77 relations: Adiabatic process, Amount of substance, Annalen der Physik, Argon, Atmosphere (unit), Atomic mass constant, August Krönig, Avogadro constant, Avogadro's law, Bar (unit), Benoît Paul Émile Clapeyron, Boltzmann constant, Boyle's law, Calorie, Charles's law, Combined gas law, Cubic metre, Density, Divergence, Divergence theorem, Dynamic pressure, Enthalpy, Entropy, Equation of state, Equipartition theorem, First principle, Free expansion, Gas, Gas constant, Gas laws, Gay-Lussac's law, Hamiltonian mechanics, Heat capacity ratio, Helium, Helmholtz free energy, Ideal gas, Internal energy, International System of Units, Isenthalpic process, Isentropic process, Isobaric process, Isochoric process, Isothermal process, Joule, Joule–Thomson effect, Kelvin, Kinetic theory of gases, Molar mass, Mole (unit), Monatomic gas, ..., Newton's laws of motion, Nitrogen, Noble gas, Number density, Origin (mathematics), Oxygen, Partition function (statistical mechanics), Pascal (unit), Perfect gas, Polytropic process, Potential energy, Pressure, Real gas, Residual property (physics), Rudolf Clausius, Specific volume, State function, Statistical mechanics, Temperature, Thermal energy, Thermodynamic equations, Thermodynamic process, Thermodynamic temperature, Unified atomic mass unit, Van der Waals equation, Volume, Volume (thermodynamics). Expand index (27 more) »
Adiabatic process
In thermodynamics, an adiabatic process is one that occurs without transfer of heat or matter between a thermodynamic system and its surroundings.
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Amount of substance
Amount of substance (symbol for the quantity is 'n') is a standard-defined quantity that measures the size of an ensemble of elementary entities, such as atoms, molecules, electrons, and other particles.
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Annalen der Physik
Annalen der Physik (English: Annals of Physics) is one of the oldest scientific journals on physics and has been published since 1799.
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Argon
Argon is a chemical element with symbol Ar and atomic number 18.
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Atmosphere (unit)
The standard atmosphere (symbol: atm) is a unit of pressure defined as.
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Atomic mass constant
In physics and chemistry, the atomic mass constant, mu, is one twelfth of the mass of an unbound atom of carbon-12 at rest and in its ground state.
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August Krönig
August Karl Krönig (20 September 1822 – 5 June 1879) was a German chemist and physicist who published an account of the kinetic theory of gases in 1856, probably after reading a paper by John James Waterston.
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Avogadro constant
In chemistry and physics, the Avogadro constant (named after scientist Amedeo Avogadro) is the number of constituent particles, usually atoms or molecules, that are contained in the amount of substance given by one mole.
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Avogadro's law
Avogadro's law (sometimes referred to as Avogadro's hypothesis or Avogadro's principle) is an experimental gas law relating the volume of a gas to the amount of substance of gas present.
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Bar (unit)
The bar is a metric unit of pressure, but is not approved as part of the International System of Units (SI).
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Benoît Paul Émile Clapeyron
Benoît Paul Émile Clapeyron (26 February 1799 – 28 January 1864) was a French engineer and physicist, one of the founders of thermodynamics.
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Boltzmann constant
The Boltzmann constant, which is named after Ludwig Boltzmann, is a physical constant relating the average kinetic energy of particles in a gas with the temperature of the gas.
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Boyle's law
Boyle's law (sometimes referred to as the Boyle–Mariotte law, or Mariotte's law) is an experimental gas law that describes how the pressure of a gas tends to increase as the volume of the container decreases.
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Calorie
A calorie is a unit of energy.
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Charles's law
Charles's law (also known as the law of volumes) is an experimental gas law that describes how gases tend to expand when heated.
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Combined gas law
The combined gas law is a gas law that combines Charles's law, Boyle's law, and Gay-Lussac's law.
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Cubic metre
The cubic metre (in British English and international spelling as used by the International Bureau of Weights and Measures) or cubic meter (in American English) is the SI derived unit of volume.
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Density
The density, or more precisely, the volumetric mass density, of a substance is its mass per unit volume.
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Divergence
In vector calculus, divergence is a vector operator that produces a scalar field, giving the quantity of a vector field's source at each point.
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Divergence theorem
In vector calculus, the divergence theorem, also known as Gauss's theorem or Ostrogradsky's theorem, reprinted in is a result that relates the flow (that is, flux) of a vector field through a surface to the behavior of the vector field inside the surface.
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Dynamic pressure
Dynamic pressure (sometimes called velocity pressure) is the increase in a moving fluid's pressure over its static value due to motion.
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Enthalpy
Enthalpy is a property of a thermodynamic system.
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Entropy
In statistical mechanics, entropy is an extensive property of a thermodynamic system.
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Equation of state
In physics and thermodynamics, an equation of state is a thermodynamic equation relating state variables which describe the state of matter under a given set of physical conditions, such as pressure, volume, temperature (PVT), or internal energy.
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Equipartition theorem
In classical statistical mechanics, the equipartition theorem relates the temperature of a system to its average energies.
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First principle
A first principle is a basic, foundational, self-evident proposition or assumption that cannot be deduced from any other proposition or assumption.
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Free expansion
Free expansion is an irreversible process in which a gas expands into an insulated evacuated chamber.
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Gas
Gas is one of the four fundamental states of matter (the others being solid, liquid, and plasma).
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Gas constant
The gas constant is also known as the molar, universal, or ideal gas constant, denoted by the symbol or and is equivalent to the Boltzmann constant, but expressed in units of energy per temperature increment per mole, i.e. the pressure-volume product, rather than energy per temperature increment per particle.
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Gas laws
The gas laws were developed at the end of the 18th century, when scientists began to realize that relationships between pressure, volume and temperature of a sample of gas could be obtained which would hold to approximation for all gases.
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Gay-Lussac's law
Gay-Lussac's law can refer to several discoveries made by French chemist Joseph Louis Gay-Lussac (1778–1850) and other scientists in the late 18th and early 19th centuries pertaining to thermal expansion of gases and the relationship between temperature, volume, and pressure.
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Hamiltonian mechanics
Hamiltonian mechanics is a theory developed as a reformulation of classical mechanics and predicts the same outcomes as non-Hamiltonian classical mechanics.
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Heat capacity ratio
In thermal physics and thermodynamics, the heat capacity ratio or adiabatic index or ratio of specific heats or Poisson constant, is the ratio of the heat capacity at constant pressure to heat capacity at constant volume.
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Helium
Helium (from lit) is a chemical element with symbol He and atomic number 2.
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Helmholtz free energy
In thermodynamics, the Helmholtz free energy is a thermodynamic potential that measures the useful work obtainable from a closed thermodynamic system at a constant temperature and volume.
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Ideal gas
An ideal gas is a theoretical gas composed of many randomly moving point particles whose only interactions are perfectly elastic collisions.
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Internal energy
In thermodynamics, the internal energy of a system is the energy contained within the system, excluding the kinetic energy of motion of the system as a whole and the potential energy of the system as a whole due to external force fields.
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International System of Units
The International System of Units (SI, abbreviated from the French Système international (d'unités)) is the modern form of the metric system, and is the most widely used system of measurement.
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Isenthalpic process
An isenthalpic process or isoenthalpic process is a process that proceeds without any change in enthalpy, H; or specific enthalpy, h.
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Isentropic process
In thermodynamics, an isentropic process is an idealized thermodynamic process that is both adiabatic and reversible.
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Isobaric process
An isobaric process is a thermodynamic process in which the pressure stays constant: ΔP.
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Isochoric process
An isochoric process, also called a constant-volume process, an isovolumetric process, or an isometric process, is a thermodynamic process during which the volume of the closed system undergoing such a process remains constant.
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Isothermal process
An isothermal process is a change of a system, in which the temperature remains constant: ΔT.
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Joule
The joule (symbol: J) is a derived unit of energy in the International System of Units.
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Joule–Thomson effect
In thermodynamics, the Joule–Thomson effect (also known as the Joule–Kelvin effect, Kelvin–Joule effect, or Joule–Thomson expansion) describes the temperature change of a real gas or liquid (as differentiated from an ideal gas) when it is forced through a valve or porous plug while keeping them insulated so that no heat is exchanged with the environment.
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Kelvin
The Kelvin scale is an absolute thermodynamic temperature scale using as its null point absolute zero, the temperature at which all thermal motion ceases in the classical description of thermodynamics.
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Kinetic theory of gases
The kinetic theory describes a gas as a large number of submicroscopic particles (atoms or molecules), all of which are in constant rapid motion that has randomness arising from their many collisions with each other and with the walls of the container.
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Molar mass
In chemistry, the molar mass M is a physical property defined as the mass of a given substance (chemical element or chemical compound) divided by the amount of substance.
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Mole (unit)
The mole, symbol mol, is the SI unit of amount of substance.
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Monatomic gas
In physics and chemistry, monatomic is a combination of the words "mono" and "atomic", and means "single atom".
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Newton's laws of motion
Newton's laws of motion are three physical laws that, together, laid the foundation for classical mechanics.
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Nitrogen
Nitrogen is a chemical element with symbol N and atomic number 7.
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Noble gas
The noble gases (historically also the inert gases) make up a group of chemical elements with similar properties; under standard conditions, they are all odorless, colorless, monatomic gases with very low chemical reactivity.
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Number density
In physics, astronomy, chemistry, biology and geography, number density (symbol: n or ρN) is an intensive quantity used to describe the degree of concentration of countable objects (particles, molecules, phonons, cells, galaxies, etc.) in physical space: three-dimensional volumetric number density, two-dimensional areal number density, or one-dimensional line number density.
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Origin (mathematics)
In mathematics, the origin of a Euclidean space is a special point, usually denoted by the letter O, used as a fixed point of reference for the geometry of the surrounding space.
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Oxygen
Oxygen is a chemical element with symbol O and atomic number 8.
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Partition function (statistical mechanics)
In physics, a partition function describes the statistical properties of a system in thermodynamic equilibrium.
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Pascal (unit)
The pascal (symbol: Pa) is the SI derived unit of pressure used to quantify internal pressure, stress, Young's modulus and ultimate tensile strength.
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Perfect gas
In physics, a perfect gas is a theoretical gas that differs from real gases in a way that makes certain calculations easier to handle.
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Polytropic process
A polytropic process is a thermodynamic process that obeys the relation: where p is the pressure, V is volume, n is the polytropic index, and C is a constant.
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Potential energy
In physics, potential energy is the energy possessed by an object because of its position relative to other objects, stresses within itself, its electric charge, or other factors.
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Pressure
Pressure (symbol: p or P) is the force applied perpendicular to the surface of an object per unit area over which that force is distributed.
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Real gas
Real gases are non-hypothetical gases whose molecules occupy space and have interactions; consequently, they adhere to gas laws.
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Residual property (physics)
In thermodynamics a residual property is defined as the difference between a real gas property and an ideal gas property, both considered at the same pressure, temperature, and composition.
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Rudolf Clausius
Rudolf Julius Emanuel Clausius (2 January 1822 – 24 August 1888) was a German physicist and mathematician and is considered one of the central founders of the science of thermodynamics.
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Specific volume
In thermodynamics, the specific volume of a substance is the ratio of the substance's volume to its mass.
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State function
In thermodynamics, a state function or function of state is a function defined for a system relating several state variables or state quantities that depends only on the current equilibrium state of the system, for example a gas, a liquid, a solid, crystal, or emulsion.
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Statistical mechanics
Statistical mechanics is one of the pillars of modern physics.
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Temperature
Temperature is a physical quantity expressing hot and cold.
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Thermal energy
Thermal energy is a term used loosely as a synonym for more rigorously-defined thermodynamic quantities such as the internal energy of a system; heat or sensible heat, which are defined as types of transfer of energy (as is work); or for the characteristic energy of a degree of freedom in a thermal system kT, where T is temperature and k is the Boltzmann constant.
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Thermodynamic equations
Thermodynamics is expressed by a mathematical framework of thermodynamic equations which relate various thermodynamic quantities and physical properties measured in a laboratory or production process.
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Thermodynamic process
Classical thermodynamics considers three main kinds of thermodynamic process: change in a system, cycles in a system, and flow processes.
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Thermodynamic temperature
Thermodynamic temperature is the absolute measure of temperature and is one of the principal parameters of thermodynamics.
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Unified atomic mass unit
The unified atomic mass unit or dalton (symbol: u, or Da) is a standard unit of mass that quantifies mass on an atomic or molecular scale (atomic mass).
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Van der Waals equation
The van der Waals equation (or van der Waals equation of state; named after Johannes Diderik van der Waals) is based on plausible reasons that real gases do not follow the ideal gas law.
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Volume
Volume is the quantity of three-dimensional space enclosed by a closed surface, for example, the space that a substance (solid, liquid, gas, or plasma) or shape occupies or contains.
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Volume (thermodynamics)
In thermodynamics, the volume of a system is an important extensive parameter for describing its thermodynamic state.
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General gas equation, Ideal Gas Law, Ideal Gas equation, Ideal gas eq, Ideal gas equation, Ideal gas laws, Ideal-gas law, Law of ideal gas, PV = nRT, PV=nRT, Perfect Gas Law, Pervnert, Pv=Nrt, Pv=nrt, The ideal gas law, The law of ideal gas, Universal gas equation, Universal gas law.
References
[1] https://en.wikipedia.org/wiki/Ideal_gas_law