Determining pressure at equilibrium with Kp

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SUMMARY

The discussion centers on calculating the equilibrium pressure of oxygen (P(O2)) in the reaction 4 Fe3O4(s) + O2(g) <----> 6 Fe2O3(s) with an equilibrium constant (Kp) of 2.5 x 10^87. The participant incorrectly assumed the relationship for Kp as 1/[O2]^2, leading to an erroneous calculation of P(O2). The correct approach requires understanding that Kp only includes gaseous components, and the participant is encouraged to revisit the equilibrium expression for accurate results.

PREREQUISITES
  • Understanding of chemical equilibrium concepts
  • Familiarity with equilibrium constants (Kp) and their calculations
  • Knowledge of significant figures in scientific calculations
  • Basic principles of gas laws and pressure relationships
NEXT STEPS
  • Review the derivation of the equilibrium constant expression for gaseous reactions
  • Study the concept of partial pressures in equilibrium systems
  • Learn about significant figures and their importance in chemical calculations
  • Explore examples of equilibrium calculations involving Kp and Kc
USEFUL FOR

Chemistry students, educators, and anyone involved in chemical equilibrium studies will benefit from this discussion, particularly those focusing on gas-phase reactions and equilibrium constants.

Emworthington
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Homework Statement


The minerals (Fe2So3) and (Fe3O4) exist in equilibrium with atmospheric oxygen.

4 Fe3O4(s) + O2(g) <----> 6 Fe2O3(s) kp = 2.5 x 10^87

Determine P(O2) at equilibrium

Homework Equations


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The Attempt at a Solution


Since the equilibrium constant can only have gases in it, I assumed that the equation would be
1/[O2]^2 so that the pressure would be 1/2.5*10^87. However, it's an online program and says that that (4*10^-88) is wrong. It also says that 2.5*10^87 is wrong. What else do you think I could do?
 
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No idea why 1/[O2]2 and not just 1/[O2], but perhaps that's just a typo.

Some of these HW programs are very anal about significant digits.
 

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