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| {{thermodynamics|cTopic=[[Thermodynamic equations|Equations]]}}
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| '''Carnot's theorem''', developed in 1824 by [[Nicolas Léonard Sadi Carnot]], also called ''Carnot's rule'' is a principle that specifies limits on the maximum efficiency any [[heat engine]] can obtain, which thus solely depends on the difference between the hot and cold temperature reservoirs.
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| Carnot's theorem states:
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| *All heat engines between two heat reservoirs are less efficient than a [[Carnot engine]] operating between the same reservoirs.
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| *Every [[Carnot engine]] between a pair of heat reservoirs is equally efficient, regardless of the working substance employed or the operation details.
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| The formula for this maximum efficiency is
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| :<math>\eta_{\text{max}} = \eta_{\text{Carnot}} = 1 - \frac{T_C}{T_H}</math>
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| where ''T<sub>C</sub>'' is the [[absolute temperature]] of the cold reservoir, ''T<sub>H</sub>'' is the [[absolute temperature]] of the hot reservoir, and the efficiency <math>\eta</math> is the ratio of the work done by the engine to the heat drawn out of the hot reservoir.
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| Based on modern thermodynamics, Carnot's theorem is a result of the [[second law of thermodynamics]]. Historically, however, it was based on contemporary [[caloric theory]] and preceded the establishment of the second law.<ref>{{cite web|url=http://www.sussex.ac.uk/chemistry/documents/a_thermodynamics_history.pdf|title=A Very Brief History of Thermodynamics|author=John Murrell|accessdate=October 5, 2010}}</ref>
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| ==Proof==
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| [[File:Carnot theorem paradox.jpg|thumb|300px|An impossible situation: A heat engine cannot drive a less efficient (reversible) heat engine without violating the second law of thermodynamics.]]
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| The proof of the Carnot theorem is a [[proof by contradiction]], or [[reductio ad absurdum]], as illustrated by the figure showing two heat engines operating between two reservoirs of different temperature. The heat engine with more efficiency (<math>\eta_M</math>) is driving a heat engine with less efficiency (<math>\eta_L</math>), causing the latter to act as a [[heat pump]]. This pair of engines receives no outside energy, and operates solely on the energy released when heat is transferred from the hot and into the cold reservoir. However, if <math>\eta_M>\eta_L</math>, then the net heat flow would be backwards, i.e., into the hot reservoir:
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| :<math>Q^\text{out}_\text{hot} = Q < \frac{\eta_M}{\eta_L}Q=Q^\text{in}_\text{hot}</math>.
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| It is [[Second law of thermodynamics#Controversies|generally agreed]] that this is impossible because it violates the [[second law of thermodynamics]].
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| We begin by verifying the values of work and heat flow depicted in the figure. First, we must point out an important caveat: the engine with less efficiency (<math>\eta_L</math>) is being driven as a heat pump, and therefore must be a ''[[reversible process (thermodynamics)|reversible]]'' engine. If the less efficient engine (<math>\eta_L</math>) is not reversible, then the device could be built, but the expressions for work and heat flow shown in the figure would not be valid.
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| By restricting our discussion to cases where engine (<math>\eta_L</math>) has less efficiency than engine (<math>\eta_M</math>), we are able to simplify notation by adopting the convention that all symbols, <math>Q</math> and <math>W</math> represent [[Sign (mathematics)#Terminology for signs|non-negative]] quantities (since the direction of energy flow never changes sign in all cases where <math>\eta_L\leqslant\eta_M</math>). Conservation of energy demands that for each engine, the energy which enters, <math> E_{in} </math>, must equal the energy which exits, <math> E_{out} </math>:
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| :<math>E_{in}^{M} = Q = (1-\eta_M)Q + \eta Q_M = E_{out}^{M} </math>,
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| :<math>E_{in}^{L} = \eta_M Q + \eta_M Q \left(\frac{1}{\eta_{L}}- 1 \right )=\frac{\eta_M}{\eta_L}Q = E_{out}^{L} </math>,
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| The figure is also consistent with the definition of [[Heat engine#Efficiency|efficiency]] as <math>\eta=W/Q_h</math> for both engines: | |
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| :<math>\eta_M= \frac{W_M}{Q^M_h}=\frac{\eta_M Q}{Q}=\eta_M</math>,
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| :<math> \eta_L=\frac{W_L}{Q^L_h}=\frac{\eta_M Q}{\frac{\eta_M}{\eta_L}Q}=\eta_L</math>.
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| It may seem odd that a hypothetical heat pump with low efficiency is being used to violate the second law of thermodynamics, but the [[figure of merit]] for refrigerator units is not efficiency, <math>W/Q_h</math> , but the [[coefficient of performance]] (COP),<ref>{{cite book|last=Tipler|first=Paul|title=Physics for Scientists and Engineers|year=2008|publisher=Freeman|isbn=9781429201322|edition=6th|coauthors=Mosca, G.|chapter=19.2, 19.7}}</ref>
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| which is <math>Q_c/W</math>. A reversible heat engine with low thermodynamic efficiency, <math>W/Q_h</math> delivers more heat to the hot reservoir for a given amount of work when it is being driven as a heat pump.
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| Having established that the heat flow values shown in the figure are correct, Carnot's theorem may be proven for irreversible and the reversible heat engines.<ref name=CarnotThoerem>{{cite web
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| |url=http://seit.unsw.adfa.edu.au/staff/sites/hrp/Literature/articles/CarnotTheorem.pdf
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| |title=Lecture 10: Carnot theorem
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| |date=Feb 7,2005
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| |accessdate=October 5, 2010}}</ref>
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| ===Reversible engines===
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| To see that every reversible engine operating between reservoirs <math>T_1</math> and <math>T_2</math> must have the same efficiency, assume that two reversible heat engines have different values of <math>\eta</math>, and let the more efficient engine (M) drive the less efficient engine (L) as a heat pump. As the figure shows, this will cause heat to flow from the cold to the hot reservoir without any external work or energy, which violates the second law of thermodynamics. Therefore both (reversible) heat engines have the same efficiency, and we conclude that:
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| :''All reversible engines that operate between the same two heat reservoirs have the same efficiency.''
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| This is an important result because it helps establish the [[Clausius theorem]], which implies that the change in [[entropy]] is unique for all reversible processes.,<ref>{{cite book|last=Ohanian|first=Hans|title=Principles of Physics|year=1994|publisher=W.W. Norton and Co.|isbn=039395773X|pages=438}}</ref>
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| :<math>\Delta S = \int_a^b \frac {dQ_{rev}}T </math>,
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| over all paths (from '''''a''''' to '''''b''''' in ''V-T'' space). If this integral were not path independent, then entropy, S, would lose its status as a [[state function|state variable]].<ref>http://faculty.wwu.edu/vawter/PhysicsNet/Topics/ThermLaw2/ThermalProcesses.html, and http://www.itp.phys.ethz.ch/education/hs10/stat/slides/Laws_TD.pdf. Both retrieved 13 December 2013.</ref>
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| ===Irreversible engines===
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| If one of the engines is irreversible, it must be the (M) engine, placed so that it reverse drives the less efficient but reversible (L) engine. But if this irreversible engine is more efficient than the reversible engine, (i.e., if <math>\eta_M >\eta_L</math>), then the second law of thermodynamics is violated. And, since the Carnot cycle represents a reversible engine, we have the first part of Carnot's theorem:
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| :''No irreversible engine is more efficient that the Carnot engine.''
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| ==Definition of thermodynamic temperature==
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| {{main|Thermodynamic temperature#Definition of thermodynamic temperature|l1=Definition of thermodynamic temperature
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| }}
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| The efficiency of the engine is the work divided by the heat introduced to the system or
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| {{NumBlk|:|<math>\eta = \frac {w_{cy}}{q_H} = \frac{q_H-q_C}{q_H} = 1 - \frac{q_C}{q_H}</math>|{{EquationRef|1}}}}
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| where w<sub>cy</sub> is the work done per cycle. Thus, the efficiency depends only on q<sub>C</sub>/q<sub>H</sub>.
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| Because all reversible engines operating between the same heat reservoirs are equally efficient, any reversible heat engine operating between temperatures ''T''<sub>1</sub> and ''T''<sub>2</sub> must have the same efficiency, meaning, the efficiency is the function of the temperatures only:
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| {{NumBlk|:|<math>\frac{q_C}{q_H} = f(T_H,T_C)</math>|{{EquationRef|2}}}}
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| In addition, a reversible heat engine operating between temperatures ''T''<sub>1</sub> and ''T''<sub>3</sub> must have the same efficiency as one consisting of two cycles, one between ''T''<sub>1</sub> and another (intermediate) temperature ''T''<sub>2</sub>, and the second between ''T''<sub>2</sub>and''T''<sub>3</sub>. This can only be the case if
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| :<math>
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| f(T_1,T_3) = \frac{q_3}{q_1} = \frac{q_2 q_3} {q_1 q_2} = f(T_1,T_2)f(T_2,T_3).
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| </math>
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| Specializing to the case that <math>T_1</math> is a fixed reference temperature: the temperature of the triple point of water. Then for any''T''<sub>2</sub>and ''T''<sub>3</sub>,
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| :<math>f(T_2,T_3) = \frac{f(T_1,T_3)}{f(T_1,T_2)} = \frac{273.16 \cdot f(T_1,T_3)}{273.16 \cdot f(T_1,T_2)}.</math>
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| Therefore, if thermodynamic temperature is defined by
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| :<math>T = 273.16 \cdot f(T_1,T) \,</math>
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| then the function ''f'', viewed as a function of thermodynamic temperature, is
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| :<math>f(T_2,T_3) = \frac{T_3}{T_2},</math>
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| and the reference temperature ''T''<sub>1</sub> has the value 273.16. (Of course any reference temperature and any positive numerical value could be used—the choice here corresponds to the Kelvin scale.)
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| It follows immediately that
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| {{NumBlk|:|<math>\frac{q_C}{q_H} = f(T_H,T_C) = \frac{T_C}{T_H}</math>|{{EquationRef|3}}}}
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| Substituting Equation {{EquationNote|3}} back into Equation {{EquationNote|1}} gives a relationship for the efficiency in terms of temperature:
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| {{NumBlk|:|<math>\eta = 1 - \frac{q_C}{q_H} = 1 - \frac{T_C}{T_H}</math>|{{EquationRef|4}}}}
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| ==Applicability to fuel cells and batteries==
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| Since [[fuel cell]]s and [[Battery (electricity)|batteries]] can generate useful power when all components of the system are at the same temperature (<math>T=T_H=T_C</math>), they are clearly not limited by Carnot's theorem, which states that no power can be generated when <math>T_H=T_C</math>. This is because Carnot's theorem applies to engines converting thermal energy to work, whereas fuel cells and batteries instead convert chemical energy to work.<ref>{{cite web
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| |url=http://docs.google.com/viewer?a=v&q=cache:KkaC5XqVzVgJ:filer.case.edu/org/hsfcproject/Unit%252036/36.1.3%2520Fuel%2520Cell%2520versus%2520Carnot%2520Efficiency.ppt+%22carnot+limit%22+%22fuel+cell%22&hl=en&gl=us&pid=bl&srcid=ADGEESj0jJDxV7N40e6SinnUfC9X_wqU6GHB4aPX6BlFRSYsfeixt1hGvyGLMAthvrl_Ws6k4r-Z8AdtYkjDqhVrIUwjO6rSA8y5JnGnqt73LWITIpc3KdeTUBe24GkaZcLs1BpHUxh5&sig=AHIEtbROSMlotD3mw6tegO0_v-uhvVwI2g
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| |title=Fuel Cell versus Carnot Efficiency
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| |accessdate=Feb 20, 2011}}</ref> Nevertheless, the [[second law of thermodynamics]] still provides restrictions on fuel cell and battery energy conversion.<ref>{{cite conference|url=http://eprints.iisc.ernet.in/42739/
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| |title=Fuel cell efficiency redefined : Carnot limit reassessed
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| |last1=Jacob|first1=Kallarackel T|last2=Jain|first2=Saurabh|conference=Q1 - Ninth International Symposium on Solid Oxide Fuel Cells (SOFC IX)|date=July 2005|location=USA}}</ref>
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| ==References==
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| {{reflist}}
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| {{DEFAULTSORT:Carnot's Theorem (Thermodynamics)}}
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| [[Category:Thermodynamics]]
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| [[Category:Physics theorems]]
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