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    The Heat Is On Deutsch

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    Viele übersetzte Beispielsätze mit "the heat is on" – Deutsch-Englisch Wörterbuch und Suchmaschine für Millionen von Deutsch-Übersetzungen. Übersetzung im Kontext von „heat is on“ in Englisch-Deutsch von Reverso Context: Deutsche Welle Global Media Forum will be the third in a row titled The. Englisch-Deutsch-Übersetzungen für The heat is on im Online-Wörterbuch stemvvvrobdebes2014.nl (Deutschwörterbuch). Übersetzung Englisch-Deutsch für the heat is on im PONS Online-Wörterbuch nachschlagen! Gratis Vokabeltrainer, Verbtabellen, Aussprachefunktion. Lernen Sie die Übersetzung für 'The heat is on.' in LEOs Englisch ⇔ Deutsch Wörterbuch. Mit Flexionstabellen der verschiedenen Fälle und Zeiten.

    The Heat Is On Deutsch

    The heat is on. Übersetzungen auf Deutsch: Deutsch Es wird Druck ausgeübt. Verwandte Phrasen. the heat is on Bedeutung, Definition the heat is on: 1. If you say the heat is on, you mean that a time of great activity and/or pressure has begun. Viele übersetzte Beispielsätze mit "the heat is on" – Deutsch-Englisch Wörterbuch und Suchmaschine für Millionen von Deutsch-Übersetzungen.

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    Möchten Sie ein Wort, eine Phrase oder eine Übersetzung hinzufügen? During the colder months when the heating is on , all the rooms should be ventilated briefly with a draught approximately every 2 hours during the day. Klicken Sie auf die Pfeile, um die Übersetzungsrichtung zu ändern. Physics tells us that supplying or extracting heat does not change the heat content of a system , it changes the internal energy or en- thalpy , depending on how the heat is supplied.. Choose your language. The Top Models of the High Class Escorts Munich are skilled in their city and support you not only to the magnificent sights Heat is on!

    The Heat Is On Deutsch Video

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    In a mixture of water vapour and air, the sensible heat is the energy necessary to produce a particular temperature change excluding any energy required for a phase change.

    Article Media. Info Print Print. Table Of Contents. Submit Feedback. Thank you for your feedback. Introduction Heat as a form of energy Heat transfer.

    The Editors of Encyclopaedia Britannica Encyclopaedia Britannica's editors oversee subject areas in which they have extensive knowledge, whether from years of experience gained by working on that content or via study for an advanced degree See Article History.

    Britannica Quiz. All About Physics Quiz. What is the phenomenon of Raman scattering, named after Indian physicist C.

    Get exclusive access to content from our First Edition with your subscription. Subscribe today. Toggle navigation HEAT. Hybrid AI processing data with smart AI and smart er humans.

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    Air is a mixture of gases and water vapour, and it is possible for the water present in the air to change phase; i. To distinguish between the energy associated with the phase change the latent heat and the energy required for a temperature change, the concept of sensible heat was introduced.

    In a mixture of water vapour and air, the sensible heat is the energy necessary to produce a particular temperature change excluding any energy required for a phase change.

    Article Media. Info Print Print. Table Of Contents. Submit Feedback. Thank you for your feedback. Introduction Heat as a form of energy Heat transfer.

    The Editors of Encyclopaedia Britannica Encyclopaedia Britannica's editors oversee subject areas in which they have extensive knowledge, whether from years of experience gained by working on that content or via study for an advanced degree See Article History.

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    In this scenario, the increase in enthalpy is equal to the quantity of heat added to the system. Since many processes do take place at constant pressure, or approximately at atmospheric pressure, the enthalpy is therefore sometimes given the misleading name of 'heat content'.

    In terms of the natural variables S and P of the state function H , this process of change of state from state 1 to state 2 can be expressed as.

    It is known that the temperature T S , P is identically stated by. Speculation on thermal energy or "heat" as a separate form of matter has a long history, see caloric theory , phlogiston and fire classical element.

    The modern understanding of thermal energy originates with Thompson 's mechanical theory of heat An Experimental Enquiry Concerning the Source of the Heat which is Excited by Friction , postulating a mechanical equivalent of heat.

    The theory of classical thermodynamics matured in the s to s. John Tyndall 's Heat Considered as Mode of Motion was instrumental in popularising the idea of heat as motion to the English-speaking public.

    The theory was developed in academic publications in French, English and German. From an early time, the French technical term chaleur used by Carnot was taken as equivalent to the English heat and German Wärme lit.

    The process function Q was introduced by Rudolf Clausius in Clausius described it with the German compound Wärmemenge , translated as "amount of heat".

    James Clerk Maxwell in his Theory of Heat outlines four stipulations for the definition of heat:. The process function Q is referred to as Wärmemenge by Clausius, or as "amount of heat" in translation.

    Use of "heat" as an abbreviated form of the specific concept of "quantity of energy transferred as heat" led to some terminological confusion by the early 20th century.

    The generic meaning of "heat", even in classical thermodynamics, is just "thermal energy". Leonard Benedict Loeb in his Kinetic Theory of Gases makes a point of using "quanitity of heat" or "heat—quantity" when referring to Q : [31].

    The internal energy U X of a body in an arbitrary state X can be determined by amounts of work adiabatically performed by the body on its surroundings when it starts from a reference state O.

    Such work is assessed through quantities defined in the surroundings of the body. It is supposed that such work can be assessed accurately, without error due to friction in the surroundings; friction in the body is not excluded by this definition.

    The adiabatic performance of work is defined in terms of adiabatic walls, which allow transfer of energy as work, but no other transfer, of energy or matter.

    In particular they do not allow the passage of energy as heat. According to this definition, work performed adiabatically is in general accompanied by friction within the thermodynamic system or body.

    For the definition of quantity of energy transferred as heat, it is customarily envisaged that an arbitrary state of interest Y is reached from state O by a process with two components, one adiabatic and the other not adiabatic.

    For convenience one may say that the adiabatic component was the sum of work done by the body through volume change through movement of the walls while the non-adiabatic wall was temporarily rendered adiabatic, and of isochoric adiabatic work.

    Then the non-adiabatic component is a process of energy transfer through the wall that passes only heat, newly made accessible for the purpose of this transfer, from the surroundings to the body.

    The change in internal energy to reach the state Y from the state O is the difference of the two amounts of energy transferred. In this definition, for the sake of conceptual rigour, the quantity of energy transferred as heat is not specified directly in terms of the non-adiabatic process.

    It is defined through knowledge of precisely two variables, the change of internal energy and the amount of adiabatic work done, for the combined process of change from the reference state O to the arbitrary state Y.

    It is important that this does not explicitly involve the amount of energy transferred in the non-adiabatic component of the combined process.

    It is assumed here that the amount of energy required to pass from state O to state Y , the change of internal energy, is known, independently of the combined process, by a determination through a purely adiabatic process, like that for the determination of the internal energy of state X above.

    The rigour that is prized in this definition is that there is one and only one kind of energy transfer admitted as fundamental: energy transferred as work.

    Energy transfer as heat is considered as a derived quantity. The uniqueness of work in this scheme is considered to guarantee rigor and purity of conception.

    The conceptual purity of this definition, based on the concept of energy transferred as work as an ideal notion, relies on the idea that some frictionless and otherwise non-dissipative processes of energy transfer can be realized in physical actuality.

    The second law of thermodynamics, on the other hand, assures us that such processes are not found in nature.

    That heat is an appropriate and natural primitive for thermodynamics was already accepted by Carnot. Its continued validity as a primitive element of thermodynamical structure is due to the fact that it synthesizes an essential physical concept, as well as to its successful use in recent work to unify different constitutive theories.

    It is sometimes proposed that this traditional kind of presentation necessarily rests on "circular reasoning"; against this proposal, there stands the rigorously logical mathematical development of the theory presented by Truesdell and Bharatha This alternative approach admits calorimetry as a primary or direct way to measure quantity of energy transferred as heat.

    It relies on temperature as one of its primitive concepts, and used in calorimetry. Such processes are not restricted to adiabatic transfers of energy as work.

    They include calorimetry, which is the commonest practical way of finding internal energy differences. It is calculated from the difference of the internal energies of the initial and final states of the system, and from the actual work done by the system during the process.

    That internal energy difference is supposed to have been measured in advance through processes of purely adiabatic transfer of energy as work, processes that take the system between the initial and final states.

    In fact, the actual physical existence of such adiabatic processes is indeed mostly supposition, and those supposed processes have in most cases not been actually verified empirically to exist.

    Referring to conduction, Partington writes: "If a hot body is brought in conducting contact with a cold body, the temperature of the hot body falls and that of the cold body rises, and it is said that a quantity of heat has passed from the hot body to the cold body.

    Referring to radiation, Maxwell writes: "In Radiation, the hotter body loses heat, and the colder body receives heat by means of a process occurring in some intervening medium which does not itself thereby become hot.

    Maxwell writes that convection as such "is not a purely thermal phenomenon". If, however, the convection is enclosed and circulatory, then it may be regarded as an intermediary that transfers energy as heat between source and destination bodies, because it transfers only energy and not matter from the source to the destination body.

    In accordance with the first law for closed systems, energy transferred solely as heat leaves one body and enters another, changing the internal energies of each.

    Transfer, between bodies, of energy as work is a complementary way of changing internal energies. Though it is not logically rigorous from the viewpoint of strict physical concepts, a common form of words that expresses this is to say that heat and work are interconvertible.

    Cyclically operating engines, that use only heat and work transfers, have two thermal reservoirs, a hot and a cold one.

    They may be classified by the range of operating temperatures of the working body, relative to those reservoirs. In a heat engine, the working body is at all times colder than the hot reservoir and hotter than the cold reservoir.

    In a sense, it uses heat transfer to produce work. In a heat pump, the working body, at stages of the cycle, goes both hotter than the hot reservoir, and colder than the cold reservoir.

    In a sense, it uses work to produce heat transfer. In classical thermodynamics, a commonly considered model is the heat engine.

    It consists of four bodies: the working body, the hot reservoir, the cold reservoir, and the work reservoir. A cyclic process leaves the working body in an unchanged state, and is envisaged as being repeated indefinitely often.

    Work transfers between the working body and the work reservoir are envisaged as reversible, and thus only one work reservoir is needed.

    But two thermal reservoirs are needed, because transfer of energy as heat is irreversible. A single cycle sees energy taken by the working body from the hot reservoir and sent to the two other reservoirs, the work reservoir and the cold reservoir.

    The hot reservoir always and only supplies energy and the cold reservoir always and only receives energy. The second law of thermodynamics requires that no cycle can occur in which no energy is received by the cold reservoir.

    Heat engines achieve higher efficiency when the difference between initial and final temperature is greater. Another commonly considered model is the heat pump or refrigerator.

    Again there are four bodies: the working body, the hot reservoir, the cold reservoir, and the work reservoir. A single cycle starts with the working body colder than the cold reservoir, and then energy is taken in as heat by the working body from the cold reservoir.

    Then the work reservoir does work on the working body, adding more to its internal energy, making it hotter than the hot reservoir.

    The hot working body passes heat to the hot reservoir, but still remains hotter than the cold reservoir. Then, by allowing it to expand without doing work on another body and without passing heat to another body, the working body is made colder than the cold reservoir.

    It can now accept heat transfer from the cold reservoir to start another cycle. The device has transported energy from a colder to a hotter reservoir, but this is not regarded as by an inanimate agency; rather, it is regarded as by the harnessing of work.

    This is because work is supplied from the work reservoir, not just by a simple thermodynamic process, but by a cycle of thermodynamic operations and processes, which may be regarded as directed by an animate or harnessing agency.

    Accordingly, the cycle is still in accord with the second law of thermodynamics. The efficiency of a heat pump is best when the temperature difference between the hot and cold reservoirs is least.

    Functionally, such engines are used in two ways, distinguishing a target reservoir and a resource or surrounding reservoir. A heat pump transfers heat, to the hot reservoir as the target, from the resource or surrounding reservoir.

    A refrigerator transfers heat, from the cold reservoir as the target, to the resource or surrounding reservoir. The target reservoir may be regarded as leaking: when the target leaks hotness to the surroundings, heat pumping is used; when the target leaks coldness to the surroundings, refrigeration is used.

    The engines harness work to overcome the leaks. According to Planck , there are three main conceptual approaches to heat. The other two are macroscopic approaches.

    One is the approach through the law of conservation of energy taken as prior to thermodynamics, with a mechanical analysis of processes, for example in the work of Helmholtz.

    This mechanical view is taken in this article as currently customary for thermodynamic theory. The other macroscopic approach is the thermodynamic one, which admits heat as a primitive concept, which contributes, by scientific induction [50] to knowledge of the law of conservation of energy.

    This view is widely taken as the practical one, quantity of heat being measured by calorimetry. Bailyn also distinguishes the two macroscopic approaches as the mechanical and the thermodynamic.

    It regards quantity of energy transferred as heat as a primitive concept coherent with a primitive concept of temperature, measured primarily by calorimetry.

    A calorimeter is a body in the surroundings of the system, with its own temperature and internal energy; when it is connected to the system by a path for heat transfer, changes in it measure heat transfer.

    The mechanical view was pioneered by Helmholtz and developed and used in the twentieth century, largely through the influence of Max Born.

    According to Born, the transfer of internal energy between open systems that accompanies transfer of matter "cannot be reduced to mechanics".

    Nevertheless, for the thermodynamical description of non-equilibrium processes, it is desired to consider the effect of a temperature gradient established by the surroundings across the system of interest when there is no physical barrier or wall between system and surroundings, that is to say, when they are open with respect to one another.

    The impossibility of a mechanical definition in terms of work for this circumstance does not alter the physical fact that a temperature gradient causes a diffusive flux of internal energy, a process that, in the thermodynamic view, might be proposed as a candidate concept for transfer of energy as heat.

    In this circumstance, it may be expected that there may also be active other drivers of diffusive flux of internal energy, such as gradient of chemical potential which drives transfer of matter, and gradient of electric potential which drives electric current and iontophoresis; such effects usually interact with diffusive flux of internal energy driven by temperature gradient, and such interactions are known as cross-effects.

    If cross-effects that result in diffusive transfer of internal energy were also labeled as heat transfers, they would sometimes violate the rule that pure heat transfer occurs only down a temperature gradient, never up one.

    They would also contradict the principle that all heat transfer is of one and the same kind, a principle founded on the idea of heat conduction between closed systems.

    One might to try to think narrowly of heat flux driven purely by temperature gradient as a conceptual component of diffusive internal energy flux, in the thermodynamic view, the concept resting specifically on careful calculations based on detailed knowledge of the processes and being indirectly assessed.

    In these circumstances, if perchance it happens that no transfer of matter is actualized, and there are no cross-effects, then the thermodynamic concept and the mechanical concept coincide, as if one were dealing with closed systems.

    But when there is transfer of matter, the exact laws by which temperature gradient drives diffusive flux of internal energy, rather than being exactly knowable, mostly need to be assumed, and in many cases are practically unverifiable.

    Consequently, when there is transfer of matter, the calculation of the pure 'heat flux' component of the diffusive flux of internal energy rests on practically unverifiable assumptions.

    In many writings in this context, the term "heat flux" is used when what is meant is therefore more accurately called diffusive flux of internal energy; such usage of the term "heat flux" is a residue of older and now obsolete language usage that allowed that a body may have a "heat content".

    In the kinetic theory , heat is explained in terms of the microscopic motions and interactions of constituent particles, such as electrons, atoms, and molecules.

    It is as a component of internal energy. In microscopic terms, heat is a transfer quantity, and is described by a transport theory, not as steadily localized kinetic energy of particles.

    Heat transfer arises from temperature gradients or differences, through the diffuse exchange of microscopic kinetic and potential particle energy, by particle collisions and other interactions.

    An early and vague expression of this was made by Francis Bacon. In statistical mechanics , for a closed system no transfer of matter , heat is the energy transfer associated with a disordered, microscopic action on the system, associated with jumps in occupation numbers of the energy levels of the system, without change in the values of the energy levels themselves.

    A mathematical definition can be formulated for small increments of quasi-static adiabatic work in terms of the statistical distribution of an ensemble of microstates.

    Quantity of heat transferred can be measured by calorimetry, or determined through calculations based on other quantities.

    Calorimetry is the empirical basis of the idea of quantity of heat transferred in a process. The transferred heat is measured by changes in a body of known properties, for example, temperature rise, change in volume or length, or phase change, such as melting of ice.

    A calculation of quantity of heat transferred can rely on a hypothetical quantity of energy transferred as adiabatic work and on the first law of thermodynamics.

    Such calculation is the primary approach of many theoretical studies of quantity of heat transferred. The discipline of heat transfer , typically considered an aspect of mechanical engineering and chemical engineering , deals with specific applied methods by which thermal energy in a system is generated, or converted, or transferred to another system.

    Although the definition of heat implicitly means the transfer of energy, the term heat transfer encompasses this traditional usage in many engineering disciplines and laymen language.

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