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For the reaction: Fe₂O3(s) + 3C0(g) = 2Fe(s) + 3CO₂(g) Equilibrium Constant K 100 0.0721 The following values of K are known. Temperature t/°C 250 1000 At 1120 °C for the reaction 2CO₂ (g) = 2CO(g) + O₂(g), K = 1.4 x 10-¹² bar. What equilibrium partial pressure of O₂ would have to be supplied to a vessel at 1120°C containing solid Fe₂O3 just to prevent the formation of Fe?

For the reaction: Fe₂O3(s) + 3C0(g) = 2Fe(s) + 3CO₂(g) Equilibrium Constant K 100 0.0721 The following values of K are known. Temperature t/°C 250 1000 At 1120 °C for the reaction 2CO₂ (g) = 2CO(g) + O₂(g), K = 1.4 x 10-¹² bar. What equilibrium partial pressure of O₂ would have to be supplied to a vessel at 1120°C containing solid Fe₂O3 just to prevent the formation of Fe?

Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter16: Spontaneity, Entropy, And Free Energy
Section: Chapter Questions
Problem 83AE: Consider the following system at equilibrium at 25C: PCl3(g)+Cl(g)PCl5(g)G=92.50KJ What will happen...
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For the reaction: Fe₂03 (s) + 3C0(g) = 2Fe(s) + 3CO₂ (g) The following values of K are known. Temperature t/°C 250 1000 Equilibrium Constant K 100 0.0721 At 1120 °C for the reaction 2CO₂ (g) = 2CO(g) + O₂(g), K = 1.4 × 10-¹² bar. What equilibrium partial pressure of O₂ would have to be supplied to a vessel at 1120°℃ containing solid Fe₂O3 just to prevent the formation of Fe?
Transcribed Image Text:For the reaction: Fe₂03 (s) + 3C0(g) = 2Fe(s) + 3CO₂ (g) The following values of K are known. Temperature t/°C 250 1000 Equilibrium Constant K 100 0.0721 At 1120 °C for the reaction 2CO₂ (g) = 2CO(g) + O₂(g), K = 1.4 × 10-¹² bar. What equilibrium partial pressure of O₂ would have to be supplied to a vessel at 1120°℃ containing solid Fe₂O3 just to prevent the formation of Fe?
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