Many important metals occur as sulfide, arsenide, and antimonide minerals, especially in the Sudbury ineral complex. The first step in processing these ores involves "roasting" the ore in air to produce the metal r metal oxide, along with nonmetal oxides that can be serious pollutants if not trapped. Suppose that you roast 2.00 kg of the mineral polymidite, Ni3S4. The balanced equation for the reaction 6: 2 Ni3S4 + 11 0₂ →6 NiO + 8 SO₂ (a) How many kg of NiO can be produced? (b) How many kg of the pollutant SO₂ can be produced? (c) How many liters of air at 25°C are required for roasting? Assume that air contains 23% O₂ by mass, nd that the density of air at 25°C is 1.2 g/L. Molar masses: Ni3S4 304.3 g/mol NiO 74.69 g/mol SO₂ 64.06 g/mol

Many important metals occur as sulfide, arsenide, and antimonide minerals, especially in the Sudbury ineral complex. The first step in processing these ores involves "roasting" the ore in air to produce the metal r metal oxide, along with nonmetal oxides that can be serious pollutants if not trapped. Suppose that you roast 2.00 kg of the mineral polymidite, Ni3S4. The balanced equation for the reaction 6: 2 Ni3S4 + 11 0₂ →6 NiO + 8 SO₂ (a) How many kg of NiO can be produced? (b) How many kg of the pollutant SO₂ can be produced? (c) How many liters of air at 25°C are required for roasting? Assume that air contains 23% O₂ by mass, nd that the density of air at 25°C is 1.2 g/L. Molar masses: Ni3S4 304.3 g/mol NiO 74.69 g/mol SO₂ 64.06 g/mol

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter20: Transition Metals And Coordination Chemistry

Section: Chapter Questions

Problem 67E

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Many important metals occur as sulfide, arsenide, and antimonide minerals, especially in the Sudburymineral complex. The first step in processing these ores involves “roasting” the ore in air to produce the metalor metal oxide, along with nonmetal oxides that can be serious pollutants if not trapped.Suppose that you roast 1.00 kg of the mineral maucherite, Ni11As8. The balanced equation for thereaction is:2 Ni11As8 + 31 O2 → 22 NiO + 8 As2O5(a) How many kg of NiO can be produced?(b) How many kg of the pollutant As2O5 can be produced?(c) How many liters of air at 25°C are required for roasting? Assume that air contains 23% O2 by mass,and that the density of air at 25°C is 1.2 g/L.Molar masses: Ni11As8 1245.0 g/mol NiO 74.69 g/mol As2O5 229.84 g/mol
1. Many important metals occur as sulfide, arsenide, and antimonide minerals, especially in the Sudbury mineral complex. The first step in processing these ores involves "roasting" the ore in air to produce the metal or metal oxide, along with nonmetal oxides that can be serious pollutants if not trapped. Suppose that you roast 3.00 kg of the mineral shandite, Ni3Pb,S2. The balanced equation for the reaction is: 2 Ni3Pb2S2 + 9 02 → 6 NiO +4 PbO + 4 SO2 (a) How many kg of NiO can be produced? (b) How many kg of the pollutant PbO can be produced? (c) How many liters of air at 25°C are required for roasting? Assume that air contains 23% O2 by mass, and that the density of air at 25°C is 1.2 g/L. Molar masses: NizPb2S2 654.6 g/mol NiO 74.69 g/mol PbO 223.20 g/mol
A slag sample is known to contain all of its iron in the forms of FeO and Fe2O3. A sample of 1,000 g of the slag was dissolved in hydrochloric acid according to the usual method, then reduced with stannous chloride and finally titrated with a 0.02237 M solution of potassium permanganate, of which 28.59 mL were used. A second aliquot of the slag sample, weighing 1,500, was dissolved in a nitrogen atmosphere to further adjust the oxidation state of the iron, it was immediately titrated with the same potassium permanganate solution. If this second experiment required 15.60 mL of permanganate solution, calculate: a) The percentage of total iron in the slag. b) The percentages of the oxide FeO and Fe2O3
An ore containing magnetite, Fe3O4 was analyzed by dissolving a 1.5419 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 0.8525 g of pure Fe2O3. Calculate the %w/w Fe3O4 in the sample.
A 6.35 kg mixed-mineral sample contains chromite (FeCr2O4) as the only chromium-bearing ore. The sample is subjected to an industrial process, using a ferrosilicon alloy as a reducing agent, which quantitatively converts all of the chromium into 12.5 kg of a ferrochrome alloy (stainless steel) which is 15.4% Cr by mass. What is the percentage of chromite (FeCr2O4) in the original sample?
The minerals chalcocite (Cu2S) and malachite (CU2CO3(OH)2) are two primary sources of copper. What is the oxidation state of copper in each of these minerals .a O The oxidation state of copper in chalcocite is +1, and in malachite it is +1. .b O The oxidation state of copper in chalcocite is +1, and in malachite it is +2. .C The oxidation state of copper in chalcocite is +2, and in malachite it is +1 .d O The oxidation state of copper in chalcocite is +2, and in malachite it is +2.
Several transition metals are prepared by reduction of themetal halide with magnesium. Titanium is prepared by the Krollmethod, in which ore (ilmenite) is converted to the gaseous chlo-ride, which is then reduced to Ti metal by molten Mg. Assuming yields of 84% for step 1 and 93% for step 2,and an excess of the other reactants, what mass of Ti metal canbe prepared from 21.5 metric tons of ilmenite?
Even though most metal sulfides are sparingly soluble in water, their solubilities differ by several orders of magnitude. This difference is sometimes used to separate the metals by controlling the pH. Use the following data to find the pH at which you can separate 0.10 M Cu2+ and 0.10 M Ni2+:
Many transition metals and their compounds are used as catalysts. Given MnO2, FeCl3, Pt, and Ni, which would you select for producing CCl4 from CS2 and Cl2?
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.