he minerals magnetite (Fe302) and hematite (Fe2O3) xygen. exist in equilibrium with atmospheric a. b. 4 Fe304 (s) + O2 (g) = 6 Fe2O3 (S) Kp = 2.5 x 1087 at 298 K Determine the partial pressure of oxygen at equilibrium for this reaction. The partial pressure of oxygen in air is 0.21 atm. In which direction proceed to get to equilibrium? c. At room temperature, both magnetite and hematite are stable long time. Using principles we have learned, why might this be so? will the reaction in air for a very, VERY

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The minerals magnetite (Fe302) and hematite (Fe2O3) exist in equilibrium with atmospheric
oxygen.
4 Fe304 (s) + O2 (g) = 6 Fe203 (s)
Kp = 2.5 × 1087 at 298 K
a. Determine the partial pressure of oxygen at equilibrium for this reaction.
b. The partial pressure of oxygen in air is 0.21 atm. In which direction
proceed to get to equilibrium?
At room temperature, both magnetite and hematite are stable
long time. Using principles we have learned, why might this be so?
C.
will the reaction
in air for a very, VERY
Transcribed Image Text:The minerals magnetite (Fe302) and hematite (Fe2O3) exist in equilibrium with atmospheric oxygen. 4 Fe304 (s) + O2 (g) = 6 Fe203 (s) Kp = 2.5 × 1087 at 298 K a. Determine the partial pressure of oxygen at equilibrium for this reaction. b. The partial pressure of oxygen in air is 0.21 atm. In which direction proceed to get to equilibrium? At room temperature, both magnetite and hematite are stable long time. Using principles we have learned, why might this be so? C. will the reaction in air for a very, VERY
Expert Solution
Step 1: Equilibrium constant

For any gaseous reaction at equilibrium,aA(g)+bB(g)cC(g)+dD(g)the equilibrium constant at constant pressure is given as,Kp=pCcpDdpAapBb

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