Consider again the system of two large, identical Einstein solids treated in Problem 2.22.

(a) For the case N=1023, compute the entropy of this system (in terms of Boltzmann's constant), assuming that all of the microstates are allowed. (This is the system's entropy over long time scales.)

(b) Compute the entropy again, assuming that the system is in its most likely macro state. (This is the system's entropy over short time scales, except when there is a large and unlikely fluctuation away from the most likely macro state.)

(c) Is the issue of time scales really relevant to the entropy of this system?

(d) Suppose that, at a moment when the system is near its most likely macro state, you suddenly insert a partition between the solids so that they can no longer exchange energy. Now, even over long time scales, the entropy is given by your answer to part (b). Since this number is less than your answer to part (a), you have, in a sense, caused a violation of the second law of thermodynamics. Is this violation significant? Should we lose any sleep over it?

Short Answer

Expert verified

(a) The entropy of this method , assuming that each one of the microstates are allowed Stotal=3.826JK1

(b) The entropy again, assuming that the system in its presumably macro state Smp=3.826JK1

(c) The entropy is given by , but over while scales it's given by which is ever slightly larger than .Smp

(d) Placea superb excellent resistance between two surfaces, keeping them from transmitting energy. In effect, this shows that the model is stuck in its current condition.

Step by step solution

01

Einstein Spheres (a)

(a) Suppose two big, similar Einstein spheres, every with Nclocks and q=2Namount of energy. We had (from issue 2.22) for the state during which all business can make are able:

Ωtotal24N8πN

This complete agency's volatility is:

Stotal=klnΩtotal

If we modify Ωtotalwith , we get:

Stotal=kln24N8πN

ln(ab)=ln(a)+ln(b),lnab=ln(a)ln(b)andlnab=bln(a)

Stotal=k4Nln(2)12ln(8πN)

k=1.38×1023JK1andN=1023:

Stotal=1.38×10234×1023×ln(2)12×ln8π×1023

Stotal=3.826JK1

02

Two solids (b)

(b) Its presumably situation, that the energy is spread evenly between the 2 solids, had a redundancy (from problem 2.22):

Ωmp24N4πN

The volatility of its most frequent state was even as follows:

Smp=klnΩmp

Assuming we swap Ωmp, we get:

Smp=kln24N4πN

Stotal=k[4Nln(2)ln(4πN)]

k=1.38×1023JK1andN=1023

Smp=1.38×10234×1023×ln(2)×ln4π×1023

Smp=3.826JK1

Hence, whether object is viewed as either an unified location with all feasible microstates or as 2 independent systems for his or her most plausible shape, the energy is virtually defined solely more by 24Nvariable.

03

Entropy (c) and (d)

(c) The entity is liberal to pursue each one of the microstates included in Stotal, over longer timeframes, yet it's extremely likely to be in or near its most frequent state at any given time. Thus, we may claim that the entropy is supplied by Smp over small scales, while it's given by Stotal very long time scales, which has become so marginally bigger than Smp.

(d) Think about a situation within which we elect some extent t so when system is in its possibly efficient than one (i.e., the entropy is Smp) and so place a wonderful resistance between two surfaces, keeping them from transmitting energy. In effect, this shows that the model is stuck in its current condition.

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Most popular questions from this chapter

For either a monatomic ideal gas or a high-temperature Einstein solid, the entropy is given by times some logarithm. The logarithm is never large, so if all you want is an order-of-magnitude estimate, you can neglect it and just say . That is, the entropy in fundamental units is of the order of the number of particles in the system. This conclusion turns out to be true for most systems (with some important exceptions at low temperatures where the particles are behaving in an orderly way). So just for fun, make a very rough estimate of the entropy of each of the following: this book (a kilogram of carbon compounds); a moose of water ; the sun of ionized hydrogen .

Use Stirling's approximation to find an approximate formula for the multiplicity of a two-state paramagnet. Simplify this formula in the limit NNto obtain ΩNe/NN. This result should look very similar to your answer to Problem 2.17; explain why these two systems, in the limits considered, are essentially the same.

For each of the following irreversible processes, explain how you can tell that the total entropy of the universe has increased.
a Stirring salt into a pot of soup.
b Scrambling an egg.
c Humpty Dumpty having a great fall.
d A wave hitting a sand castle.
e Cutting down a tree.
fBurning gasoline in an automobile.

The mixing entropy formula derived in the previous problem actually applies to any ideal gas, and to some dense gases, liquids, and solids as well. For the denser systems, we have to assume that the two types of molecules are the same size and that molecules of different types interact with each other in the same way as molecules of the same type (same forces, etc.). Such a system is called an ideal mixture. Explain why, for an ideal mixture, the mixing entropy is given by

ΔSmixing=klnNNA

where Nis the total number of molecules and NAis the number of molecules of type A. Use Stirling's approximation to show that this expression is the same as the result of the previous problem when both Nand NAare large.

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.

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