“Does Entropy contradict Evolution?” [1] . Creationists point out a serious contradiction or paradox about Entropy. Whereas the world and the Universe should work to chaos according to the second law of Thermodynamics with Entropy, since the Bing Bang and the primordial soap, stars, planets, life, more organized worlds have appeared and not a more chaotic world. For scientist, this paradox would only be apparent, because the Chaos would be created “elsewhere”. For Creationist, if there is a contradiction between the two assessments, that means that one is false, and it would be the Evolution one. Here, the purpose is not to debate or to argue about Evolution vs. Creationism. But our purpose will be to recognize this paradox, and between the two assessments, if one is false, it would be the Entropy function.

Let us remind ourselves where Entropy function (noted S) comes from and its role in thermodynamic efficiency and in the increase of disorder.

Sadi Carnot found the engine efficiency of a thermal motor depends only of its temperatures: the higher the difference of temperatures is, the higher the efficiency is.For a thermodynamic cycle, the efficiency η is defined by

Like water falling from top to bottom to turn the wheel of a mill, Sadi Carnot compared in 1824 the temperature to an invisible fluid dropping from hot to cold which would turn thermodynamic engines [2] . But for his part Joule demonstrated that Heat is not a fluid, and can be proceed from the Work.

Later Rudolf Clausius created in 1854 the Entropy function, which name means “content transformative” and sounds like “Energy”. Because it is not easy to define the entropy itself, difference of entropy () of a system is defined as:

where T is the absolute temperature of the system, and the incremental reversible transfer of heat into that system. Using the equivalence of Heat and Work, efficiency can be written:

And thanks to this Entropy function, it can be demonstrated that the engine efficiency will be limited by the temperature of the sources:

where is the temperature of the hot source, and the temperature of the cold source. is called the Carnot efficiency.

In 1877, Boltzmann linked the Entropy function to the probability of the number of specific ways in which a system may be arranged, especially with irreversible movements of particles.

At the beginning of the 20^thcentury, Bergson stated that the entire Universe is changing over time, in a constant direction. And since then, the Entropy function is linked to the Chaos.

An easy way would be to disconnect the Entropy function from the Chaos, but even keeping the original concept of Claudius with reversible transfer, it remains another paradox.

Entropy variation is defined by reversible transfer of heat, as seen in Equation (2):

cf Equation (2)

But what does a “reversible” transfer of heat mean? It would mean that heat could go from one side to another, back and forth indefinitely without any change in the environment!… In a way, a perpetual transfer! Let us remember that the reversible transfer of heat was imagined when heat was still considered as a fluid. In fact the heat goes from the hot source to the cold source, and so “any real transformation is irreversible in fact” [3] . Because variation of entropy is defined by reversible heat, that means that demonstrations using entropy are based on impossible transfers!

Let us now try to demonstrate thermodynamic properties without using this Entropy function, qualified by Bergson [4] as the most “metaphysical” of the physical laws.

“Internal” energy is not named as such to distinguish it from an external energy, but from the kinetic energy of the system and from the potential energy of the system. From a microscopic point of view, it is the sum of the kinetic energies of the atoms, and it is called U. From a microscopic point of view, it is difficult to define it and in practice, internal energy cannot be measured. It is always surprising to base a theory on a concept we cannot measure!

If internal energy cannot be measured, its main property is easy to define and to measure: the variation of internal energy is the sum of the work and the heat exchanged with the outside.

It is called the first law of Thermodynamics

Traditionally, the infinitesimal work exchanged by the system with the outside is calculated thanks to the formula

with the volume variation and the external pressure.

It is surprising that the work received or supplied by the “internal” system is due to the “external” pressure only. A work refers to a volume variation, a movement. According to the mechanical principle of inertia, a movement is due to a force. A force cannot exist if the internal pressure is equal to the external pressure. In fact, a force depends of the “difference” of pressure between the inside and the outside. Let us clarify

・ is the work supplied (<0) or received (>0) by the outside, the Universe

・ is the work supplied (<0) or received (>0) by the inside, the system

・ the variation of volume of the outside, the Universe

・ the variation of volume of the inside, the system

When the volume of the inside system increases (respectively decreases), the volume of the outside decreases (respectively increases):

Taking an axis positive from Left to Right, general expression of the transferred work is:

which means, if the system is on the Left side, and the outside on the right side (see Figure 1):

Due to Equation (9), we can check that

Note: when we get the same pressure inside and outside, we get equilibrium, there is no movement and so no work:

The energy radiated by a body in vacuum is proportional to its temperature according to Stéphan-Boltz- mann law [5] [6] :

with the constant, T the temperature and A the area of the body.

What is true for a single body should be true for several bodies. Let us have an adiabatic (without loss of heat) enclosure with two bodies inside (see Figure 2).

First one will emit (so it will have a negative value) the energy

and this emitted energy will be received (so it will have a positive value) by the second body. The second body will emit the energy

and this emitted energy will be received by the first body. When we do the balance, the energy emitted and received by each body is

for the first body

and for the second body

We can check at the equilibrium where the temperatures are equal that each body emits and receives the same amount of energy, thus the balance for each body is nil:

Note: mathematically, the difference of temperature is equal to

So the energy emitted and received by a body can also be written as

where is the outside temperature (of the source), is the inside temperature (of the system) and s is a factor depending on the temperature:

Why should we use this group? Because at the usual temperature, for example at 10˚C and 30˚C, the mathematical difference of s with the average temperature (20˚C) will be about 0.1%, which is insignificant:

and

And with regards to the difference with the entropy, s is only a calculation, it is not a state “function”.

To conclude, we do not need to use the Entropy function to explain that Heat goes from hot to cold. It can be explained by a hot body emitting more heat than a cold body, and so the difference of heat looks like a heat transfer from the hot body to the cold body.

To simplify the reading (and the writing), when it is possible or easier we will use:

・ Small letters for the internal system.

・ Capital letters for the external Universe, or sources.

・ is the energy emitted and received from the cold inside system.

・ is the energy emitted and received from the cold outside source.

Another application (from Equations (10) and (11).

・ is the work received or supplied by the internal system (small letters).

・ is the work received or supplied by the external Universe (Capital letters).

Let us now demonstrate the first “isentropic” law without using the entropy function.

Traditionally the Laplace law is demonstrated by using the two equations hereafter

and

cf. Equation (6)

Then, it is done the hypothesis of a reversible way (let us remember that a reversible way does not exist) in order to write the equality:

which is clearly excessive, because when the internal pressure and the external pressure are equal, there is no movement!

We will use the perfect gas formula and definitions hereafter:

With previous equations, it is traditionally demonstrated that

According to the first law of thermodynamic, with the new expression defined earlier:

cf Equation (5)

which can also be written as:

In the case of an adiabatic transformation (and so irreversible), there is no heat exchange:

and using Equations (10) and (26):

Dividing by the temperature:

Using Equation (7) on the variation of internal and external volume

And using Equation (26) of perfect gas, for internal gas and for external gas

For the outside Universe, it is considered as infinite,

So

And so

Then

Integrating it:

Then using Equation (31) on the property of :

Which is equivalent, using Equation (26) of perfect gas

It is nothing else than the Laplace law:

The difference with the classical demonstration is that it has not been confused and. Only the adiabatic property (and not the “reversible” property) was used. That means Laplace law has been demonstrated without using neither the Entropy function nor the Entropy property.

Traditionally to demonstrate the Carnot efficiency, the in-equation hereafter is used, which links the sources temperatures to the exchanged energies:

where (>0) is the energy received from the HOT source and (<0) the energy supplied to the COLD source. This equation comes from the Entropy function.

The trouble is it is forgotten that when two bodies (the system and the source) are at the same temperature, there is no exchange of heat (see Figure 3):

Starting again from the definition of the cycle efficiency with Equation (1) and (3),

the Carnot efficiency is mathematically undefined!

Let us check now the situation without using the Entropy function or its property.

Sadi Carnot considered the temperature as a fluid: the higher the temperature difference is, the more efficient it is (as for mill, the higher the water level difference is, the more efficient it is). He did not used the entropy function (which was invented by Rudolf Clausius).

Here, we still have the same conclusion―the higher the temperature difference is, the more efficient it is― but for other reasons:

・ Because they are isenthalpic (without heat exchange), the work received on BC is equal to the work delivered in DA: balance is nil.

・ Because they are quite isotherm, the heat received in CD is transformed into work, and the work received in AB is transformed into “heat” to the cold source. But in the cycle, the heat received is proportional to the temperature of the hot source (cf Equation (81)), and the heat delivered is proportional to the cold one. So the system receives more heat than it delivers, and so the balance is delivered in work. See Figure 6.