Limestone(CaCO3) is used to remove acidic pollutants from smokestack flue gases in a sequence of decomposition-combination reactions. The limestone is heated to form lime (CaO), which reacts with sulfur dioxide to form calcium sulfite. Assuming a 70.5% yield in the overall reaction, what mass of limestone is required to remove all the sulfur dioxide formed by the combustion of 69000 kg coal that is 0.42 mass % sulfur?
Limestone(CaCO3) is used to remove acidic pollutants from smokestack flue gases in a sequence of decomposition-combination reactions. The limestone is heated to form lime (CaO), which reacts with sulfur dioxide to form calcium sulfite. Assuming a 70.5% yield in the overall reaction, what mass of limestone is required to remove all the sulfur dioxide formed by the combustion of 69000 kg coal that is 0.42 mass % sulfur?
Chemistry by OpenStax (2015-05-04)
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ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
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Chapter4: Stoichiometry Of Chemical Reactions
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Coal Combustion -- Limestone for SO2 Scrubbing
Limestone(CaCO3) is used to remove acidic pollutants from smokestack flue gases in a sequence of decomposition-combination reactions. The limestone is heated to form lime (CaO), which reacts with sulfur dioxide to form calcium sulfite. Assuming a 70.5% yield in the overall reaction, what mass of limestone is required to remove all the sulfur dioxide formed by the combustion of 69000 kg coal that is 0.42 mass % sulfur?
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