Some sulfur in present in coal in the form of pyrite (FeS2). When is burns , it pollutes the air with the combustion product SO2 , as shown by the following chemical equation. 4 FeS2(s) + 1102 (g) 2FE203(s) + 8SO2 (s) What mass of SO2 is produced by the combustion of 38.8 g of FeS2?

Some sulfur in present in coal in the form of pyrite (FeS2). When is burns , it pollutes the air with the combustion product SO2 , as shown by the following chemical equation. 4 FeS2(s) + 1102 (g) 2FE203(s) + 8SO2 (s) What mass of SO2 is produced by the combustion of 38.8 g of FeS2?

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter20: Environmental Chemistry-earth's Environment, Energy, And Sustainability

Section: Chapter Questions

Problem 40PS

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Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

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Some sulfur in present in coal in the form of pyrite (FeS2). When is burns , it
pollutes the air with the combustion product SO2 , as shown by the following
chemical equation.
4 FeS2(s) + 1102 (g)
2FE203(s) +8SO2 (s)
What mass of SO2 is produced by the combustion of 38.8 g of FeS2?

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4.90 Iron metal can be refined (rom the mineral hematite (Fe2O3). One way of converting the mineral to iron is to react it with carbon monoxide, as shown below: Fe2O3+3CO2Fe+3CO2 Because the hematite is obtained from various ores, it is usually not in a pure form. Suppose an iron manufacturer has 2.00 X 105 kg of ore available, and the ore is 93% Fe2O3 by mass. (There is no iron in the remaining 7% of the ore.) How many moles of Fe2O3are present in this ore? How many kg of pure iron could be obtained from this sample of ore? Assume that the process has a 100% yield and that excess CO is available.
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