Joule-Kelvin

Joule-Thomson effect, Joule-Kelvin effect... 

We can also write the Joule-Kelvin equation (9a) in the form... 

The Joule-Kelvin experiment has recently (1909) been repeated by J. P. Dalton, who finds, for the plug effect in air ... 

The Joule-Kelvin effect may also be calculated from van der Waals equation. For an expansion from i to r2 at constant temperature, let the change of intrinsic energy be 112 — iii = Amt. 

In an idealized Joule-Thomson experiment (also called the Joule-Kelvin experiment) a gas is confined by pistons in a cylinder that is divided into two parts by, a rigid porous membrane (see Fig. 7.3). The gas, starting at pressure P, and temperature 7, is expanded adiabatically and quasi-statically through the membrane to pressure P2 and temperature T2. The two pressures are kept constant during the experiment. If V1 is the initial volume of the number of moles of gas that pass through the membrane and V2 is the final volume of this quantity of gas, then the work done by the gas... 

B Hess, Joule, Kelvin, and Gibbs all contributed to thermochemistry and have thermodynamic entities named after them. Volta, Faraday, and Galvani (choice D) contributed to electrochemistry, Kekule to organic chemistry, London to chemical bonding, Boyle and Charles to gas laws, Arrhenius to acid/base chemistry and thermochemstry, Pauli to quantum theory, Davy and Ramsay to element isolation, and Mendeleev to the periodic table. 

The differential coefficient pi was first investigated by James Joule and William Thomson in the 1850s [23], before Thomson was elevated to the peerage, to become the first Lord Kelvin. So it is also referred to as the Joule-Kelvin coefficient. 

Several famous scientists have contributed to certain aspects of the second law of thermodynamics, among them are Carnot, Joule, Kelvin, Clausius, Planck, and Boltzmann. Various formulations of the second law have been created. This process still continues. Subsequently we will mainly focus on the formulation of Clausius. 

The unit of entropy is indirectly determined by the stipulation above [Eq. (3.6)] and our definition for T. The unit for energy is called Joule (J), and the temperature unit Kelvin (K), resulting in the entropy unit Joule/Kelvin (J K ). This is exactly the... 

In the treatment of biogas the Joule-Kelvin effect cannot be neglected. A biogas feed contains art equimolar mixture of methane to carbon dioxide. If a pressure of 50 bar is applied at the feed side at 30°C calculate then the recovery S at which the permeate temperature has been decreased below 0°C.(Assume that only carbon dioxide permeates through the membrane and that beat transfer is much faster than mass transfer). The Joule-Kelvin coefficient of carbon dioxide is, = 1.2 K/bar. 

For further cooling of a fluid, a common procedure is to use a continuous throttling process in which the fluid is forced to flow through a porous plug, valve, or other constriction that causes an abrupt drop in pressure. A slow continuous adiabatic throttling of a gas is called the Joule-Thomson experiment, or Joule-Kelvin experiment, after the two scientists who collaborated between 1852 and 1862 to design and analyze this procedure. ... 

The temperatures T and T can be measured directly. When values of T" versus p" are plotted for a series of Joule-Thomson experiments having the same values of T and p and different values of p", the curve drawn through the points is a curve of constant enthalpy. The slope at any point on this curve is equal to the Joule-Thomson coefficient (or Joule-Kelvin coefficient) defined by... 

Joule-Kelvin effect Seejoule-thomson effect. 

The Joule-Thomson effect (or Joule-Kelvin effect or Kelvin-Joule effect) [3-6] describes the temperature increase or decrease of a liquid or a real gas such as natural gas, CO2 or N2 when it expands freely from high pressure to low pressure at a constant enthalpy condition (i.e., adiabatic expansion) where no heat is transferred to or from the fluid and no external mechanical woric is extracted from the fluid. 

We proceed, then, with the establishment of the first and second laws through the contributions of Carnot, Clapeyron, Joule, Kelvin, and Clausius, relying on the excellent book of D.S.L. Cardwell (1971)From Watt to Clausius, the Rise of Thermodynamics in the Early Industrial Age. 

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