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Many other thermodynamic processes will result in a change in volume. A polytropic process , in particular, causes changes to the system so that the quantity p V n {\displaystyle pV^{n}} is constant (where p {\displaystyle p} is pressure, V {\displaystyle V} is volume, and n {\displaystyle n} is the polytropic index, a constant).
Boyle's law is a gas law, stating that the pressure and volume of a gas have an inverse relationship. If volume increases, then pressure decreases and vice versa, when the temperature is held constant. Therefore, when the volume is halved, the pressure is doubled; and if the volume is doubled, the pressure is halved.
In continuum mechanics and thermodynamics, a control volume (CV) is a mathematical abstraction employed in the process of creating mathematical models of physical processes. In an inertial frame of reference , it is a fictitious region of a given volume fixed in space or moving with constant flow velocity through which the continuuum (a ...
Replacing work with a change in volume gives = Since the process is isochoric, dV = 0 , the previous equation now gives d U = d Q {\displaystyle dU=dQ} Using the definition of specific heat capacity at constant volume, c v = ( dQ / dT )/ m , where m is the mass of the gas, we get d Q = m c v d T {\displaystyle dQ=mc_{\mathrm {v} }\,dT}
where V 100 is the volume occupied by a given sample of gas at 100 °C; V 0 is the volume occupied by the same sample of gas at 0 °C; and k is a constant which is the same for all gases at constant pressure. This equation does not contain the temperature and so is not what became known as Charles's Law.
In thermodynamics and fluid mechanics, the compressibility (also known as the coefficient of compressibility [1] or, if the temperature is held constant, the isothermal compressibility [2]) is a measure of the instantaneous relative volume change of a fluid or solid as a response to a pressure (or mean stress) change.
Chemical thermodynamics is the study of the interrelation of energy with chemical reactions or with a physical change of state within the confines of the laws of thermodynamics. The primary objective of chemical thermodynamics is determining the spontaneity of a given transformation.
In thermodynamics, a departure function is defined for any thermodynamic property as the difference between the property as computed for an ideal gas and the property of the species as it exists in the real world, for a specified temperature T and pressure P. Common departure functions include those for enthalpy, entropy, and internal energy.