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The 2nd law of thermodynamics, a physical law that tells us that entropy always increases, is always true strictly because the tendency of masses of molecules to assemble themselves from states of low probability to states of ever increasing probability. Every system that is left to itself (i.e. not imposed upon by an intelligent being or beings) will eventually change toward a condition of maximum probability (sometimes paraphrased as; if you think things are mixed up now, just wait). This principle applies equally to information content of any system. This fact has great implications on the materialistic theory of evolution (i.e. common ancestry): nearly all states (e.g. arrangements) in which molecules can naturally self organize themselves into are meaningless and useless to the formation of the necessary structures required by all types of lifes organisms to have come into existence. Those states (e.g. arrangements) of molecules that are meaningful to (e.g. provide a necessary function for the existence of -) the diverse types of organism found on this planet are, by comparison, almost infinitely small. The logical conclusion is that the 2nd law demands that molecules will naturally arrange themselves into patterns that are unsuitable for life and for broad range evolution to occur. Therefore, scientifically speaking, the broad range concept of evolution, sometimes called macro-evolution or the General Theory of Evolution, that all organism extinct and extant share a common ancestor, is in violation of the 2nd Law and is thereby scientifically falsified. In academia very few will use the word falsified as Evolution has become an untouchable Icon, the golden calf of the materialistic worldview.
The following are quotations from scientists who understand the 2nd law as derivative of the law of increasing probability, and with full application to open systems as well as isolated. Physicist Harold F Blum, Perspectives in Evolution, American Scientist, vol. 43 (October 1955), pp 595‑610. pp. 595-6
A major consequence of the second law of thermodynamics is that all real processes go toward a condition of greater probability. The probability function generally used in thermodynamics is entropy . Thus orderliness is associated with low entropy; randomness with high entropy . The second law of thermodynamics says that left to itself any isolated system will go toward greater entropy, which also means toward greater randomness and greater likelihood.
Sommerfeld, Arnold, Thermodynamics and Statistical Mechanics, Lectures on Theoretical Physics, vol. V (New York: Academic Press, 1956), p. 155. (eq 10)
[where = entropy generated locally, s = entropy flux, e = mass density, = time rate of entropy change.]
Equation (10) together with the inequality  = can be regarded as the differential formulation of the Second Law of Thermodynamics. The statement in integral form, namely that the entropy in an isolated system cannot decrease, can be replaced by its corollary in differential form which asserts that the quantity of entropy generated locally cannot be negative irrespective of whether the system is isolated or not, and irrespective of whether the process under consideration is irreversible or not.
Ross, John, 2nd Law of Thermodynamics, Letter-to-the-Editor, Chemical and Engineering News, vol. 58 (July 7, 1980), p. 40. Ross was at Harvard University. p. 40
there are no known violations of the second law of thermodynamics. Ordinarily the second law is stated for isolated systems, but the second law applies equally well to open systems .
There is somehow associated with the field of far-from-equilibrium phenomena the notion that the second law of thermodynamics fails for such systems. It is important to make sure that this error does not perpetuate itself.
Physicist Richard P. Feynman is consistent with Blums statement, explains entropy as the flow from order to disorder, from states of lower probability to states of higher probability.
He gives the example of filming two gases, a gas of white particles and a gas of black particles, in a container separated by a boundary. He calls this state highly ordered as all the black particles in the container are all on one side and all the white particles are on the other side. When the boundary is removed, the particles will mix together, order decreases and disorder increases. This is considered an irreversible process. But Feynman has an objection, if you play the film backwards, the particles separate and all the white particles go to one side of the container and the black particles go to the other side of the container, and not only that, but careful observation shows that no physical laws are broken, all the particles are moving at just the right speed and are forming just the right collisions at just the right angle for this to happen. Thus the process is reversible and, Feynman adds, so is all the fundamental laws of physics. So what is it that makes the natural mixing of the two gases irreversible? Feynman's answer is `probability'. The number of states (particle distribution) of disorder far outnumbers the number of states of order, so much so that it becomes unrealistic to expect reversibility. The gases are moving from states of very low probability to states of much higher probability, moving from order to disorder.
The following are quotations from scientists who understand the 2nd law as derivative of the law of increasing probability, and with full application to open systems as well as isolated. Physicist Harold F Blum, Perspectives in Evolution, American Scientist, vol. 43 (October 1955), pp 595‑610. pp. 595-6
A major consequence of the second law of thermodynamics is that all real processes go toward a condition of greater probability. The probability function generally used in thermodynamics is entropy . Thus orderliness is associated with low entropy; randomness with high entropy . The second law of thermodynamics says that left to itself any isolated system will go toward greater entropy, which also means toward greater randomness and greater likelihood.
Sommerfeld, Arnold, Thermodynamics and Statistical Mechanics, Lectures on Theoretical Physics, vol. V (New York: Academic Press, 1956), p. 155. (eq 10)
[where = entropy generated locally, s = entropy flux, e = mass density, = time rate of entropy change.]
Equation (10) together with the inequality  = can be regarded as the differential formulation of the Second Law of Thermodynamics. The statement in integral form, namely that the entropy in an isolated system cannot decrease, can be replaced by its corollary in differential form which asserts that the quantity of entropy generated locally cannot be negative irrespective of whether the system is isolated or not, and irrespective of whether the process under consideration is irreversible or not.
Ross, John, 2nd Law of Thermodynamics, Letter-to-the-Editor, Chemical and Engineering News, vol. 58 (July 7, 1980), p. 40. Ross was at Harvard University. p. 40
there are no known violations of the second law of thermodynamics. Ordinarily the second law is stated for isolated systems, but the second law applies equally well to open systems .
There is somehow associated with the field of far-from-equilibrium phenomena the notion that the second law of thermodynamics fails for such systems. It is important to make sure that this error does not perpetuate itself.
Physicist Richard P. Feynman is consistent with Blums statement, explains entropy as the flow from order to disorder, from states of lower probability to states of higher probability.
He gives the example of filming two gases, a gas of white particles and a gas of black particles, in a container separated by a boundary. He calls this state highly ordered as all the black particles in the container are all on one side and all the white particles are on the other side. When the boundary is removed, the particles will mix together, order decreases and disorder increases. This is considered an irreversible process. But Feynman has an objection, if you play the film backwards, the particles separate and all the white particles go to one side of the container and the black particles go to the other side of the container, and not only that, but careful observation shows that no physical laws are broken, all the particles are moving at just the right speed and are forming just the right collisions at just the right angle for this to happen. Thus the process is reversible and, Feynman adds, so is all the fundamental laws of physics. So what is it that makes the natural mixing of the two gases irreversible? Feynman's answer is `probability'. The number of states (particle distribution) of disorder far outnumbers the number of states of order, so much so that it becomes unrealistic to expect reversibility. The gases are moving from states of very low probability to states of much higher probability, moving from order to disorder.