Bibliography: p. 14.
|Statement||by H. H. Dewing and A. A. Cochran.|
|Series||Report of investigations - Bureau of Mines ; 8322, Report of investigations (United States. Bureau of Mines) -- 8322.|
|Contributions||Cochran, A. A.|
|The Physical Object|
|Pagination||14 p. :|
|Number of Pages||14|
Sulfuric Acid Extraction Technique for Recovering Zinc and Sulfur from Sphalerite. The Bureau of Mines conducted a laboratory-scale investigation of a technique that produces zinc sulfate and elemental sulfur from sphalerite concentrates by reaction with sulfuric acid at deg to deg c and ambient pressure. Reaction with to Indium and zinc extraction from an indium-bearing zinc residue were investigated using sphalerite concentrate as a reductant in sulfuric acid medium. For economic and environmental reasons, many of the byproducts of extraction are reclaimed. Sulfur dioxide gas, for example, is captured and turned into sulfuric acid — which can then be used in the extraction process or sold for such purposes as fertiliser manufacture. Oxidised copper ores can be treated by hydrometallurgical extraction. The use of ozone as an oxidant for the direct leaching of zinc sulfide (sphalerite) concentrate in sulfuric acid medium under atmospheric pressure was explored. The influence of acid concentration, feed gas injection rate, particle size distribution, stirring speed, temperature and slurry density on zinc extraction efficiency was examined. The experimental results showed that the leaching.
This paper examines the influence of cobalt and silver ion concentration on the extraction and kinetics of zinc dissolution from sphalerite. The mechanism involves catalysis of a galvanic oxidation! reduction that produces elemental sulfur in place of SO2 gas. A 95% maximum zinc recovery was achieved under the experimental conditions. The apparent activation energy suggested . To produce sulfuric acid, the concentration of SO 2 in the flue gas must be sufficiently high. However, two stumbling blocks complicate the ability of roasting lead–zinc tailings to satisfy the requirements of the SO 2 concentration. One drawback is that the sulfur content of lead–zinc tailings is 10–26%, significantly less than the. Balaza et al. () chemically pre-leached chalcopyrite in a M Fe 2 (SO 4) 3 + M H 2 SO 4 solution at 90 °C for 5– min, and then contacted the pre-leach residue with Acidithiobacillus ferrooxidans bacteria to study the copper recovery. By the application of X-ray photoelectron spectroscopy (XPS), Balaza et al. () showed that the amount of elemental sulfur . Sulfuric acid extraction technique for recovering zinc and sulfur from sphalerite / By H. H. (H. Harvey) Dewing and joint author. A. A. (Andrew A.) Cochran. Abstract. Includes bibliographical references (p. 14).Mode of access: Internet Topics.
Sulfuric acid, dense, colorless, oily, corrosive liquid; one of the most important of all chemicals, prepared industrially by the reaction of water with sulfur trioxide. In one of its most familiar applications, sulfuric acid serves as the electrolyte in lead-acid storage batteries. Similar results were observed with sulfuric acid leaching of zinc silicate calcine and ferric sulfate leaching zinc sulfides by Souza et al. (34, 35). The decrease in the Zn leaching rate with the. Zinc is a chemical element with the symbol Zn and atomic number Zinc is a slightly brittle metal at room temperature and has a blue-silvery appearance when oxidation is removed. It is the first element in group 12 of the periodic some respects, zinc is chemically similar to magnesium: both elements exhibit only one normal oxidation state (+2), and the Zn 2+ and Mg 2+ ions are of. The proposed method takes advantage of the presence of sulfur in the processed material which upon roasting is converted to sulfuric acid (IV)—a leaching agent for selective extraction of zinc. The properly adjusted pH of the aqueous medium in which the leaching process is carried out is the key factor determining the quantitative and.