Originally Posted by alpinestarhero (Post 1136935)

Makes sense to me, but i think of it in a thermodynamic sense: dG = -RTlnK etc etc..

Basicly, if you have lotsa pressure, theres theres less room for gas (theres a bunch of fun equations that allow you to calculate the volume of gas - the ideal gas law and a slightly more complicated amended gas law for higher presures). So water in a confined vessel (SV cooling system) will probably boil at 120 degrees C or soemthing. And ontop of a mountain, yea, water will boil at less than 100 degrees C (soemthing like 70 in some cases! lukewarm tea anyone?).

Just as an experiment that we can all do; boil a pan of water. Keep the lid on while its boiling - notice how after a while thres not alot of steam (equilibriated!). Then take off the lid and move away - all the steam comes out as there is more room. I've done this while boiling potatoes and got a scalded hand (heres more fun! When the steam condenses on your hand, turning from a gas to a liquid, it releases energy - bonds made. This is why steam scalds!)

BTW, good to have another chemist on board. What year are you in?

Matt