Experimental Virial Equation for real gases

In summary, the experimental virial equation for real gases, Pv = A(1+BP), shows that at low pressures, gases behave more ideally and follow Boyle's law. However, as pressure increases, there are deviations and the virial expansion can be used to introduce a correction. This information can be found in the source "Chemical engineering thermodynamics" by Smith & van Ness. The accompanying figures likely represent data or illustrations related to the virial equation and its applications.
  • #1
tanaygupta2000
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In the experimental virial equation for real gases,
Pv = A(1+BP) (for small values of P)
as 'P' approaches zero, then why do we get some finite value of 'Pv' instead of approaching to zero value, since 'Pv' is directly proportional to 'P' ?

{P = Pressure of gas, v = Molar volume of gas, A,B = Virial Constants}
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  • #2
At low pressure, gases behave more and more ideally. Boyle's law has ##PV = ## constant. A non-zero constant ! ##PV = n RT## in the ideal gas law .
At higher pressures you get deviations and the virial expansion is one way to introduce a correction.

Read up in e.g. Smith & van Ness: Chemical engineering thermodynamics

PS has your source some caption with the three figures ? What do they represent ?
 

1. What is the Experimental Virial Equation for real gases?

The Experimental Virial Equation is a mathematical relationship that describes the behavior of real gases at various temperatures and pressures. It takes into account the attractive and repulsive forces between gas molecules, which are not accounted for in the ideal gas law.

2. How does the Experimental Virial Equation differ from the Ideal Gas Law?

The ideal gas law assumes that gas molecules have no volume and do not interact with each other. However, the Experimental Virial Equation takes into account the volume and intermolecular forces of real gas molecules, making it a more accurate representation of gas behavior.

3. What are the limitations of the Experimental Virial Equation?

The Experimental Virial Equation only applies to gases at relatively low pressures and high temperatures, where the effects of intermolecular forces are significant. It also cannot accurately describe the behavior of gases that undergo phase changes.

4. How is the Experimental Virial Equation derived?

The Experimental Virial Equation is derived from the statistical mechanics of gas molecules and their interactions, as well as experimental data on the behavior of real gases. It is a complex equation that involves several constants and variables.

5. What are the practical applications of the Experimental Virial Equation?

The Experimental Virial Equation is used in many industrial and scientific applications, such as in the design and operation of gas pipelines and processing plants. It is also used in the study of the behavior of gases in various environments, such as in space or deep-sea diving. Additionally, it is a critical tool in the development of new technologies, such as fuel cells and refrigeration systems.

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