In a metallurgical process the mineral pyrite, FeS2, is roasted in air: FeS 2 +O 2 Fe 2 O 3 +SO 2 The SO 2 is then converted into H 2 SO 4 in the following reactions: 2SO 2 +O 2 2SO 3; SO 3 +H 2 SO 4 H 2 S 2 O 7; H 2 S 2 O 7 +H 2 O 2H 2 SO 4 Assuming the mineral is 24.0\%FeS 2 and the remainder is inert, what mass of H 2 SO 4 is produced if 155 g of the mineral is used?
In a metallurgical process the mineral pyrite, FeS2, is roasted in air: FeS 2 +O 2 Fe 2 O 3 +SO 2 The SO 2 is then converted into H 2 SO 4 in the following reactions: 2SO 2 +O 2 2SO 3; SO 3 +H 2 SO 4 H 2 S 2 O 7; H 2 S 2 O 7 +H 2 O 2H 2 SO 4 Assuming the mineral is 24.0\%FeS 2 and the remainder is inert, what mass of H 2 SO 4 is produced if 155 g of the mineral is used?
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.57QE
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In a metallurgical process the mineral pyrite, FeS2, is roasted in air: FeS 2 +O 2 Fe 2 O 3 +SO 2 The SO 2 is then converted into H 2 SO 4 in the following reactions: 2SO 2 +O 2 2SO 3; SO 3 +H 2 SO 4 H 2 S 2 O 7; H 2 S 2 O 7 +H 2 O 2H 2 SO 4 Assuming the mineral is 24.0\%FeS 2 and the remainder is inert, what mass of H 2 SO 4 is produced if 155 g of the mineral is used?
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