Chapter 3: Q. 3.19 (page 107)
Fill in the missing algebraic steps to derive equations 3.30, 3.31, and 3.33.
Short Answer
Thus the equations are derived to fill the missing steps.
Chapter 3: Q. 3.19 (page 107)
Fill in the missing algebraic steps to derive equations 3.30, 3.31, and 3.33.
Thus the equations are derived to fill the missing steps.
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Figure 3.3 shows graphs of entropy vs. energy for two objects, A and B. Both graphs are on the same scale. The energies of these two objects initially have the values indicated; the objects are then brought into thermal contact with each other. Explain what happens subsequently and why, without using the word "temperature."

In order to take a nice warm bath, you mix 50 liters of hot water at with 25 liters of cold water at . How much new entropy have you created by mixing the water?
Suppose you have a mixture of gases (such as air, a mixture of nitrogen and oxygen). The mole fraction of any species is defined as the fraction of all the molecules that belong to that species: . The partial pressure of species is then defined as the corresponding fraction of the total pressure: . Assuming that the mixture of gases is ideal, argue that the chemical potential of species in this system is the same as if the other gases were not present, at a fixed partial pressure .
A cylinder contains one liter of air at room temperature ( ) and atmospheric pressure . At one end of the cylinder is a massless piston, whose surface area is . Suppose that you push the piston in very suddenly, exerting a force of . The piston moves only one millimeter, before it is stopped by an immovable barrier of some sort.
(a) How much work have you done on this system?
(b) How much heat has been added to the gas?
(c) Assuming that all the energy added goes into the gas (not the piston or cylinder walls), by how much does the internal energy of the gas increase?
(d) Use the thermodynamic identity to calculate the change in the entropy of the gas (once it has again reached equilibrium).
In 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.
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