Learning Objectives

By the end of this section, you will be able to do the following:

Identify probabilities in entropy
Analyze statistical probabilities in entropic systems

The information presented in this section supports the following AP® learning objectives and science practices:

7.B.1.1 The student is able to construct an explanation, based on atomic-scale interactions and probability, of how a system approaches thermal equilibrium when energy is transferred to it or from it in a thermal process. (S.P. 6.2)

Photograph of many coins laid down on a surface, some with heads shown up and some with tails shown up.

Figure 15.40 When you toss a coin a large number of times, heads and tails tend to come up in roughly equal numbers. Why doesn't heads come up 100, 90, or even 80 percent of the time? (credit: Jon Sullivan, PDPhoto.org)

The various ways of formulating the second law of thermodynamics tell what happens rather than why it happens. Why should heat transfer occur only from hot to cold? Why should energy become ever less available to do work? Why should the universe become increasingly disorderly? The answer is that it is a matter of overwhelming probability. Disorder is simply vastly more likely than order.

When you watch an emerging rain storm begin to wet the ground, you will notice that the drops fall in a disorganized manner both in time and in space. Some fall close together, some far apart, but they never fall in straight, orderly rows. It is not impossible for rain to fall in an orderly pattern, just highly unlikely, because there are many more disorderly ways than orderly ones. To illustrate this fact, we will examine some random processes, starting with coin tosses.

Coin Tosses

What are the possible outcomes of tossing five coins? Each coin can land either heads or tails. On the large scale, we are concerned only with the total heads and tails and not with the order in which heads and tails appear. The following possibilities exist:

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\begin{matrix} 5 heads, 0 tails \\ 4 heads, 1 tail \\ 3 heads, 2 tails \\ 2 heads, 3 tails \\ 1 head, 4 tails \\ 0 head, 5 tails \end{matrix}

These are what we call macrostates. A macrostate is an overall property of a system. It does not specify the details of the system, such as the order in which heads and tails occur or which coins are heads or tails.

Using this nomenclature, a system of five coins has the six possible macrostates just listed. Some macrostates are more likely to occur than others. For instance, there is only one way to get five heads, but there are several ways to get three heads and two tails, making the latter macrostate more probable. Table 15.3 lists of all the ways in which five coins can be tossed, taking into account the order in which heads and tails occur. Each sequence is called a microstate—a detailed description of every element of a system.


	Individual microstates	Number of microstates
5 heads, 0 tails	HHHHH	1
4 heads, 1 tail	HHHHT, HHHTH, HHTHH, HTHHH, THHHH	5
3 heads, 2 tails	HTHTH, THTHH, HTHHT, THHTH, THHHT HTHTH, THTHH, HTHHT, THHTH, THHHT	10
2 heads, 3 tails	TTTHH, TTHHT, THHTT, HHTTT, TTHTH, THTHT, HTHTT, THTTH, HTTHT, HTTTH	10
1 head, 4 tails	TTTTH, TTTHT, TTHTT, THTTT, HTTTT	5
0 heads, 5 tails	TTTTT	1
		Total: 32

Table 15.3 5-Coin Toss

The macrostate of three heads and two tails can be achieved in 10 ways and is thus 10 times more probable than the one having five heads. Not surprisingly, it is equally probable to have the reverse, two heads and three tails. Similarly, it is equally probable to get five tails as it is to get five heads. Note that all of these conclusions are based on the crucial assumption that each microstate is equally probable. With coin tosses, this requires that the coins not be asymmetric in a way that favors one side over the other, as with loaded dice. With any system, the assumption that all microstates are equally probable must be valid, or the analysis will be erroneous.

The two most orderly possibilities are five heads or five tails. (They are more structured than the others.) They are also the least likely, only two out of 32 possibilities. The most disorderly possibilities are three heads and two tails and its reverse. (They are the least structured.) The most disorderly possibilities are also the most likely, with 20 out of 32 possibilities for the three heads and two tails and its reverse. If we start with an orderly array like five heads and toss the coins, it is very likely that we will get a less orderly array as a result, since 30 out of the 32 possibilities are less orderly. So even if you start with an orderly state, there is a strong tendency to go from order to disorder, from low entropy to high entropy. The reverse can happen, but it is unlikely.


Macrostate		Number of microstates
Heads	Tails	(W)
100	0	1
99	1	$1.0 \times 10^{2}$
95	5	$7.5 \times 10^{7}$
90	10	$1.7 \times 10^{13}$
75	25	$2.4 \times 10^{23}$
60	40	$1.4 \times 10^{28}$
55	45	$6.1 \times 10^{28}$
51	49	$9.9 \times 10^{28}$
50	50	$1.0 \times 10^{29}$
49	51	$9.9 \times 10^{28}$
45	55	$6.1 \times 10^{28}$
40	60	$1.4 \times 10^{28}$
25	75	$2.4 \times 10^{23}$
10	90	$1.7 \times 10^{13}$
5	95	$7.5 \times 10^{7}$
1	99	$1.0 \times 10^{2}$
0	100	1

		Total: $1.27 \times 10^{30}$

Table 15.4 100-Coin Toss

This result becomes dramatic for larger systems. Consider what happens if you have 100 coins instead of just five. The most orderly arrangements (most structured) are 100 heads or 100 tails. The least orderly (least structured) is that of 50 heads and 50 tails. There is only one way (1 microstate) to get the most orderly arrangement of 100 heads. There are 100 ways (100 microstates) to get the next most orderly arrangement of 99 heads and one tail (also 100 to get its reverse). And there are $1.0 \times 10^{29}$ ways to get 50 heads and 50 tails, the least orderly arrangement. Table 15.4 is an abbreviated list of the various macrostates and the number of microstates for each macrostate. The total number of microstates—the total number of different ways 100 coins can be tossed—is an impressively large $1 . 27 \times 10^{30}$ . Now, if we start with an orderly macrostate like 100 heads and toss the coins, there is a virtual certainty that we will get a less orderly macrostate. If we keep tossing the coins, it is possible, but exceedingly unlikely, that we will ever get back to the most orderly macrostate. If you tossed the coins once each second, you could expect to get either 100 heads or 100 tails once in $2 \times 10^{22}$ years! This period is 1 trillion ( $10^{12}$ ) times longer than the age of the universe, and so the chances are essentially zero. In contrast, there is an 8 percent chance of getting 50 heads, a 73 percent chance of getting from 45 to 55 heads, and a 96 percent chance of getting from 40 to 60 heads. Disorder is highly likely.

Disorder in a Gas

The fantastic growth in the odds favoring disorder that we see in going from five to 100 coins continues as the number of entities in the system increases. Let us now imagine applying this approach to perhaps a small sample of gas. Because counting microstates and macrostates involves statistics, this is called statistical analysis. The macrostates of a gas correspond to its macroscopic properties, such as volume, temperature, and pressure; and its microstates correspond to the detailed description of the positions and velocities of its atoms. Even a small amount of gas has a huge number of atoms: $1.0 {cm}^{3}$ of an ideal gas at 1.0 atm and $0º C$ has $2 . 7 \times 10^{19}$ atoms. So each macrostate has an immense number of microstates. In plain language, this means that there are an immense number of ways in which the atoms in a gas can be arranged, while still having the same pressure, temperature, and so on.

The most likely conditions (or macrostates) for a gas are those we see all the time—a random distribution of atoms in space with a Maxwell-Boltzmann distribution of speeds in random directions, as predicted by kinetic theory. This is the most disorderly and least structured condition we can imagine. In contrast, one type of very orderly and structured macrostate has all of the atoms in one corner of a container with identical velocities. There are very few ways to accomplish this (very few microstates corresponding to it), and so it is exceedingly unlikely ever to occur. (See Figure 15.41(b)). Indeed, it is so unlikely that we have a law saying that it is impossible, which has never been observed to be violated—the second law of thermodynamics.

Two states of a container of gas are shown. In state a, the gas molecules, depicted as small green spheres, are randomly distributed in the container, with random velocities (an arrow is attached to each sphere, and the arrows vary in length and direction). This state is labeled likely. In state b, the molecules are clustered in the lower left-hand corner of the container and the arrows are much shorter. This state is labeled highly unlikely.

Figure 15.41 (a) The ordinary state of gas in a container is a disorderly, random distribution of atoms or molecules with a Maxwell-Boltzmann distribution of speeds. It is so unlikely that these atoms or molecules would ever end up in one corner of the container that it might as well be impossible. (b) With energy transfer, the gas can be forced into one corner and its entropy greatly reduced. But left alone, it will spontaneously increase its entropy and return to the normal conditions, because they are immensely more likely.

The disordered condition is one of high entropy, and the ordered one has low entropy. With a transfer of energy from another system, we could force all of the atoms into one corner and have a local decrease in entropy, but at the cost of an overall increase in entropy of the universe. If the atoms start out in one corner, they will quickly disperse and become uniformly distributed and will never return to the orderly original state (Figure 15.41(b)). Entropy will increase. With such a large sample of atoms, it is possible—but unimaginably unlikely—for entropy to decrease. Disorder is vastly more likely than order.

The arguments that disorder and high entropy are the most probable states are quite convincing. The great Austrian physicist Ludwig Boltzmann (1844–1906)—who, along with Maxwell, made so many contributions to kinetic theory—proved that the entropy of a system in a given state (a macrostate) can be written as

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S = k ln W,

where $k = 1 . 38 \times 10^{- 23} J/K$ is Boltzmann's constant, and $ln W$ is the natural logarithm of the number of microstates $W$ corresponding to the given macrostate. $W$ is proportional to the probability that the macrostate will occur. Thus entropy is directly related to the probability of a state—the more likely the state, the greater its entropy. Boltzmann proved that this expression for $S$ is equivalent to the definition $Δ S = Q / T$ , which we have used extensively.

Thus the second law of thermodynamics is explained on a very basic level: entropy either remains the same or increases in every process. This phenomenon is due to the extraordinarily small probability of a decrease, based on the extraordinarily larger number of microstates in systems with greater entropy. Entropy can decrease, but for any macroscopic system, this outcome is so unlikely that it will never be observed.

Example 15.9 Entropy Increases in a Coin Toss

Suppose you toss 100 coins starting with 60 heads and 40 tails, and you get the most likely result, 50 heads and 50 tails. What is the change in entropy?

Strategy

Noting that the number of microstates is labeled $W$ in Table 15.4 for the 100-coin toss, we can use $Δ S = S_{f} - S_{i} = k ln W_{f} - k ln W_{i}$ to calculate the change in entropy.

Solution

The change in entropy is

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Δ S = S_{f} - S_{i} = k ln W_{f} - k ln W_{i,}

where the subscript i stands for the initial 60 heads and 40 tails state, and the subscript f for the final 50 heads and 50 tails state. Substituting the values for $W$ from Table 15.4 gives

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\begin{array}{l} Δ S & = & (1.38 \times 10^{- 23} J/K) [ln (1.0 \times 10^{29}) - ln (1.4 \times 10^{28})] \\ = & 2.7 \times 10^{- 23} J/K \end{array}

Discussion

This increase in entropy means we have moved to a less orderly situation. It is not impossible for further tosses to produce the initial state of 60 heads and 40 tails, but it is less likely. There is about a 1 in 90 chance for that decrease in entropy ( $- 2 . 7 \times 10^{- 23} J/K$ ) to occur. If we calculate the decrease in entropy to move to the most orderly state, we get $Δ S = - 92 \times 10^{- 23} J/K$ . There is about a $1 in 10^{30}$ chance of this change occurring. So while very small decreases in entropy are unlikely, slightly greater decreases are impossibly unlikely. These probabilities imply, again, that for a macroscopic system, a decrease in entropy is impossible. For example, for heat transfer to occur spontaneously from 1.00 kg of $0º C$ ice to its $0º C$ environment, there would be a decrease in entropy of $1 . 22 \times 10^{3} J/K$ . Given that a $Δ S {of 10}^{- 21} J/K$ corresponds to about a $1 in 10^{30}$ chance, a decrease of this size ( $10^{3} J/K$ ) is an utter impossibility. Even for a milligram of melted ice to spontaneously refreeze is impossible.

Problem-Solving Strategies for Entropy

Examine the situation to determine if entropy is involved.
Identify the system of interest and draw a labeled diagram of the system showing energy flow.
Identify exactly what needs to be determined in the problem (identify the unknowns). A written list is useful.
Make a list of what is given or can be inferred from the problem as stated (identify the knowns). You must carefully identify the heat transfer, if any, and the temperature at which the process takes place. It is also important to identify the initial and final states.
Solve the appropriate equation for the quantity to be determined (the unknown). Note that the change in entropy can be determined between any states by calculating it for a reversible process.
Substitute the known value along with their units into the appropriate equation, and obtain numerical solutions complete with units.
To see if it is reasonable: Does it make sense? For example, total entropy should increase for any real process or be constant for a reversible process. Disordered states should be more probable and have greater entropy than ordered states.

15.7 Statistical Interpretation of Entropy and the Second Law of Thermodynamics: The Underlying Explanation

Learning Objectives