# Clausius theorem

Clausius theorem Thermodynamics The classical Carnot heat engine show Branches show Laws show Systems show System properties show Material properties show Equations show Potentials show HistoryCulture show Scientists show Other Category vte The Clausius theorem (1855) states that for a thermodynamic system (z.B. heat engine or heat pump) exchanging heat with external reservoirs and undergoing a thermodynamic cycle, {displaystyle oint {frac {delta Q}{T_{Text{surr}}}}leq 0,} wo {displaystyle delta Q} is the infinitesimal amount of heat absorbed by the system from the reservoir and {Anzeigestil T_{Text{surr}}} is the temperature of the external reservoir (surroundings) at a particular instant in time. The closed integral is carried out along a thermodynamic process path from the initial/final state to the same initial/final state. In principle, the closed integral can start and end at an arbitrary point along the path.

If there are multiple reservoirs with different temperatures {Anzeigestil links(T_{1},T_{2},Punkte ,T_{n}Rechts)} , then Clausius inequality reads: {displaystyle oint left({frac {delta Q_{1}}{T_{1}}}+{frac {delta Q_{2}}{T_{2}}}+cdots +{frac {delta Q_{n}}{T_{n}}}Rechts)leq 0.} In the special case of a reversible process, the equality holds.[1] The reversible case is used to introduce the state function known as entropy. This is because in a cyclic process the variation of a state function is zero. Mit anderen Worten, the Clausius statement states that it is impossible to construct a device whose sole effect is the transfer of heat from a cool reservoir to a hot reservoir.[2] Äquivalent, heat spontaneously flows from a hot body to a cooler one, not the other way around.[3] The generalized "inequality of Clausius"[4] {displaystyle dS_{Text{sys}}geq {frac {delta Q}{T_{Text{surr}}}}} for an infinitesimal change in entropy S applies not only to cyclic processes, but to any process that occurs in a closed system.

Inhalt 1 Geschichte 2 Nachweisen 3 Siehe auch 4 Verweise 5 Weiterlesen 6 External links History The Clausius theorem is a mathematical explanation of the second law of thermodynamics. It was developed by Rudolf Clausius who intended to explain the relationship between the heat flow in a system and the entropy of the system and its surroundings. Clausius developed this in his efforts to explain entropy and define it quantitatively. In more direct terms, the theorem gives us a way to determine if a cyclical process is reversible or irreversible. The Clausius theorem provides a quantitative formula for understanding the second law.

Clausius was one of the first to work on the idea of entropy and is even responsible for giving it that name. What is now known as the Clausius theorem was first published in 1862 in Clausius' sixth memoir, "On the Application of the Theorem of the Equivalence of Transformations to Interior Work". Clausius sought to show a proportional relationship between entropy and the energy flow by heating (δQ) into a system. In a system, this heat energy can be transformed into work, and work can be transformed into heat through a cyclical process. Clausius writes that "The algebraic sum of all the transformations occurring in a cyclical process can only be less than zero, oder, as an extreme case, equal to nothing." Mit anderen Worten, the equation {displaystyle oint {frac {delta Q}{T}}=0} with Q being energy flow into the system due to heating and T being absolute temperature of the body when that energy is absorbed, is found to be true for any process that is cyclical and reversible. Clausius then took this a step further and determined that the following relation must be found true for any cyclical process that is possible, reversible or not. This relation is the "Clausius inequality".

{displaystyle oint {frac {delta Q}{T_{Text{surr}}}}leq 0} Now that this is known, there must be a relation developed between the Clausius inequality and entropy. The amount of entropy S added to the system during the cycle is defined as {displaystyle Delta S{=}oint {frac {delta Q}{T}}} It has been determined, as stated in the second law of thermodynamics, that the entropy is a state function: It depends only upon the state that the system is in, and not what path the system took to get there. This is in contrast to the amount of energy added as heat ( Q) and as work ( W), which may vary depending on the path. In a cyclic process, deshalb, the entropy of the system at the beginning of the cycle must equal the entropy at the end of the cycle, {displaystyle Delta S=0} , regardless of whether the process is reversible or irreversible. In the irreversible case, entropy will be created in the system, and more entropy must be extracted than was added {Anzeigestil (Delta S_{Text{surr}}>0)} in order to return the system to its original state. In the reversible case, no entropy is created and the amount of entropy added is equal to the amount extracted.

If the amount of energy added by heating can be measured during the process, and the temperature can be measured during the process, the Clausius inequality can be used to determine whether the process is reversible or irreversible by carrying out the integration in the Clausius inequality.

Proof The temperature that enters in the denominator of the integrand in the Clausius inequality is actually the temperature of the external reservoir with which the system exchanges heat. At each instant of the process, the system is in contact with an external reservoir.

Because of the Second Law of Thermodynamics, in each infinitesimal heat exchange process between the system and the reservoir, the net change in entropy of the "universe", so to say, ist {displaystyle dS_{Text{Total}}=dS_{Text{Sys}}+dS_{Text{Res}}geq 0} .

When the system takes in heat by an infinitesimal amount {displaystyle delta Q_{1}} ( {displaystyle geq 0} ), for the net change in entropy {displaystyle dS_{{Text{Total}}_{1}}} in this step to be positive, the temperature of the "hot" reservoir {Anzeigestil T_{Text{Hot}}} needs to be slightly greater than the temperature of the system at that instant. If the temperature of the system is given by {Anzeigestil T_{1}} at that instant, dann {textstyle dS_{{Text{Sys}}_{1}}={frac {delta Q_{1}}{T_{1}}}} , und {Anzeigestil T_{Text{Hot}}geq T_{1}} forces us to have: {displaystyle -dS_{{Text{Res}}_{1}}={frac {delta Q_{1}}{T_{Text{Hot}}}}leq {frac {delta Q_{1}}{T_{1}}}=dS_{{Text{Sys}}_{1}}} This means the magnitude of the entropy "loss" from the reservoir, {textstyle left|dS_{{Text{Res}}_{1}}Rechts|={frac {delta Q_{1}}{T_{Text{Hot}}}}} is less than the magnitude of the entropy "gain" {textstyle dS_{{Text{Sys}}_{1}}={frac {delta Q_{1}}{T_{1}}}} ( {displaystyle geq 0} ) by the system: Ähnlich, when the system at temperature {Anzeigestil T_{2}} expels heat in magnitude {displaystyle -delta Q_{2}} ( {displaystyle delta Q_{2}leq 0} ) into a colder reservoir (at temperature {Anzeigestil T_{Text{Cold}}leq T_{2}} ) in an infinitesimal step, then again, for the Second Law of Thermodynamics to hold, one would have, in an exactly similar manner: {displaystyle -dS_{{Text{Res}}_{2}}={frac {delta Q_{2}}{T_{Text{Cold}}}}leq {frac {delta Q_{2}}{T_{2}}}=dS_{{Text{Sys}}_{2}}} Hier, the amount of heat 'absorbed' by the system is given by {displaystyle delta Q_{2}} ( {displaystyle leq 0} ), signifying that heat is transferring from the system to the reservoir, mit {displaystyle dS_{{Text{Sys}}_{2}}leq 0} . The magnitude of the entropy gained by the reservoir, {textstyle dS_{{Text{Res}}_{2}}={frac {|delta Q_{2}|}{T_{Text{cold}}}}} is greater than the magnitude of the entropy loss of the system {Anzeigestil links|dS_{{Text{Sys}}_{2}}Rechts|} Since the total change in entropy for the system is 0 in a cyclic process, if one adds all the infinitesimal steps of heat intake and heat expulsion from the reservoir, signified by the previous two equations, with the temperature of the reservoir at each instant given by {Anzeigestil T_{Text{surr}}} , man bekommt, {displaystyle -oint dS_{Text{Res}}=oint {frac {delta Q}{T_{Text{surr}}}}leq oint dS_{Text{Sys}}=0.} Im Speziellen, {displaystyle oint {frac {delta Q}{T_{Text{surr}}}}leq 0,} which was to be proven.

Zusammenfassend, (the inequality in the third statement below, being obviously guaranteed by the second law of thermodynamics, which is the basis of our calculation), {displaystyle oint dS_{Text{Res}}geq 0} {displaystyle oint dS_{Text{Sys}}=0} (as hypothesized) {displaystyle oint dS_{Text{Total}}=oint dS_{Text{Res}}+oint dS_{Text{Sys}}geq 0} For a reversible cyclic process, there is no generation of entropy in each of the infinitesimal heat transfer processes, so the following equality holds, {displaystyle oint {frac {delta Q_{Text{rev}}}{T}}=0.} Daher, the Clausius inequality is a consequence of applying the second law of thermodynamics at each infinitesimal stage of heat transfer, and is thus in a sense a weaker condition than the Second Law itself.

See also Kelvin-Planck statement Carnot's theorem (thermodynamics) Carnot heat engine Introduction to entropy References ^ Clausius theorem at Wolfram Research ^ Finn, Colin B. P. Thermal Physics. 2und Aufl., CRC-Presse, 1993. ^ Giancoli, Douglas C. Physics: Principles with Applications. 6Das D., Pearson/Prentice Hall, 2005. ^ Mortimer, R. G. Physical Chemistry. 3Dr. Ed., p. 120, Akademische Presse, 2008. Further reading Morton, EIN. S., and P.J. Beckett. Basic Thermodynamics. New York: Philosophical Library Inc., 1969. Print. Saad, Michel A. Thermodynamics for Engineers. Englewood Cliffs: Lehrlingshalle, 1966. Print. Hsieh, Jui Sheng. Principles of Thermodynamics. Washington, Gleichstrom: Scripta Book Company, 1975. Print. Zemansky, Mark W. Heat and Thermodynamics. 4Das D. New York: McGwaw-Hill Book Company, 1957. Print. Clausius, Rudolf. The Mechanical Theory of Heat. London: Taylor and Francis, 1867. eBook External links Judith McGovern (2004-03-17). "Proof of Clausius's theorem". Archived from the original on July 19, 2011. Oktober abgerufen 4, 2010. "The Clausius Inequality And The Mathematical Statement Of The Second Law" (Pdf). Oktober abgerufen 5, 2010. The Mechanical Theory of Heat (eBook). Dezember abgerufen 1, 2011. Kategorien: Laws of thermodynamicsPhysics theorems

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