pages 316-326. DOI: https://doi.org/10.1016/j.gca.2018.11.010. Use the above information when citing this article. Chlorine and bromine isotope evolution within a fully developed Upper Permian natural salt sequence HGM Eggenkampa,*, P Louvatb, J Griffioenc,d, P Agriniera aÉquipe de Géochimie des Isotopes Stables, Institut de Physique du Globe de Paris, Sorbonne Paris Cité, UMR 7154, CNRS, 1 rue Jussieu, 75238 Paris Cedex 05, France bÉquipe de Géochimie des Enveloppes Externes, Institut de Physique du Globe de Paris, Sorbonne Paris Cité, UMR 7154, CNRS, 1 rue Jussieu, 75238 Paris Cedex 05, France cTNO Geological Survey of the Netherlands, P.O. Box 80015, Utrecht, The Netherlands dCopernicus Institute of Sustainable Development, Utrecht University, P.O. Box 80115, Utrecht, The Netherlands *Corresponding author, email [email protected] Abstract The behaviour of chlorine and bromine isotopes in evaporite deposits differs significantly. We studied the isotope variations of both elements in a fully developed natural salt sequence from Zechstein evaporite deposits (Wuchiapingian, Upper Permian) in the Northern Netherlands. We observed that the Cl isotope variations follow previously predicted characteristics, showing slightly positive δ37Cl (relative to seawater) in halite (NaCl) dominated layers (up to +0.05 ‰), decreasing to moderately negative values in carnallite (KMgCl3•6H2O) and bischofite (MgCl2•6H2O) dominated layers (down to -0.55 ‰). Bromine isotope variations, the first ever measured in marine evaporite samples, show a different characteristic. δ81Br values 1 of 27 decrease quickly in layers dominated by halite (from +0.2 to -0.5 ‰) and increase again in layers dominated by carnallite and bischofite (up to - 0.1±0.2‰). -
Reflectance Spectral Characteristics of Minerals in the Mboukoumassi
minerals Article Reflectance Spectral Characteristics of Minerals in the Mboukoumassi Sylvite Deposit, Kouilou Province, Congo Xian-Fu Zhao 1,2, Zong-Qi Wang 1,*, Jun-Ting Qiu 3,* and Yang Song 2 1 Ministry of Land and Resources Key Laboratory of Metallogeny and Mineral Assessment, Institute of Mineral Resources, Chinese Academy of Geological Sciences, Beijing 100037, China; [email protected] 2 School of Earth Sciences and Resources, China University of Geosciences, Beijing 100083, China; [email protected] 3 National Key Laboratory of Science and Technology on Remote Sensing Information and Image Analysis, Beijing Research Institute of Uranium Geology, Beijing 100029, China * Correspondence: [email protected] (Z.-Q.W.); [email protected] (J.-T.Q.); Tel.: +86-10-82251207 (Z.-Q.W.); +86-10-64962683 (J.-T.Q.) Academic Editor: Dimitrina Dimitrova Received: 20 March 2016; Accepted: 23 May 2016; Published: 14 June 2016 Abstract: This study presents reflectance spectra, determined with an ASD Inc. TerraSpec® spectrometer, of five types of ore and gangue minerals from the Mboukoumassi sylvite deposit, Democratic Republic of the Congo. The spectral absorption features, with peaks at 999, 1077, 1206, 1237, 1524, and 1765 nm, of the ore mineral carnallite were found to be different from those of gangue minerals. Spectral comparison among carnallite samples from different sylvite deposits suggests that, in contrast to spectral shapes, the absorption features of carnallite are highly reproducible. Heating of carnallite to 400 and 750˝C, and comparing the spectra of heated and non-heated samples, indicates that spectral absorption is related to lattice hydration or addition of hydroxyl. -
Solmat-D-17-00752R1
Elsevier Editorial System(tm) for Solar Energy Materials and Solar Cells Manuscript Draft Manuscript Number: SOLMAT-D-17-00752R1 Title: Development of low-cost inorganic salt hydrate as a thermochemical energy storage material Article Type: Full Length Article Keywords: thermochemical storage material; bischofite; isothermal kinetics; dehydration reaction; salt hydrate Corresponding Author: Dr. Svetlana Ushak, Doctor in Chemistry Corresponding Author's Institution: University of Antofagasta First Author: Veronica Mamani Order of Authors: Veronica Mamani; Andrea Gutierrez; Svetlana Ushak, Doctor in Chemistry Abstract: Thermochemical storage is based on a reversible chemical reaction; energy can be stored when an endothermic chemical reaction occurs and then, energy is released when it is reversed in an exothermic reaction. According to literature and based on the energy storage density (esd), MgCl2·6H2O is a promising candidate material for thermochemical energy storage. Bischofite is an inorganic salt obtained as a by-product material from extraction processes of non-metallic minerals, from Salar de Atacama in Chile, containing approximately 95% of MgCl2·6H2O. Thus, the purpose of this study was to characterize the dehydration reaction of bischofite ore, studied as a low-cost thermochemical storage material. Thermogravimetric data for bischofite were obtained using a TGA instrument coupled to a DSC, at four different isotherms 70 °C, 80 °C, 90 °C and 100 °C. The results of conversion reaction (α-t) from the thermal dehydration experiments, demonstrated the first phase of dehydration with the loss of two water molecules. The study showed a typical sigmoid curve with a significant acceleration in the conversion at the beginning of the reaction until it reaches a maximum rate, where the curve keeps constant. -
Evaluation of Nacl and Mgcl2 Heat Exchange Fluids in a Deep Binary
Moore and Holländer Geotherm Energy (2021) 9:8 https://doi.org/10.1186/s40517-021-00190-3 RESEARCH Open Access Evaluation of NaCl and MgCl2 heat exchange fuids in a deep binary geothermal system in a sedimentary halite formation Kayla R. Moore* and Hartmut M. Holländer *Correspondence: [email protected] Abstract Department of Civil Halite formations are attractive geothermal reservoirs due to their high heat conductiv- Engineering, University of Manitoba, Winnipeg, MB ity, resulting in higher temperatures than other formations at similar depths. However, R3T 5V6, USA halite formations are highly reactive with undersaturated water. An understanding of the geochemical reactions that occur within halite-saturated formation waters can inform decision making regarding well construction, prevention of well clogging, for- mation dissolution, and thermal short-circuiting. Batch reaction and numerical 3-D fow and equilibrium reactive transport modeling were used to characterize the produced NaCl-brine in a well targeting a halite-saturated formation. The potential for inhibition of precipitation and dissolution using an MgCl2-brine and NaCl MgCl2-brine were also investigated. Within the injection well, heating of an NaCl-brine+ from 70 to 120 °C caused the solubility of halite to decrease, resulting in the potential dissolution of 1 0.479 mol kg− halite at the formation. Conversely, cooling from 120 to 100 °C in the 1 production well resulted in potential precipitation of 0.196 mol kg− halite. Concur- rent precipitation of anhydrite is also expected. Introduction of MgCl2 into the heat exchange brine, which has a common Cl− ion, resulted in a decreased potential for 1 dissolution by 0.290 mol kg− halite within the formation, as well as decreased precipi- tation within the production well, compared to the NaCl-brine. -
A Specific Gravity Index for Minerats
A SPECIFICGRAVITY INDEX FOR MINERATS c. A. MURSKyI ern R. M. THOMPSON, Un'fuersityof Bri.ti,sh Col,umb,in,Voncouver, Canad,a This work was undertaken in order to provide a practical, and as far as possible,a complete list of specific gravities of minerals. An accurate speciflc cravity determination can usually be made quickly and this information when combined with other physical properties commonly leads to rapid mineral identification. Early complete but now outdated specific gravity lists are those of Miers given in his mineralogy textbook (1902),and Spencer(M,i,n. Mag.,2!, pp. 382-865,I}ZZ). A more recent list by Hurlbut (Dana's Manuatr of M,i,neral,ogy,LgE2) is incomplete and others are limited to rock forming minerals,Trdger (Tabel,l,enntr-optischen Best'i,mmungd,er geste,i,nsb.ildend,en M,ineral,e, 1952) and Morey (Encycto- ped,iaof Cherni,cal,Technol,ogy, Vol. 12, 19b4). In his mineral identification tables, smith (rd,entifi,cati,onand. qual,itatioe cherai,cal,anal,ys'i,s of mineral,s,second edition, New york, 19bB) groups minerals on the basis of specificgravity but in each of the twelve groups the minerals are listed in order of decreasinghardness. The present work should not be regarded as an index of all known minerals as the specificgravities of many minerals are unknown or known only approximately and are omitted from the current list. The list, in order of increasing specific gravity, includes all minerals without regard to other physical properties or to chemical composition. The designation I or II after the name indicates that the mineral falls in the classesof minerals describedin Dana Systemof M'ineralogyEdition 7, volume I (Native elements, sulphides, oxides, etc.) or II (Halides, carbonates, etc.) (L944 and 1951). -
The Chemistry of Germanium, Tin and Lead
The Chemistry of Germanium, Tin and Lead Anil J Elias, IIT Delhi Relative natural abundance on the earths crust of group 14 elements are as follows which indicate the rareness of germanium Carbon 0.18% The major end uses for Silicon 27% germanium, worldwide, were Germanium 0.00014% estimated to be fiber-optic Tin 0.00022% systems, 30%; infrared optics, 25%; Lead 0.00099% polymerization catalysts, 25%; electronics and solar electric applications, 15%; and other (phosphors, metallurgy, and chemotherapy), 5%. The main compounds of commercial importance of germanium are germanium tetrachloride and germanium dioxide. Unlike silicon, germanium forms stable divalent compounds like GeCl2 and GeO. A major difference with silicon is the fact 2- - that it forms GeCl6 and GeCl3 . Zone-refined crystalline germanium typically is 99.9999 percent pure and impurities are typically less than 100 ppb, and electrically active impurities, less than 0.5 ppb. GeO2 is dissolved in concentrated HCl to make germanium tetrachloride (GeCl4) which is a fuming liquid similar to SiCl4 having a boiling point of 86.5 C. The GeCl4 is purified by fractional distillation in glass or fused quartz equipments. The purified GeCl4 is hydrolyzed with deionized water to yield GeO2. After drying, the GeO2 is reduced with hydrogen at 760° C to form germanium metal powder, which is then melted and cast into bars, known as first-reduction bars. These bars are then zone-refined to polycrystalline metal that typically contains less than 100 ppb total impurities and less than 0.5 ppb electrically active impurities. Six salient properties of germanium which differ from that of silicon makes the foundations for all its applications. -
Thermophysical Characterization of a By-Product from the Non-Metallic Industry As Inorganic PCM
Thermophysical characterization of a by-product from the non-metallic industry as inorganic PCM Svetlana Ushak1,2,*, Andrea Gutierrez1, Hector Galleguillos1,2, Angel G. Fernandez1,2, Luisa F. Cabeza3, Mario Grágeda1,2 1 Department of Chemical Engineering and Mineral Processing and Center for Advanced Study of Lithium and Industrial Minerals (CELiMIN), Universidad de Antofagasta, Campus Coloso, Av. Universidad de Antofagasta 02800, Antofagasta, Chile. *[email protected] 2 Solar Energy Research Center (SERC-Chile), Av Tupper 2007, Piso 4, Santiago, Chile 3 GREA Innovació Concurrent, Universitat de Lleida, Edifici CREA, Pere de Cabrera s/n, 25001, Lleida, Spain Abstract Physical characterization and thermal properties of bischofite, a by-product from the non- metallic industry, were determined and compared with those to MgCl2·6H2O with the idea of using it as phase change material in thermal energy storage applications. The melting point and heat of fusion were measured in the temperature range from 30°C to 150°C, where Tfus and ΔHfus were 100°C and 115 kJ/kg for bischofite, and 114.5°C and 135 kJ/kg for MgCl2·6H2O. The solid heat capacity was determined from 25°C to 60°C, being 2.1 kJ/(kg·K) at 60°C for both samples. The measurements of the liquid heat capacity of bischofite were done from 105°C to 113°C and the Cp showed linear increase from 5.61 kJ/(kg·K) to 9.01 kJ/(kg·K). The thermal stability test (30 heating/cooling cycles) of bischofite and MgCl2·6H2O shows subcooling of about 37K and 29K, respectively.