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Chuck,

I'm going to be away for 3 weeks from tomorrow and desperately  
trying to clear my desk, so I don't have time for a meaningful reply 
(not that it would necessarily be that much help anyway). I'll get 
back to you, but hopefully someone else on the list will be able to 
help you out in the meantime.

Regards

Wilson


> Wilson,
>     
>    Thanks for the input on this;  I see your point.
> 
>    I am packing furiously for a trip to the Keys tonight and do not have time
> 
> for a suitable response but I would like to pose a couple of instant
> questions 
> before I go and perhaps take this up again when I return, if you don't mind.
>   
> I hope none of these are stupid - I haven't had much time to ponder them. 
> 
> *  Are gases in solution compressable ?   If so, is the rate of compression 
> limited by the rate of diffusion of additional molecules of gas into the 
> intermolecular spaces ?
> 
> *  Does a liquid act as a non-compressable container who's intermolecular 
> spaces are open to the ambient environment and filled with gas molecules 
> as pressure forces them into this space ? 
> 
> *  Is the rate of diffusion variable with the effective size of these
> "openings" 
> at the interface of the liquid and the ambient environment and by the volume 
> and "shape" of intermolecular space available in the liquid ?   I realize
> that the 
> liquid is a dynamic environment and there are no actual stationary openings. 
> 
> *   It appears that gases can only enter solution at the surface of a liquid
> but 
> can exit from any point within the fluid as evidenced by bubbles forming in
> the 
> middle of a carbonated liquid when pressure is released.   Does this mean 
> that gasses are able to exit solution much faster that they can enter by
> virtue 
> of a greater number of suitable exit points once super saturation leads to
> free 
> phase gas formation ?
> 
> *  Is it true that though diatomic molecules attached to hemoglobin exert no 
> partial pressure, during the time that they are in transit from the interior
> of 
> the erythrocyte through the plasma and intercellular fluids to the somatic
> cell 
> they do contribute to the partial pressure of that gas so that the local
> partail 
> pressure may vary as this process proceeds at different rates ?
> 
> *  Is the reason a warm liquid will not hold as much dissolved gas as a cool 
> one because the heat energy of the liquid molecules tends to push gas 
> molecules out of the intermolecular spaces of the liquid  or because the 
> transfer of energy to the gas molecules effectively raises the partial
> pressure 
> of the dissolved gases ?  Both ?   Neither ?
> 
> *  Do mechanical forces on a liquid (incompressable container) generate 
> heat energy that can be transmitted to the dissolved gases ?   If not, then 
> I must assume that such forces have no effect on dissolved gases and 
> that the only avenue to physically affecting these dissolved molecules is by
> squeezing more gas molecules into the intermolecular spaces. 
> 
> Thanks for any light you can shed on these.  See you in a few days,
> 
> Chuck
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> 
> 
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