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.
All the tools & learning materials you need for study success - in one app.
Get started for freeIn 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.
In Section 2.5 I quoted a theorem on the multiplicity of any system with only quadratic degrees of freedom: In the high-temperature limit where the number of units of energy is much larger than the number of degrees of freedom, the multiplicity of any such system is proportional to , where is the total number of degrees of freedom. Find an expression for the energy of such a system in terms of its temperature, and comment on the result. How can you tell that this formula for cannot be valid when the total energy is very small?
When the sun is high in the sky, it delivers approximately 1000 watts of power to each square meter of earth's surface. The temperature of the surface of the sun is about , while that of the earth is about .
(a) Estimate the entropy created in one year by the flow of solar heat onto a square meter of the earth.
(b) Suppose you plant grass on this square meter of earth. Some people might argue that the growth of the grass (or of any other living thing) violates the second law of thermodynamics, because disorderly nutrients are converted into an orderly life form. How would you respond?
What partial-derivative relation can you derive from the thermodynamic identity by considering a process that takes place at constant entropy? Does the resulting equation agree with what you already knew? Explain.
Experimental measurements of heat capacities are often represented in reference works as empirical formulas. For graphite, a formula that works well over a fairly wide range of temperatures is (for one mole)
where , and . Suppose, then, that a mole of graphite is heated at constant pressure from to . Calculate the increase in its entropy during this process. Add on the tabulated value of (from the back of this book) to obtain .
What do you think about this solution?
We value your feedback to improve our textbook solutions.