Entropy is defined as the quantitative measure of disorder or randomness in a system. The concept comes out of thermodynamics, which deals with the transfer of heat energy within a system. Instead of talking about some form of "absolute entropy," physicists generally discuss the change in entropy that takes place in a specific thermodynamic process. Key Takeaways: Calculating Entropy
Entropy is a measure of probability and the molecular disorder of a macroscopic system.
If each configuration is equally probable, then the entropy is the natural logarithm of the number of configurations, multiplied by Boltzmann's constant: S = kB ln W
For entropy to decrease, you must transfer energy from somewhere outside the system.
How to Calculate Entropy In an isothermal process, the change in entropy (delta-S) is the change in heat (Q) divided by the absolute temperature (T): delta-S = Q/T In any reversible thermodynamic process, it can be represented in calculus as the integral from a process's initial state to its final state of dQ/T. In a more general sense, entropy is a measure of probability and the molecular disorder of a macroscopic system. In a system that can be described by variables, those variables may assume a certain number of configurations. If each configuration is equally probable, then the entropy is the natural logarithm of the number of configurations, multiplied by Boltzmann's constant: S = kB ln W where S is entropy, kB is Boltzmann's constant, ln is the natural logarithm, and W represents the number of possible states. Boltzmann's constant is equal to 1.38065 × 10−23 J/K. Units of Entropy Entropy is considered to be an extensive property of matter that is expressed in terms of energy divided by temperature. The SI units of entropy are J/K (joules/degrees Kelvin). Entropy and the Second Law of Thermodynamics One way of stating the second law of thermodynamics is as follows: in any closed system, the entropy of the system will either remain constant or increase. You can view this as follows: adding heat to a system causes the molecules and atoms to speed up. It may be possible (though tricky) to reverse the process in a closed system without drawing any energy from or releasing energy somewhere else to reach the initial state. You can never get the entire system "less energetic" than when it started. The energy doesn't have any place to go. For irreversible processes, the combined entropy of the system and its environment always increases. Misconceptions About Entropy This view of the second law of thermodynamics is very popular, and it has been misused. Some argue that the second law of thermodynamics means that a system can never become more orderly. This is untrue. It just means that to become more orderly (for entropy to decrease), you must transfer energy from somewhere outside the system, such as when a pregnant woman draws energy from food to cause the fertilized egg to form into a baby. This is completely in line with the second law's provisions. Entropy is also known as disorder, chaos, and randomness, though all three synonyms are imprecise. Absolute Entropy A related term is "absolute entropy," which is denoted by S rather than ΔS. Absolute entropy is defined according to the third law of thermodynamics. Here a constant is applied that makes it so that the entropy at absolute zero is defined to be zero. Entropy and Heat Death of the Universe
Some scientists predict the entropy of the universe will increase to the point where the randomness creates a system incapable of useful work. When only thermal energy remains, the universe would be said to have died of heat death.
However, other scientists dispute the theory of heat death. Some say the universe as a system moves further away from entropy even as areas within it increase in entropy. Others consider the universe as part of a larger system. Still others say the possible states do not have equal likelihood, so ordinary equations to calculate entropy do not hold valid.
Example of Entropy A block of ice will increase in entropy as it melts. It's easy to visualize the increase in the disorder of the system. Ice consists of water molecules bonded to each other in a crystal lattice. As ice melts, molecules gain more energy, spread further apart, and lose structure to form a liquid. Similarly, the phase change from a liquid to a gas, as from water to steam, increases the energy of the system.
On the flip side, energy can decrease. This occurs as steam changes phase into water or as water changes to ice. The second law of thermodynamics is not violated because the matter is not in a closed system. While the entropy of the system being studied may decrease, that of the environment increases. Entropy and Time Entropy is often called the arrow of time in this universe because matter in isolated systems tends to move from order to disorder, and I have written a theory on this, "Algebraic Formulation Of Time" If you're very much enthusiastic to read my theory you can contact me or comment below, and i will provide you the pdf of it.
Sources: Clausius, Rudolf (1850). On the Motive Power of Heat, and on the Laws which can be deduced from it for the Theory of Heat. Poggendorff's Annalen der Physick, LXXIX (Dover Reprint). ISBN 978-0-486-59065-3. Landsberg, P.T. (1984). "Can Entropy and "Order" Increase Together?". Physics Letters. 102A (4): 171–173. doi:10.1016/0375-9601(84)90934-4
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