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3. In a blast furnace, carbon monoxide (CO) is used to reduce ferric oxide (Fe,0,) to metallic iron, with carbon dioxide as a by-product. The equilibrium constant K, for the redox reaction is 19.9 at 1 000 K. If the equilibrium pressure of CO, is 2.4 atm, how much pressure is exerted by CO? Fe,O,(s) + 3CO(g) 2Fe(s) + 3CO,(g)

3. In a blast furnace, carbon monoxide (CO) is used to reduce ferric oxide (Fe,0,) to metallic iron, with carbon dioxide as a by-product. The equilibrium constant K, for the redox reaction is 19.9 at 1 000 K. If the equilibrium pressure of CO, is 2.4 atm, how much pressure is exerted by CO? Fe,O,(s) + 3CO(g) 2Fe(s) + 3CO,(g)

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter13: Electrochemistry
Section: Chapter Questions
Problem 13.101PAE
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3. In a blast furnace, carbon monoxide (CO) is used to reduce ferric oxide (Fe,0,) to metallic iron, with carbon dioxide as a by-product. The equilibrium constant K, for the redox reaction is 19.9 at 1000 K. If the equilibrium pressure of CO, is 2.4 atm, how much pressure is exerted by CO? Fe,O,(s) + 3CO(9) = 2Fe(s) + 3CO,lg)
Transcribed Image Text:3. In a blast furnace, carbon monoxide (CO) is used to reduce ferric oxide (Fe,0,) to metallic iron, with carbon dioxide as a by-product. The equilibrium constant K, for the redox reaction is 19.9 at 1000 K. If the equilibrium pressure of CO, is 2.4 atm, how much pressure is exerted by CO? Fe,O,(s) + 3CO(9) = 2Fe(s) + 3CO,lg)
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