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entropies

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Definitions of entropies in various dictionaries:

noun - (communication theory) a numerical measure of the uncertainty of an outcome

noun - (thermodynamics) a thermodynamic quantity representing the amount of energy in a system that is no longer available for doing mechanical work

adj - a thermodynamic measure of disorder [n -PIES] : ENTROPIC

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Possible Dictionary Clues
Plural form of entropy.
A thermodynamic quantity representing the unavailability of a system's thermal energy for conversion into mechanical work, often interpreted as the degree of disorder or randomness in the system.
Lack of order or predictability gradual decline into disorder.
(in information theory) a logarithmic measure of the rate of transfer of information in a particular message or language.

Entropies might refer to
In statistical mechanics, Entropy is an extensive property of a thermodynamic system. It is closely related to the number Ω of microscopic configurations (known as microstates) that are consistent with the macroscopic quantities that characterize the system (such as its volume, pressure and temperature). Under the assumption that each microstate is equally probable, the entropy * * * * S * * * {\displaystyle S} * is the natural logarithm of the number of microstates, multiplied by the Boltzmann constant kB. Formally,* * * * S * = * * k * * * B * * * * ln * ⁡ * Ω * * (assuming equiprobable microstates) * * . * * * {\displaystyle S=k_{\mathrm {B} }\ln \Omega {\text{ (assuming equiprobable microstates)}}.} * Macroscopic systems typically have a very large number Ω of possible microscopic configurations. For example, the entropy of an ideal gas is proportional to the number of gas molecules N. Roughly twenty liters of gas at room temperature and atmospheric pressure has N ≈ 6×1023 (Avogadro's number). At equilibrium, each of the Ω ≈ eN configurations can be regarded as random and equally likely. * The second law of thermodynamics states that the entropy of an isolated system never decreases. Such systems spontaneously evolve towards thermodynamic equilibrium, the state with maximum entropy. Non-isolated systems may lose entropy, provided their environment's entropy increases by at least that amount so that the total entropy increases. Entropy is a function of the state of the system, so the change in entropy of a system is determined by its initial and final states. In the idealization that a process is reversible, the entropy does not change, while irreversible processes always increase the total entropy. * Because it is determined by the number of random microstates, entropy is related to the amount of additional information needed to specify the exact physical state of a system, given its macroscopic specification. For this reason, it is often said that entropy is an expression of the disorder, or randomness of a system, or of the lack of information about it. The concept of entropy plays a central role in information theory. * Boltzmann's constant, and therefore entropy, have dimensions of energy divided by temperature, which has a unit of joules per kelvin (J K−1) in the International System of Units (or kg m2 s−2 K−1 in terms of base units). The entropy of a substance is usually given as an intensive property—either entropy per unit mass (SI unit: J K−1 kg−1) or entropy per unit amount of substance (SI unit: J K−1 mol−1).

Entropies might refer to

In statistical mechanics, Entropy is an extensive property of a thermodynamic system. It is closely related to the number Ω of microscopic configurations (known as microstates) that are consistent with the macroscopic quantities that characterize the system (such as its volume, pressure and temperature). Under the assumption that each microstate is equally probable, the entropy
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* {\displaystyle S=k_{\mathrm {B} }\ln \Omega {\text{ (assuming equiprobable microstates)}}.}
* Macroscopic systems typically have a very large number Ω of possible microscopic configurations. For example, the entropy of an ideal gas is proportional to the number of gas molecules N. Roughly twenty liters of gas at room temperature and atmospheric pressure has N ≈ 6×1023 (Avogadro's number). At equilibrium, each of the Ω ≈ eN configurations can be regarded as random and equally likely.
* The second law of thermodynamics states that the entropy of an isolated system never decreases. Such systems spontaneously evolve towards thermodynamic equilibrium, the state with maximum entropy. Non-isolated systems may lose entropy, provided their environment's entropy increases by at least that amount so that the total entropy increases. Entropy is a function of the state of the system, so the change in entropy of a system is determined by its initial and final states. In the idealization that a process is reversible, the entropy does not change, while irreversible processes always increase the total entropy.
* Because it is determined by the number of random microstates, entropy is related to the amount of additional information needed to specify the exact physical state of a system, given its macroscopic specification. For this reason, it is often said that entropy is an expression of the disorder, or randomness of a system, or of the lack of information about it. The concept of entropy plays a central role in information theory.
* Boltzmann's constant, and therefore entropy, have dimensions of energy divided by temperature, which has a unit of joules per kelvin (J K−1) in the International System of Units (or kg m2 s−2 K−1 in terms of base units). The entropy of a substance is usually given as an intensive property—either entropy per unit mass (SI unit: J K−1 kg−1) or entropy per unit amount of substance (SI unit: J K−1 mol−1).

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