Be sure to answer all parts. A key step in the extraction of iron from its ore is FeO(s) + CO(g) = Fe(s) + CO2(g) Kp = 0.403 at 1,000°C This step occurs in the 700°C to 1,200°C zone within a blast furnace. What are the equilibrium partial pressures of CO(g) and CO2(g) when 1.2600 atm of CO(g) and excess FeO(s) react in a sealed container at 1000°C? Pco = atm PCO₂ atm

Chemistry: Principles and Reactions
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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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Be sure to answer all parts.
A key step in the extraction of iron from its ore is
FeO(s) + CO(g) = Fe(s) + CO2(g) Kp = 0.403 at 1,000°C
This step occurs in the 700°C to 1,200°C zone within a blast furnace. What are the equilibrium partial
pressures of CO(g) and CO2(g) when 1.2600 atm of CO(g) and excess FeO(s) react in a sealed container
at 1000°C?
Pco =
atm
PCO₂
atm
Transcribed Image Text:Be sure to answer all parts. A key step in the extraction of iron from its ore is FeO(s) + CO(g) = Fe(s) + CO2(g) Kp = 0.403 at 1,000°C This step occurs in the 700°C to 1,200°C zone within a blast furnace. What are the equilibrium partial pressures of CO(g) and CO2(g) when 1.2600 atm of CO(g) and excess FeO(s) react in a sealed container at 1000°C? Pco = atm PCO₂ atm
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