Chapter 3: Q. 3.17 (page 103)
Verify every entry in the third line of Table 3.2 (starting with .
Short Answer
All the entries in the third line are verified.
Chapter 3: Q. 3.17 (page 103)
Verify every entry in the third line of Table 3.2 (starting with .
All the entries in the third line are verified.
All the tools & learning materials you need for study success - in one app.
Get started for freeIn Problem 1.55 you used the virial theorem to estimate the heat capacity of a star. Starting with that result, calculate the entropy of a star, first in terms of its average temperature and then in terms of its total energy. Sketch the entropy as a function of energy, and comment on the shape of the graph.
Consider a monatomic ideal gas that lives at a height z above sea level, so each molecule has potential energy in addition to its kinetic energy.
(a) Show that the chemical potential is the same as if the gas were at sea level, plus an additional term :
(You can derive this result from either the definition or the formula
(b) Suppose you have two chunks of helium gas, one at sea level and one at height z, each having the same temperature and volume. Assuming that they are in diffusive equilibrium, show that the number of molecules in the higher chunk is
in agreement with the result of Problem 1.16.
In Problem you computed the entropy of an ideal monatomic gas that lives in a two-dimensional universe. Take partial derivatives with respect to , and N to determine the temperature, pressure, and chemical potential of this gas. (In two dimensions, pressure is defined as force per unit length.) Simplify your results as much as possible, and explain whether they make sense.
Consider an Einstein solid for which both N and q are much greater than . Think of each oscillator as a separate "particle."
(a) Show that the chemical potential is
role="math" localid="1646995468663"
(b) Discuss this result in the limits and , concentrating on the question of how much increases when another particle carrying no energy is added to the system. Does the formula make intuitive sense?
In solid carbon monoxide, each CO molecule has two possible orientations: CO or OC. Assuming that these orientations are completely random (not quite true but close), calculate the residual entropy of a mole of carbon monoxide.
What do you think about this solution?
We value your feedback to improve our textbook solutions.