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Use a computer to plot formula 2.22directly, as follows. Define z=q_{A}/q, so that (1-z)=q_{B}/q. Then, aside from an overall constant that we'll ignore, the multiplicity function is [4z(1-z)]N, where zranges from 0to1and the factor of 4ensures that the height of the peak is equal to 1for any N. Plot this function forN=1,10,100,1000, and 10,000. Observe how the width of the peak decreases asNincreases.

Short Answer

Expert verified

The width of the peak decreases as Nincreases.

Step by step solution

01

High temperature 

For large systems at high temperatures, so that q>>Nwe have the approximate formula:

qeNN

If we now have two such solids and allow them to interact, the number of microstates for the combined system for any given macrostate (that is, a given division of the total energy q=q_{A}+q_{B} between the two solids) is just the product of the numbers for the two separate solids:

qAeNANAqBeNBNB

We've already seen that the most probable state for a pair of interacting solids is the state in which the energy quanta are distributed evenly between the two systems, so that qAqB=NANB Our goal is to investigate how likely it is that the distribution of energy will deviate significantly from this most probable state. To make things simpler, we'll take N_{A}=NB=Nso that both solids are the same size. Then:

eqANNeqBNN=e2N2NqAqBN

02

The shape of this curve

but, q_{B}=q-q_{A}, so:

e2N2NqAq-qAN

With Nheld constant, the shape of this curve is determined by the qAq-qAN, factor. If we pull out a factor of q2, we get:

qAq-qAN=q2qAq1-qAqNqAq-qAN=q2NqAq1-qAqN

qAq-qAN=qqAqq1-qAqN

let, z=qAq, we get:

qAq-qAN=q2N[z(1-z)]N

We can get a feel for how the curve's shape changes as we increase Nby plotting

[z(1-z)]N

for several values ofN

03

Graph of vertical change

zitself ranges from 0to 1and z(1-z)has a maximum value of 0.25a0.25t z=0.5, so we can scale the graph to a vertical range of 0to 1by inserting a factor of 4inside the parentheses. That is, we plot:

(4z(1-z))N

I used python to draw the graph, the code is illustrated in following picture

04

Shape of diagram

05

Curves of violet

The curves are forN=1N=10 (blue), (orange), N=100(green), N=1000(red) and N=10000(violet)

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Most popular questions from this chapter

Fun with logarithms.
a Simplify the expressionealnb. (That is, write it in a way that doesn't involve logarithms.)
b Assuming that b<<a, prove that ln(a+b)(lna)+(b/a). (Hint: Factor out the afrom the argument of the logarithm, so that you can apply the approximation of part d of the previous problem.)

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?

Consider a system of two Einstein solids, with N{A} = 300, N{B} = 200 and q{total} = 100 (as discussed in Section 2.3). Compute the entropy of the most likely macrostate and of the least likely macrostate. Also compute the entropy over long time scales, assuming that all microstates are accessible. (Neglect the factor of Boltzmann's constant in the definition of entropy; for systems this small it is best to think of entropy as a pure number.) 65

Find an expression for the entropy of the two-dimensional ideal gas considered in Problem 2.26. Express your result in terms of U,AandN.

How many possible arrangements are there for a deck of 52playing cards? (For simplicity, consider only the order of the cards, not whether they are turned upside-down, etc.) Suppose you start w e in the process? Express your answer both as a pure number (neglecting the factor of k) and in SI units. Is this entropy significant compared to the entropy associated with arranging thermal energy among the molecules in the cards?

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