21. Kinetic Theory of Ideal Gases

Mean Free Path of Gases

Chemistry of Gases (34 of 40) Mean Free Path: Basics

Mean Free Path

Example: Calculating the mean free path through air

Calculating Radius of Nitrogen

6.9 Mean Free Path, Diffusion, & Effusion of Gases

Mean Free Path, Mean Free Time, & Root Mean Square Velocity Formula   Chemistry & Physics Problems

<p>Laboratory environments can achieve pressures of 3.5×10<sup>-13</sup> atm and temperatures of 300K. Calculate the mean free path (in km) of air molecules, which you can assume are diatomic.</p>

Mean Free Path, Diffusion, and Effusion of Gases

Chemical Kinetics 1.4 - Mean Free Path

Calculate the mean free path of air molecules at 3.50 * 10^-13 atm and 300 K. (This pressure is readily attainable in the laboratory; see Exercise 18.23.) As in Example 18.8, model the air molecules as spheres of radius 2.0 * 10^-10 m.

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