It should be determined for the largest intermolecular forces among the following compounds. . Concept introduction: London dispersion forces: These forces are often found in the halogen ( F 2 and I 2 ), the Nobel gases ( Ne and Ar ) and other non-polar molecule, such as carbon dioxide and methane. London dispersion forces are first observes in London so it’s named like this. This is the part of Vander Waals forces, or weak intermolecular attractions.

Question

An expression for the root mean square velocity, vrms, of a gas was derived. Using Maxwell’s velocity distribution, one can also calculate the mean velocity and the most probable velocity (mp) of a collection of molecules. The equations used for these two quantities are vmean=(8RT/πM)1/2 and vmp=(2RT/M)1/2 These values have a fixed relationship to each other.(a) Arrange these three quantities in order of increasing magnitude.(b) Show that the relative magnitudes are independent of the molar mass of the gas.(c) Use the smallest velocity as a reference for establishing the order of magnitude and determine the relationship between the larger and smaller values.

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Question

Chapter 11.4, Problem 2RC

Interpretation Introduction

Interpretation: It should be determined for the largest intermolecular forces among the following compounds. .

Concept introduction:

London dispersion forces:

These forces are often found in the halogen ( F2 and I2 _), the Nobel gases (Ne and Ar) and other non-polar molecule, such as carbon dioxide and methane.

London dispersion forces are first observes in London so it’s named like this.

This is the part of Vander Waals forces, or weak intermolecular attractions.

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