Chalcopyrite (CuFeS2), is an important source of copper. A typicalchalcopyrite ore contains about0.75% Cu. What volume of sulfur dioxide at 25°C and 1 atm pressure isproduced when one boxcarg.load (4 x 10 ft³) of chalcopyrite ore (density = 2.6 ) is roasted?cm3Assume all the sulfur inthe ore is converted to SO2 and no other source of sulfur is present.Find the following: (do not express your answer in scientific notation, do not input the unit,space or comma, your answer should be in two decimal places) Find the following: (do not express your answer in scientific notation, do not input the unit,space or comma, your answer should be in two decimal places)a. mass in grams of the chalcopyrite ore =b. mass in grams of copper =c. no.of moles of SO, =mold. volume of SO2 =Note: Use the following in solving the problem1 ft 30.48 cmFor atomic weight (see periodic table in your module)LatmR= 0.082057molo N

Given the percent composition of Cu in the ore = 0.75 % Cu Given the volume of chalcopyrite ore…

Answered: Chalcopyrite (CuFeS2), is an important…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter16: Spontaneity Of Reaction

Section: Chapter Questions

Problem 48QAP

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What volume of sulfur dioxide at 25ᵒCand 1 atm pressure is produced when one boxcarload ( 4 x 10^3 cu.ft) of chalcopyrite ore (density =2.6 g/cu.cm) is roasted? Assume all the sulfur inthe ore is converted to SO2 and no other source ofsulfur is present.
Chalcopyrite (CuFeS2), is an important source of copper. A typical chalcopyrite ore contains about 0.75% Cu. What volume of sulfur dioxide at 25ᵒC and 1 atm pressure is produced when one boxcar load ( 4 x 10^3 cu.ft) of chalcopyrite ore (density = 2.6 g/cu.cm) is roasted? Assume all the sulfur in the ore is converted to SO2 and no other source of sulfur is present.
chalcopyrite (cufes2) is an important ore contains about 0.75% cu. what volume of sulfur oxide at 25 c and 1atm pressure is produced when one boxcar load (4x10^3 ft^3) of chalcopyrite ore (density = 2.6 g/cm^3) is roasted? assume all the sulfur in the ore is converted to so2 and no other source of sulfur is present.
Chalcopyrite (LaTeX: CuFeS_2C u F e S 2), is an important source of copper. A typical chalcopyrite ore contains about0.75% Cu. What volume of sulfur dioxide at 25ᵒCand 1 atm pressure is produced when one boxcarload ( 4 x 10^3 cu.ft) of chalcopyrite ore (density = 2.6 g/cu.cm) is roasted? Assume all the sulfur in the ore is converted to LaTeX: SO_2S O 2 and no other source of sulfur is presen
World production of chromite (FeCr₂O₄), the main ore ofchromium, was 1.5107metric tons in 2003. To isolate chro-mium, a mixture of chromite and sodium carbonate is heated inair to form sodium chromate, iron(III) oxide, and carbon diox-ide. The sodium chromate is dissolved in water, and this solutionis acidified with sulfuric acid to produce the less soluble sodiumdichromate. The sodium dichromate is filtered out and reduced with carbon to produce chromium(III) oxide, sodium carbonate,and carbon monoxide. The chromium(III) oxide is then reduced to chromium with aluminum metal. (a) Write balanced equations for each step. (b) What mass of chromium (in kg) could be pre-pared from the 2003 world production of chromite?
CH1CH2CH3CH4CH5CH6CH7CH8CH9CH10CH11CH12CH13CH14CH15CH16CH17CH18CH19CH20CH21CH22CH23 1QP2QP3QP4QP5QP6QP7QP8QP9QP10QP11QP12QP13QP14QP15QP16QP17QP18QP19QP20QP21QP22QP23QP24QP25QP26QP27QP28QP29QP30QP31QP32QP33QP34QP35QP36QP37QP38QP39QP40QP41CP42CP43CP44CP45CP Chalcopyrite, CuFeS2, is an important source of copper. A typical chalcopyrite ore contains about 0.75% Cu. What volume of sulfur dioxide at 25°C and 1.00 atm pressure is produced when one boxcar load (4.00 × 103 ft3) of chalcopyrite ore (d= 2.6 g/cm3) is roasted? Assume all the sulfur in the ore is converted to SO2 and no other source of sulfur is present
Oxyacetylene torches rely on a precise mixture of fuel (C2H2(g)) to oxygen to optimize the welding process. _ C2H2 (g) + _ O2 (g) ---> CO2 (g) + _H2O (g) Calculate the volume (in L) of O2(g) required to react completely with 14.5 L of acetylene. Assume both substances are at SATP.
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?
The most important commercial ore of chromiumis chromite (FeC r 2 O 4 ). One of the steps in theprocess used to extract chromium from the ore is thereaction of chromite with coke (carbon) to produceferrochrome (FeC r 2 ).2C(s) + FeC r 2 O 4 (s) → FeC r 2 (s) + 2C O 2 (g)What mole ratio would you use to convert from molesof chromite to moles of ferrochrome?
For the alloy Mg-45 wt% Pb alloy at 500 C, what is the weight percentage of Pb in liquid?
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.
Write a balanced equation for this process. Liquid potassium (k) is reacted with solid aluminium oxide (Al2O3) and potassium oxide(K2O) dust is produced.

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