
#1
Nov1905, 10:49 PM

P: 1,239

I know that the relationship between pressure and temperature for an ideal gas is linear. The relationship between vapor pressure and temperature for a liquid, however, is exponential. To make it linear we take the natural log and end up with: [tex] \ln P = \frac{\Delta H_{vap}}{RT} + b [/tex]. How did we get [tex] \frac{\Delta H_{vap}}{RT}[/tex] to be the slope? The yaxis is [tex] \ln P [/tex] and the xaxis is [tex] \frac{1000}{T} [/tex].
Thanks 



#2
Nov2005, 07:01 AM

P: 1,239

anybody have any ideas?
thanks 



#3
Nov2005, 10:02 AM

P: 603

I'm not sure what your question really is but if you plot lnP vs 1000/T the slope will be
[tex] \frac{\Delta H_{vap}}{1000 R} [/tex] 



#4
Nov2005, 01:51 PM

Sci Advisor
P: 988

ClausiusClapeyron equationWhich variable are you trying to solve or prove something for? 



#5
Nov2005, 01:58 PM

P: 1,239

The slope was actually [tex]\frac{\Delta H_{vap}}{R} [/tex]. I think it was meant to be written as: [tex] \ln P = \frac{\Delta H_{vap}}{R}\frac{1}{T} + b [/tex]
Is this correct? Thanks 


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