How to approach this Brownian Motion Problems

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Homework Help Overview

The discussion revolves around understanding concepts related to Brownian motion and the ideal gas law, particularly the differences between various gas constants and their applications in equations. Participants are exploring the implications of these constants in the context of the problem presented.

Discussion Character

  • Conceptual clarification, Assumption checking

Approaches and Questions Raised

  • Participants are questioning the differences between Ra and R in the context of the ideal gas law and Boyle's law. There is an exploration of whether these constants are equivalent and how they relate to the equations provided.

Discussion Status

The discussion is ongoing, with participants offering clarifications about the ideal gas law and its variables. Some have expressed confusion regarding the interpretation of certain terms in the equations, indicating a productive exchange of ideas without a clear consensus yet.

Contextual Notes

There is mention of a specific problem attachment and a link to additional resources, suggesting that participants are working within the constraints of a homework assignment. The discussion also highlights a lack of clarity regarding the definitions of variables such as n and n0.

xiaozegu
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Why do you think there's a difference? Isn't it just the universal gas constant in both cases?
 
clamtrox said:
Why do you think there's a difference? Isn't it just the universal gas constant in both cases?

Is Bolye's law's Ra equal to the R in the PV=NRT?
Bolye's law is PV = RaT
 
xiaozegu said:
Is Bolye's law's Ra equal to the R in the PV=NRT?
Bolye's law is PV = RaT

Sorry, but that's gibberish. Read more carefully what is done.

The ideal gas law is PV = nRT, where n is the number of moles of gas, V is volume, p is pressure, T is temperature and R is the gas constant.

The form used in the book you quote has instead v = V/n, volume per mole, and reads Pv = RT.
 
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clamtrox said:
Sorry, but that's gibberish. Read more carefully what is done.

The ideal gas law is PV = nRT, where n is the number of moles of gas, V is volume, p is pressure, T is temperature and R is the gas constant.

The form used in the book you quote has instead v = V/n, volume per mole, and reads Pv = RT.

Thanks. But I still do not know how to interpret the n and n0 in the after equation. Isn't n is 1 mol?
 

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