Confused by an exercise on the subject of chemical equilibrium

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SUMMARY

This discussion centers on the confusion surrounding an exercise from the "Introduction to Chemical Equilibrium" course, specifically regarding gas reactions and their concentrations. The concept of "fugacity" was raised but is not included in the exercise materials. Participants clarified that the concentration of a gas can be understood similarly to general concentration, defined as the number of moles per volume, and can be converted using the ideal gas law, particularly focusing on the starting pressure of the system.

PREREQUISITES
  • Understanding of the ideal gas law
  • Basic knowledge of gas concentrations and partial pressures
  • Familiarity with chemical equilibrium concepts
  • Introduction to fugacity in thermodynamics (optional for this exercise)
NEXT STEPS
  • Study the ideal gas law and its applications in chemical reactions
  • Research the concept of fugacity and its relevance in gas mixtures
  • Explore the relationship between concentration and partial pressure in gases
  • Review exercises related to chemical equilibrium for practical understanding
USEFUL FOR

Students of chemistry, particularly those studying chemical equilibrium, educators preparing course materials, and anyone seeking to clarify concepts related to gas reactions and their concentrations.

samy4408
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Homework Statement
I assume that they talk about partial pressure and calculate it instead of the concentration .
Relevant Equations
PV = nRT
1649548997424.png

Hello , i am a little confused about this exercise because we talk about gases reaction and we are asked about the concentrations
P.S : i have other questions that depends on your answer .
Thanks .
 
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Are you familiar with the concept of "fugacity?"
 
no,this exercise is from the problem set of a course called "introduction to chemical equilibrium " and the concept of "fugacity" is not mentioned .
 
Last edited:
Concentration of a gas in a mixture is not much different from a concentration in general - just number of moles in a volume. Can be reasonably easily interconverted with the partial pressure.
 
From the ideal gas law, what is the starting pressure?
 

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