Experimental Virial Equation for real gases

  • #1
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}
Screenshot_2018-09-08-06-42-30-043_com.adobe.reader.jpeg
 

Attachments

  • Screenshot_2018-09-08-06-42-30-043_com.adobe.reader.jpeg
    Screenshot_2018-09-08-06-42-30-043_com.adobe.reader.jpeg
    39.4 KB · Views: 357

Answers and Replies

  • #2
BvU
Science Advisor
Homework Helper
14,269
3,631
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 ?
 

Related Threads on Experimental Virial Equation for real gases

Replies
0
Views
2K
Replies
1
Views
984
Replies
1
Views
1K
  • Last Post
Replies
8
Views
4K
  • Last Post
Replies
5
Views
3K
  • Last Post
Replies
5
Views
1K
Replies
1
Views
959
  • Last Post
Replies
3
Views
6K
  • Last Post
Replies
1
Views
6K
Replies
3
Views
3K
Top