A key step in the extraction of iron from its ore is shown below. FeO(s) + CO(g) = Fe(s) + CO2(g) Kp = 0.403 at 1000°C This step occurs in the 700° to 1200°C zone within a blast furnace. What are the equilibrium partial pressures of CO(g) and CO2(g) when 2.05 atm CO(g) and excess FeO(s) react in a sealed container at 1000°C?
A key step in the extraction of iron from its ore is shown below. FeO(s) + CO(g) = Fe(s) + CO2(g) Kp = 0.403 at 1000°C This step occurs in the 700° to 1200°C zone within a blast furnace. What are the equilibrium partial pressures of CO(g) and CO2(g) when 2.05 atm CO(g) and excess FeO(s) react in a sealed container at 1000°C?
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter12: Gaseous Chemical Equilibrium
Section: Chapter Questions
Problem 22QAP: Calculate K for the formation of methyl alcohol at 100C: CO(g)+2H2(g)CH3OH(g) given that at...
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A key step in the extraction of iron from its ore is shown below.
FeO(s) + CO(g) = Fe(s) + CO2(g) Kp = 0.403 at 1000°C
This step occurs in the 700° to 1200°C zone within a blast furnace. What are the equilibrium partial pressures of CO(g) and CO2(g) when 2.05 atm CO(g) and excess FeO(s) react in a sealed container at 1000°C?
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