98 Heat Death
The Second Law of Thermodynamics Revisited
The introduced in the previous chapters states that thermal energy will always spontaneously transfer from higher temperature to lower temperature. In order to aid in our study of other thermodynamic processes, such as phase changes, a more general version of the Second Law can be stated in terms of energy concentration and dispersion: any must move an isolated system toward a state of more uniform dispersion of energy throughout the system. By we mean one for which energy does not leave or enter. For example, we know that higher means a greater average per molecule, so we can think of temperature as a measure of the of thermal energy in an object. If we consider a hot object in a cold room as our complete system, then the thermal energy in our system is not very well dispersed because it’s more concentrated in the hot object. The predicts that energy should move from the hot object to the cold environment to better disperse the energy, and that is what we observe. However, the heat transfer will only occur until the thermal energy is maximally dispersed, which corresponds to , and is indicated by the object and environment having the same temperature.
Everyday Examples: Sweating, Dew, and Rain
When we sweat to exhaust by we aren’t actively grabbing the hottest water molecules, pulling then away from their neighbors, and throwing them into the gas phase. The evaporation happens spontaneously because stored in water molecules that are stuck together is relatively concentrated compared to thermal energy stored in water molecules zipping around in the air and free to disperse. The transfer of thermal energy to sweat (by ), followed by evaporation is a because it increases the dispersion of energy throughout the system made up of you, the sweat, and the surrounding air. Therefore, evaporation of sweat is a .
When the reaches 100% then has maximally dispersed the available . Any additional evaporation would begin to over-concentrate energy in the air and decrease the overall level of energy dispersion. Therefore, we don’t see evaporation occurring once 100% humidity is reached. In fact if the humidity gets pushed above 100% (by a drop in air without a loss of water vapor) then energy is over-concentrated in the air and thus increasing dispersion of energy requires that water molecules come out of the vapor phase and occurs spontaneously. When the liquid condenses on surfaces we call it , when the liquid condenses on particles in the air and falls to the ground we call it rain.
(S) is a measure of energy within a system. An increase in the entropy corresponds to an increase in dispersion of energy. A decrease in entropy would correspond to energy being less dispersed, or increasing energy . Therefore the can also be stated as: a process will happen spontaneously if it increases the total entropy of an isolated system. The change in entropy for a constant-temperature process can be calculated from the heat transferred (Q) and the at which the transfer occurs (T) as:
Notice that we definitely need to use the absolute temperature scale when working with the change in equation, or else we might find ourselves attempting to divide by zero. Let’s apply this equation and the entropy version of the to the second part of the previous Reinforcement Exercise.
Everyday Example: Entropy Change of Melting
If you place ice in a warm room and leave it alone, it will melt. The ice would be a because it will happen all on it’s own, so we should find that melting increases the total entropy (ΔS > 0). Let’s check that out. We’ll keep it simple and calculate change in entropy of one kilogram of ice, which melts at 0 °C, or 273 K.
Next we calculate the change in for the room. The same that went into melting the ice came out of the room, so the Q for the room is the same as for the ice, only negative. Let’s pick a typical room temperature of 20 °C for our example, which is 293 K:
Now we just add up the two changes to get the total:
Our entropy change is greater than zero, so the states that ice melting in warm room is a , which we observe it to be.
are inherently . For example, we could not reverse the spontaneous process of transfer from your body to sweat and then to the environment by . Imagine trying to run around and grab all the water vapor molecules and shove them back into the liquid on our skin and then make those water molecules collide with skin molecules in just the right way to conduct thermal energy back into your body! Good luck. If the process could be reversed, the net change would be zero, but that is not a real possibility. Any real process increases the entropy because irreversible at some level, meaning energy is further dispersed throughout the system without a realistic opportunity to put it back where it was. We have arrived at yet another version of the : any real process increases the total entropy of the universe. For example, even if you could reverse the process we described above, the you released during that running around would decrease the of energy in your body and disperse it throughout the room.The system, which includes you, would not cause have returned to the original conditions at all. In fact, the total entropy would have increased by even more than before you tried to reverse the process. For example, as you ran around, more sweat would have evaporated and you would have to chase those molecules down as well, and so on–you could never win! We can’t keep the of the universe from increasing.
Everyday Examples: Human Mechanical Efficiency
Muscle contraction relies on the release of stored in ATP molecules. Before contraction, that energy is concentrated into certain molecules in certain areas of a muscle cell. When that energy is released, the of the molecules decreases, so the entropy of their environment must increase by more, and this is achieved because most of the energy released from the ATP molecules is degraded to and distributed to the environment. After contraction, a muscle cell must be reorganized, which decreases , but we know overall entropy must increase for any real process, so some additional must be to the environment during reorganization in order to provide the necessary entropy increase. All of this thermal energy is “wasted” because it is came from stored , but is not available for use by the body to do . Therefore, and the limit the of the human body.
Everyday Example: Geothermal Heat Engine
Let’s imagine molten rock from the Earth’s pushes partway through the Earth’s , and keeps a region of at a constant of 300 °C . If the rock was not too deep, we could install pipes in the rock, and then boil water by running it through the pipes. We would basically have a giant pressure cooker! Rather than cook food, we could release the pressurized steam to push on a piston or spin a turbine. After releasing the pressure and getting some work out, we would be left with lower pressure steam. We could condense the steam back to water by running it through pipes exposed to the 20 °C air above ground. would transfer from the steam to the air as , the steam would condense into liquid water, and we could start again.
Machines like the one described that convert into are called a . Your car is powered by an internal combustion heat engine. Let’s see how and the determine the of our geothermal heat engine.
First we calculate the entropy change when 1000 J of thermal energy transfers out of the rock to the water to run the engine, remembering to convert the 300 °C rock temperature to by adding 273 K:
If our engine is real, then so are its processes, which means that running the engine must increase the total of the universe, according to the . We need to find out how much must be transferred from the low pressure steam into the air at 30 °C (293 K) in order for the entropy of the air to increase by at least as much as the rock entropy decreased (1.75 J/K). We can find this by rearranging the change in entropy equation and inserting a positive entropy change that is equal in size to the the negative change experienced by the hot rock:
Transferring the 511 J of into the air leaves only 489 J of the original 1000 J input energy available for doing . Therefore the maximum possible of our engine is limited, no matter how well designed, even if all mechanical inefficiencies like could some how be eliminated. The maximum theoretical is:
Multiplying by 100 % would give us the efficiency as a percentage: 49 %. This is a maximum possible efficiency. Any engine we actually built would be less efficient.
The told us that you cannot build an engine that is more than 100 % efficient because energy cannot be created. Even worse, the tells us that even if we managed to eliminate all mechanical inefficiencies, such as , we still can’t get up to 100 % because all engines must exhaust some energy in order to increase entropy overall. The theoretical maximum efficiency, which is always less than 100 %, is known as the (ec) and depends only on the high and low operating temperatures (TH and TL), as we saw in the previous example. Most of the work we did in the previous example can be short-cut by the equation for Carnot Efficiency (ec):
The theoretical engine which could actually produce that theoretically maximum efficiency is known as the Carnot Engine. The operating principles of the Carnot Engine are well known, having been developed by Nicolas Léonard Sadi Carnot in 1824, but the engine cannot be realistically designed or built.
Reinforcement Exercise: Carnot Efficiency
Check that the previous short-cut equation gives the correct maximum for our geothermal .
What is the of our geothermal heat engine if the hot rock was actually at 550 C° instead of 300 C° ?
You will find that this engine is more just because the hot operating temperature higher, even though it still works in the same way and nothing else has changed. The efficiency increased because the input energy started out more concentrated and less dispersed (indicated by higher temperature), so less of that energy had to become dispersed in the environment, or wasted, in order to ensure that entropy increased by a sufficient amount to satisfy the . Thermal energy that starts out concentrated (at high temperature) is known as high quality energy.
In addition to limiting our in doing mechanical work, the drives our bodies toward higher , which means with the environment. Unless the environmental temperature happens to be near body temperature, reaching thermal equilibrium means death. Life also requires of chemical potential energy, but due to the the Second Law we tend toward chemical equilibrium, which is not survivable. Concentrations of electrical energy drive your nervous system, but due to the Second Law we are constantly at risk of reaching an internal electrical equilibrium with no electrical activity. Life is a constant battle against various types of equilibrium that would correspond to maximum , but also to death. The necessary to fight off our own entropy increase is what we consider basic metabolism. Doing that work, and even taking in the energy required to do that work, involves real processes that provide even more opportunity for entropy increases in a seemingly viscous cycle. You can’t beat the! Even as we manage to prevent our own entropy increase we cause the entropy of the environment to increase by a greater amount than what we prevented in ourselves. In fact, a complete dispersion of energy, so that all matter is at equilibrium, and no processes remain which would increase the entropy, and nothing really happens all, is one possible fate of the universe which has been dubbed heat death. At least we don’t expect heat death of the universe to occur for at least 10100 years. 
- "Thermodynamics of Skeletal Muscle Fiber: Do We Need to Redefine "Active" and "Resting" States?" by I. Y. Cristlieb and E. Cesarman, Cadiovascular and Pulmonary Research Center, The Medical College of Pennsylvania/Hahnemann University ↵
- "Carnot heat engine" by Wikipedia ↵
- OpenStax, College Physics. OpenStax CNX. Mar 6, 2019 http://firstname.lastname@example.org ↵
the total entropy of an isolated system can never decrease over time, meaning objects left to themselves will always trend toward thermal equilibrium, meaning that thermal energy will always spontaneously transfer from hot system to cold system
a process which occurs naturally on its own, without the need for work to be done in forcing it to happen.
a system for which neither thermal energy or particles are allowed to leave or enter.
a measure of the average kinetic energy of the particles (e.g., atoms and molecules) in an object, which determines how relatively hot or cold an object feels
energy stored in the microscopic motion of atoms and molecules (microscopic kinetic energy)
relative amount of one substance or quantity contained or stored within another substance or quantity, such as thermal energy per molecule
a two systems are in thermal equilibrium when they do not exchange heat, which means they must be at the same temperature
vaporization that occurs on the surface of a liquid as it changes into the gas phase
the process by which heat or directly transmitted through a substance when there is a difference of temperature between adjoining regions, without movement of the material
a measure of how many water molecules are in the vapor phase relative to the maximum number that could possibly be in the vapor phase at at a given temperature. A relative humidity of 100% means that no more water molecules can be added to the vapor phase.
Process of vapor changing phase into a liquid.
water that condenses on cool surfaces at night, when decreasing temperature forces humidity to 100% or higher
A measure of energy dispersion in a system.
the action or process of distributing a quantity over a wide space
SI unit of temperature
changing phase from solid to liquid.
An amount of thermal energy transferred due to a difference in temperature.
a process that is not a reversible process in which the system and environment can be restored to exactly the same initial states that they were in before the process
heat transferred to the environment rather than being used to do useful work
energy stored in the chemical bonds of a substance
A quantity representing the effect of applying a force to an object or system while it moves some distance.
ratio of useful work performed to total energy expended
the mantle is the mostly-solid bulk of Earth's interior. The mantle lies between Earth's dense, super-heated core and its thin outer layer, the crust.
the relatively thin layer of rock that makes up the outermost solid shell of our planet
hard rock exposed or buried at the earth's surface
the sum of potential and kinetic energy
devices for converting thermal energy to useful work and exhaust heat
a force that acts on surfaces in opposition to sliding motion between the surfaces
the change in internal energy of a system is equal to the heat added to the system minus the work done by the system
the maximum theoretical efficiency that a heat engine could achieve when operating between two set temperatures, as permitted by the Second Law of Thermodynamics