Compare average distance between molecules to size of N2

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SUMMARY

The discussion focuses on comparing the calculated volume of a single nitrogen molecule (N2) with its experimentally determined size, specifically the Van der Waals (VdW) radius. The calculated volume is 3.99x10^-23 m^3, leading to a cubic root of 3.42x10^-8 m. Participants clarify that the comparison should be made between the VdW radius, a one-dimensional measurement, and the edge length of the cubic volume occupied by the molecule in a gaseous state. The distinction between volume and length is emphasized, highlighting the need for precise understanding of molecular dimensions.

PREREQUISITES
  • Understanding of the Ideal Gas Law (Pv=nRt)
  • Knowledge of Van der Waals radius and its significance in molecular size
  • Familiarity with cubic volume calculations and dimensional analysis
  • Basic concepts of molecular structure and electron cloud distribution
NEXT STEPS
  • Research the calculation of Van der Waals radius for various molecules
  • Study the implications of molecular size on gas behavior and properties
  • Explore the relationship between molecular volume and intermolecular forces
  • Learn about experimental methods for measuring molecular dimensions
USEFUL FOR

Students in chemistry or physics, particularly those studying molecular dynamics, gas laws, and molecular size comparisons. This discussion is beneficial for anyone looking to deepen their understanding of molecular measurements and their implications in physical chemistry.

wololo
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Homework Statement


Capture.PNG

Homework Equations


Pv=nRt

The Attempt at a Solution


I already calculated V for a single molecule = 3.99x10^-23 m^3 and the cubic root of this volume gives 3.42x10^-8 m. However, I don't understand what I should do next. What does it mean to compare the value I obtained to the "size" of a molecule? Thanks
 
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I would start googling for "water molecule size". They want you to compare the volume calculated with experimental data describing the distance between atoms (plus some space for the electron cloud).
 
I looked up Van der Wall radius online (did not learn about it in class) and found how to measure the radius, diameter and volume of a specific molecule given it's experimentally measured constant b, but what puzzles me is that they ask me to compare the "size" (I assume van der wall volume?) of the molecule, a cubic meter value, with an unrelated one dimensional distance value. I feel as though they did not specify accurately enough what we need to do.
 
VdW radius is not a volume, it is length, just like the length you calculated. You are asked to compare the "radius" of a molecule (as determined experimentally) with the edge of a cube that such a molecule occupies in a gas. I see no ambiguity.
 

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