Compute the entropy of a mole of helium at room temperature and atmospheric pressure, pretending that all the atoms are distinguishable. Compare to the actual entropy, for indistinguishable atoms, computed in the text.
We have to find the entropy of helium atom at room temperature and atmospheric pressure.
The entropy of an ideal gas is given by
where V is the volume
U is the energy
N is the number of molecules
m is the mass of a single molecule
h is Planck’s constant.
The molecules are indistinguishable, so for any configuration of the molecules in position and momentum space, interchanging any of the molecules makes no difference. This assumption introduces the factor of N! in the denominator of the multiplicity function :
If we assume that the molecules are all distinguishable, we can follow through the derivation, but without the N!, we start with
We find that the term in 1 changes to and the factor in the logarithm loses its N, so we get
Textbook: An Introduction to Thermal Physics
Author: Daniel V. Schroeder
Since the solution to 39P from 2 chapter was answered, more than 481 students have viewed the full step-by-step answer. An Introduction to Thermal Physics was written by and is associated to the ISBN: 9780201380279. This textbook survival guide was created for the textbook: An Introduction to Thermal Physics , edition: 1. The answer to “Compute the entropy of a mole of helium at room temperature and atmospheric pressure, pretending that all the atoms are distinguishable. Compare to the actual entropy, for indistinguishable atoms, computed in the text.” is broken down into a number of easy to follow steps, and 33 words. The full step-by-step solution to problem: 39P from chapter: 2 was answered by , our top Physics solution expert on 07/05/17, 04:29AM. This full solution covers the following key subjects: atoms, indistinguishable, entropy, distinguishable, helium. This expansive textbook survival guide covers 10 chapters, and 454 solutions.