How to Calculate Kp for a Sealed Vessel at Equilibrium?

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SUMMARY

The discussion focuses on calculating the equilibrium constant Kp for the reaction I2 (g) + Cl2 (g) <-> 2 ICl (g) at 2000K, given initial partial pressures of 0.3 atm for I2 and Cl2, and 0.5 atm for ICl. At equilibrium, the partial pressure of ICl increases by 52.8%, resulting in a final pressure of 0.764 atm. The user struggles with using an ICE table to determine the changes in partial pressures and correctly calculate Kp, as they encounter issues with the total pressure equation leading to cancellation.

PREREQUISITES
  • Understanding of chemical equilibrium concepts
  • Familiarity with the ICE (Initial, Change, Equilibrium) table method
  • Knowledge of calculating equilibrium constants (Kp) for gaseous reactions
  • Basic grasp of partial pressures in gas mixtures
NEXT STEPS
  • Review the concept of chemical equilibrium and Le Chatelier's principle
  • Practice constructing and using ICE tables for various equilibrium problems
  • Learn how to derive Kp from partial pressures in gas-phase reactions
  • Explore the impact of temperature changes on equilibrium constants
USEFUL FOR

Chemistry students, particularly those studying chemical equilibrium, and educators looking for examples of Kp calculations in gas-phase reactions.

veitch
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Homework Statement



Given a sealed vessel at 2000K, initially contains I2 (g) + Cl2 (g) <- -> 2 ICl (g) with partial pressures .3 atm, .3 atm and .5 atm respectively. At equilibrium the partial pressure of ICl has increased by 52.8% (so .764 atm)... calculate Kp. But that is one part that confuses me. Does only one pressure change?

Anyway.. I just did a Kp calculation for a previous question with no change and got the proper answer (it's given)... but using an ICE table in that question allowed me to solve for x to figure out the diffferent pressures... I tried to do that here but Got:

I2 Cl2 ICl
(.3-x) (.3-x) (.5+2x)

but if I add them together and equal to the total pressure (1.1 atm) ... everything cancels out. I admit I don't have a great understanding of pressures yet... any help would be greatly appreciated.
 
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All partial pressures change in this case.
 

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