Chemistry Confused by an exercise on the subject of chemical equilibrium

AI Thread Summary
The discussion revolves around confusion regarding an exercise related to gas reactions and their concentrations in the context of chemical equilibrium. Participants clarify that the concentration of a gas in a mixture is similar to general concentration, defined as the number of moles per volume, and can be converted to partial pressure using the ideal gas law. The concept of "fugacity" is not relevant to the exercise, as it is not covered in the course material. Additionally, there is a request for clarification on the starting pressure for the calculations. Understanding these principles is essential for solving the exercise effectively.
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
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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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