we all know determining the joule thomson coefficient is determined by performing irreversible adiabatic process, i.e. constant enthalpy process, it may be determined foe any gas .
Since enthalpy remains constant in this process
let h1 be the enthalpy before the irreversible expansion and h2 be the enthalpy after expansion, h1=h2 . for a real gas h enthalpy is a function of pressure and temperature so it may get cooled or get warm according to nature of gas and conditions
but for an ideal gas h=f(T) only since h= u +pv [they both are dependent on absolute temperature] so while going through irreversible expansion the gas does not depend on pressure .
mathematically,
let @ be joule thomson coefficient
$ be parial derivative
@= 1/ cp multiplied by [T multiplied by{$v/$t}at constant pressure -v]
for an ideal gas $v/$T at constant pressure becomes v/T also pv =RT {observe equations are written on per kg basis} so v/T= R/p so we get @=0
the value of joule Thomson coefficient for an ideal gas is 0 (zero)
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two application joule thomson 1. linde methode 2. liquiefied
if all other factors remain constant (pressure and moles) then the temperature goes up proportionately. (assuming the ideal gas law.)
use the T=2a/(bk) equation shown in the first link, plugging in a and b values found in the second link. proofs are shown in the joule-thomson expansion wikipedia page as well as the van der waals equation of state page.
A joule
Joule-Thompson coefficient for methane
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two application joule thomson 1. linde methode 2. liquiefied
It is an experiment in which the Joule-Thomson coefficient is measured. Basically, you are expanding a gas under adiabatic conditions to ensure constant enthalpy and you will notice that there will be a temperature change (most likely cooling).
It is an experiment in which the Joule-Thomson coefficient is measured. Basically, you are expanding a gas under adiabatic conditions to ensure constant enthalpy and you will notice that there will be a temperature change (most likely cooling).
two application joule thomson 1. linde methode 2. liquiefied
its temperature dependent
if all other factors remain constant (pressure and moles) then the temperature goes up proportionately. (assuming the ideal gas law.)
There is for every gas a point called the inversion temperature. Above this temperature, the gas exhibits a reverse Joule-Thompson effect and warms on expansion instead of cooling. The inversion temperatures for hydrogen and helium are quite low compared to those of most other gases.
The one and only macroscopic thermodynamic property that the internal energy of an ideal gas depends on is its temperature.
The temperature drops. When a real (non ideal) gas expands ( in such a way that it does not take in heat from the environment- so called adiabatic) for example when hot air rises into a low pressure region the gas will cools. Real gases when they expand freely cool, this is the basis of the refrigerator (Joule Thomson effect). The explanation is that the separation of gas molecules involves "work" done against intermolecular forces which leads to a reductio in the kinetic of the molecules, hence the observed temperature.
use the T=2a/(bk) equation shown in the first link, plugging in a and b values found in the second link. proofs are shown in the joule-thomson expansion wikipedia page as well as the van der waals equation of state page.