File Name: difference between heat and work in thermodynamics .zip
The key difference between work and heat is that work is the ordered motion in one direction whereas heat is the random motion of molecules. Work and heat are the two most important concepts of thermodynamics.
The laws of thermodynamics define a group of physical quantities, such as temperature , energy , and entropy , that characterize thermodynamic systems in thermodynamic equilibrium. The laws also use various parameters for thermodynamic processes , such as thermodynamic work and heat , and establish relationships between them. They state empirical facts that form a basis of precluding the possibility of certain phenomena, such as perpetual motion.
In addition to their use in thermodynamics , they are important fundamental laws of physics in general, and are applicable in other natural sciences. Traditionally, thermodynamics has recognized three fundamental laws, simply named by an ordinal identification, the first law, the second law, and the third law. The zeroth law of thermodynamics defines thermal equilibrium and forms a basis for the definition of temperature: If two systems are each in thermal equilibrium with a third system, then they are in thermal equilibrium with each other.
The first law of thermodynamics states that, when energy passes into or out of a system as work , heat , or matter , the system's internal energy changes in accord with the law of conservation of energy. The second law of thermodynamics states that in a natural thermodynamic process , the sum of the entropies of the interacting thermodynamic systems never decreases.
Another form of the statement is that heat does not spontaneously pass from a colder body to a warmer body. The third law of thermodynamics states that a system's entropy approaches a constant value as the temperature approaches absolute zero.
With the exception of non-crystalline solids glasses the entropy of a system at absolute zero is typically close to zero. The first and second law prohibit two kinds of perpetual motion machines, respectively: the perpetual motion machine of the first kind which produces work with no energy input, and the perpetual motion machine of the second kind which spontaneously converts thermal energy into mechanical work.
The history of thermodynamics is fundamentally interwoven with the history of physics and history of chemistry and ultimately dates back to theories of heat in antiquity. The laws of thermodynamics are the result of progress made in this field over the nineteenth and early twentieth centuries. The first established thermodynamic principle, which eventually became the second law of thermodynamics, was formulated by Sadi Carnot in in his book Reflections on the Motive Power of Fire.
By , as formalized in the works of scientists such as Rudolf Clausius and William Thomson , what are now known as the first and second laws were established. Later, Nernst's theorem or Nernst's postulate , which is now known as the third law, was formulated by Walther Nernst over the period — While the numbering of the laws is universal today, various textbooks throughout the 20th century have numbered the laws differently.
In some fields, the second law was considered to deal with the efficiency of heat engines only, whereas what was called the third law dealt with entropy increases. Gradually, this resolved itself and a zeroth law was later added to allow for a self-consistent definition of temperature. Additional laws have been suggested, but have not achieved the generality of the four accepted laws, and are generally not discussed in standard textbooks.
The zeroth law of thermodynamics provides for the foundation of temperature as an empirical parameter in thermodynamic systems and establishes the transitive relation between the temperatures of multiple bodies in thermal equilibrium. The law may be stated in the following form:. If two systems are both in thermal equilibrium with a third system, then they are in thermal equilibrium with each other. Though this version of the law is one of the most commonly stated versions, it is only one of a diversity of statements that are labeled as "the zeroth law".
Some statements go further, so as to supply the important physical fact that temperature is one-dimensional and that one can conceptually arrange bodies in a real number sequence from colder to hotter.
These concepts of temperature and of thermal equilibrium are fundamental to thermodynamics and were clearly stated in the nineteenth century. The name 'zeroth law' was invented by Ralph H. Fowler in the s, long after the first, second, and third laws were widely recognized. The law allows the definition of temperature in a non-circular way without reference to entropy, its conjugate variable. Such a temperature definition is said to be 'empirical'. The first law of thermodynamics is a version of the law of conservation of energy , adapted for thermodynamic processes.
In general, the conservation law states that the total energy of an isolated system is constant; energy can be transformed from one form to another, but can be neither created nor destroyed. In a closed system i. Note, an alternate sign convention , not used in this article, is to define W as the work done on the system by its surroundings :. When two initially isolated systems are combined into a new system, then the total internal energy of the new system, U system , will be equal to the sum of the internal energies of the two initial systems, U 1 and U 2 :.
Combining these principles leads to one traditional statement of the first law of thermodynamics: it is not possible to construct a machine which will perpetually output work without an equal amount of energy input to that machine. Or more briefly, a perpetual motion machine of the first kind is impossible.
The second law of thermodynamics indicates the irreversibility of natural processes, and, in many cases, the tendency of natural processes to lead towards spatial homogeneity of matter and energy, and especially of temperature. It can be formulated in a variety of interesting and important ways. One of the simplest is the Clausius statement, that heat does not spontaneously pass from a colder to a hotter body.
It implies the existence of a quantity called the entropy of a thermodynamic system. In terms of this quantity it implies that. When two initially isolated systems in separate but nearby regions of space, each in thermodynamic equilibrium with itself but not necessarily with each other, are then allowed to interact, they will eventually reach a mutual thermodynamic equilibrium.
The sum of the entropies of the initially isolated systems is less than or equal to the total entropy of the final combination.
Equality occurs just when the two original systems have all their respective intensive variables temperature, pressure equal; then the final system also has the same values. The second law is applicable to a wide variety of processes, both reversible and irreversible. While reversible processes are a useful and convenient theoretical limiting case, all natural processes are irreversible.
A prime example of this irreversibility is the transfer of heat by conduction or radiation. It was known long before the discovery of the notion of entropy that when two bodies, initially of different temperatures, come into direct thermal connection, then heat immediately and spontaneously flows from the hotter body to the colder one. Entropy may also be viewed as a physical measure concerning the microscopic details of the motion and configuration of a system, when only the macroscopic states are known.
Such details are often referred to as disorder on a microscopic or molecular scale, and less often as dispersal of energy. For two given macroscopically specified states of a system, there is a mathematically defined quantity called the 'difference of information entropy between them'. This defines how much additional microscopic physical information is needed to specify one of the macroscopically specified states, given the macroscopic specification of the other — often a conveniently chosen reference state which may be presupposed to exist rather than explicitly stated.
A final condition of a natural process always contains microscopically specifiable effects which are not fully and exactly predictable from the macroscopic specification of the initial condition of the process.
This is why entropy increases in natural processes — the increase tells how much extra microscopic information is needed to distinguish the initial macroscopically specified state from the final macroscopically specified state.
The third law of thermodynamics can be stated as: . A system's entropy approaches a constant value as its temperature approaches absolute zero. At zero temperature, the system must be in the state with the minimum thermal energy, the ground state. The constant value not necessarily zero of entropy at this point is called the residual entropy of the system. Note that, with the exception of non-crystalline solids e.
Microstates are used here to describe the probability of a system being in a specific state, as each microstate is assumed to have the same probability of occurring, so macroscopic states with fewer microstates are less probable.
In general, entropy is related to the number of possible microstates according to the Boltzmann principle :.
The Onsager reciprocal relations have been considered the fourth law of thermodynamics. These relations are derived from statistical mechanics under the principle of microscopic reversibility in the absence of magnetic fields. Given a set of extensive parameters X i energy, mass, entropy, number of particles and thermodynamic forces F i related to intrinsic parameters, such as temperature and pressure , the Onsager theorem states that .
From Wikipedia, the free encyclopedia. Axiomatic basis of thermodynamics. The classical Carnot heat engine. Classical Statistical Chemical Quantum thermodynamics. Zeroth First Second Third. System properties. Note: Conjugate variables in italics. Work Heat. Material properties.
Carnot's theorem Clausius theorem Fundamental relation Ideal gas law. Free energy Free entropy. History Culture. History General Entropy Gas laws. Entropy and time Entropy and life Brownian ratchet Maxwell's demon Heat death paradox Loschmidt's paradox Synergetics.
Caloric theory Theory of heat. Heat ". Thermodynamics Heat engines. Nucleation Self-assembly Self-organization Order and disorder. Main article: History of thermodynamics. See also: Timeline of thermodynamics and Philosophy of thermal and statistical physics.
See also: Thermodynamic cycle. Kroemer, H. Thermal Physics , second edition, W. Thermodynamics and Statistical Mechanics , vol. Bopp, J. Meixner, translated by J. Kestin, Academic Press, New York, p. Chapter 1, 'An Outline of Thermodynamical Structure', pp. Journal of Chemical Education. Encyclopedia Britannica. Retrieved Categories : Laws of thermodynamics Scientific laws.
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Work and heat are the two most important theories in thermodynamics. Both are highly related but they are not the same. The Key Difference Between Heat and.
The laws of thermodynamics define a group of physical quantities, such as temperature , energy , and entropy , that characterize thermodynamic systems in thermodynamic equilibrium. The laws also use various parameters for thermodynamic processes , such as thermodynamic work and heat , and establish relationships between them. They state empirical facts that form a basis of precluding the possibility of certain phenomena, such as perpetual motion. In addition to their use in thermodynamics , they are important fundamental laws of physics in general, and are applicable in other natural sciences. Traditionally, thermodynamics has recognized three fundamental laws, simply named by an ordinal identification, the first law, the second law, and the third law.
Path Function and Point Function. Path function and Point function are introduced to identify the variables of thermodynamics.
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