Copper is produced from chalcopyrite concentrate from a mixed type ore containing 1.2% CuFeS2 (chalcopyrite) and 6% Cu3 (CO3) 2 (OH) 2 (azurite) by sulfating roasting leaching method. 4 tons of chalcopyrite concentrate is roasted daily. If it is assumed that the amount of iron in the solution is 20% under the same conditions, how much copper is produced in 1 day?

Copper is produced from chalcopyrite concentrate from a mixed type ore containing 1.2% CuFeS2 (chalcopyrite) and 6% Cu3 (CO3) 2 (OH) 2 (azurite) by sulfating roasting leaching method. 4 tons of chalcopyrite concentrate is roasted daily. If it is assumed that the amount of iron in the solution is 20% under the same conditions, how much copper is produced in 1 day?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter19: The Chemistry Of The Main-group Elements

Section19.5: Extraction By Chemical Oxidation-reduction: Phosphorus, Bromine, And Iodine

Problem 19.3PSP

See similar textbooks

Similar questions

blast furnace makes pig iron containing 3.6% C, 1.4% Si and 95% Fe. The ore used contains 80% FE2O3, 12% SiO2 and 8% Al2O3. The coke analysis shows the presence of 10% SiO2 and 90% C. The flux used is pure CaCO3. The exit gases contain 28% CO and 14% CO2. The coke ratio is 1000 kg/t pig iron. Flux is 400 kg/t pig iron. Calculate per tonne of pig iron: (a) the weight of the slag made, (b) the weight of the ore used, (c) the composition of slag the air required at NTP.
Impure nickel, refined by smelting sulfide ores in a blast furnace, can be convertedinto metal from 99.90% to 99.99% purity by the Mond process. The primaryreaction involved in the Mond process is:Ni(s) + 4CO(g) ⇌ Ni(CO)4(g)In the second step of the Mond process, the gaseous Ni(CO)4 is isolated andheated to 227°C. The purpose of this step is to deposit as much nickel as possibleas pure solid (the reverse of the preceding reaction). Calculate the equilibriumconstant for the preceding reaction at 227°C.
One can view the blast furnace from a simple viewpoint as a process in which the principal reaction is: Fe2O3 + C → Fe + CO But some other undesirable side reactions occur, mainly Fe2O3 +C → FeO+CO After mixing 600 lb of carbon (coke) with 1.00 ton of pure iron oxide, Fe2O3, the process produces 1200 lb of pure iron, 183 lb of FeO and 85 lb of Fe2O3. Calculate the pounds of carbon used up and the pounds of CO produced per ton of Fe2O3 charged and the selectivity in this process (of Fe with respect to FeO).
A 1.1324 g sample of magnetite ore was dissolved in concentrated HCl to give a solution that contained a mixture of Fe2+ and Fe3+. Nitric acid was added and the solution was boiled for a few minutes, which converted all of the iron to Fe3+. The Fe3+ was then precipitated as Fe2O3*xH2O by addition of NH3. After filtration and washing, the residue was ignited at a high temp to give 0.5394 g of pure Fe2O3. What is the percent Fe and the percent Fe3O4 in the sample?
Which method of concentration of an ore is preferred in the following cases and why?(1) The ore has higher density particles mixed with a large bulk of low densityimpurities(2) The ore consists of copper sulphide intermixed with clay particles Give an example of amalgam
An ore containing magnetite, Fe3O4, was analysed by dissolving a 4.9 g sample in concentrated HCl, giving a mixture of Fe2+ and Fe3+. After adding HNO3 to oxidize any Fe2+ to Fe3+, the resulting solution was diluted with water and the Fe3+ precipitated as Fe(OH)3 by adding NH3. After filtering and rinsing, the residue was ignited, giving 2.8 g of pure Fe2O3. Calculate the %w/w Fe3O4 in the sample (Fe3O4 =231.54 g/mol, Fe2O3 = 159.69 g/mol)
(i) Name the method of refining of metals such as Germanium.(ii) In the extraction of Al, impure Al2O3 is dissolved in cone. NaOH to form sodium aluminate and leaving impurities behind. What is the name of this process?(iii) What is the role of coke in the extraction of iron from its oxides?
Describe the role of the following :(i) SiO2 in the extraction of copper from copper matte(ii) NaCN in froth floatation process
describe the important features of the microstructure for low carbon steel, medium carbon steel (annealing), medium carbon steel (normalizing), white cast iron, and ductile cast iron.
A prospector wants to know how much gold is in the ore that he has been mining. A sample weighing 11.2456 grams is dissolved in Aqua Regia (a mixture of HCl and HNO3). That sample is then transferred to a 200.00 mL volumetric flask and diluted to the mark with water. This is called solution 1. A volumetric pipet is used to transfer 10.00 mL of solution 1 to a second 500.00 mL volumetric flask. The second flask is filled to the mark resulting in solution 2. 5.00 mL of solution 2 is analyzed and found to contain 13.45 ppm Au. Answer each of the questions below. 1. What is the concentration of Au in solution 1. The units should be ppm 2. How many micrograms of Au are in the 5.00 mL sample that was measured? 3. How many micrograms of gold were in the 500.00 mL flask containing solution 2. 4. How many grams Au were in the flask containing solution 1 5. What is the %Au in the original sample?
5. Write a report on the element vanadium (v), where the report includes the properties and characteristics of the metal, its ores, its interactions, its modification methods, and the crystalline structures of the minerals
A sample of slag (ore tailings) from a blast furnace was analyzed to determine the SiO2 content. A sample of 0.5003 g of slag was decomposed with HCl, leaving a solid residue with a mass of 0.1414 g. The residue was subsequently treated with HF and H2SO4 and heated to convert all the SiO2 present in the sample to SiF4, which is volatile and was evaporated leaving a residue with a mass of 0.0183 g. Determine the percentage by mass (% m/m) of SiO2 in the sample.