Register to reply

Kinetic theory of gases

by abstrkt
Tags: gases, kinetic, theory
Share this thread:
abstrkt
#1
Nov22-05, 07:51 PM
P: 2
Two gas cylinders are identical. One contains the monatomic gas argon (Ar), and the other contains an equal mass of the monatomic gas radon (Rn). The pressures in the cylinders are the same, but the temperatures are different. Determine the ratio KEAvg,radon / KEAvg,argon of the average kinetic energy of a radon atom to the average kinetic energy of a argon atom.

I was thinking since P = NMV^2/3L^3 to set that equal to each other for the same pressure, but im lost on how to approach it from there. Any help will be appreciated. Thanks.
Phys.Org News Partner Science news on Phys.org
World's largest solar boat on Greek prehistoric mission
Google searches hold key to future market crashes
Mineral magic? Common mineral capable of making and breaking bonds
Physics Monkey
#2
Nov22-05, 08:15 PM
Sci Advisor
HW Helper
Physics Monkey's Avatar
P: 1,332
From the kinetic theory we have [tex] P V = \frac{2}{3} E [/tex] for monatomic ideal gases (a pretty good approximation for the noble gases). The answer is one step way.


Register to reply

Related Discussions
Kinetic theory of gases Introductory Physics Homework 2
Kinetic theory of gases Advanced Physics Homework 3
Kinetic Theory of gases Advanced Physics Homework 1