Thx a bunch!
Now I wonder how this all works out becuase the stock cap is supposed to vent at 7psi. Based on this data, that cant be much more than 200 deg F.
Am I missing something?
In a closed container the pressure you see is determined by the temperature vs vapor pressure for the mixture you have. As Bill Blue mentioned, if you have the system totally full of fluid, you will get an immediate rise in pressure, due to the expansion of water, that doesn't follow the curves in the chart because water doesn't compress. An "expansion" tank should always have enough room for the water to expand.
The newer systems that are filled to the top use a "recovery" tank to store the water pushed past the cap, and return it to the system when temperature is reduced. No direct relationship to pressure and temperature. The pressure can actually be below 0 as the mixture cools.
From the chart, a 7 PSI vapor pressure occurs at about 190F with a 50/50 anti-freeze mixture. Above that temperature, some vapor/coolant will be expelled past the radiator cap. This vapor escape will also provide some cooling as the hottest molecules are the ones that escape.
Of course, the cap has to seal and be working properly. Otherwise it's just like a pot of water on the stove. The higher the temperature, the faster the mixture evaporates. Over time, I think you would get a higher concentration of ethylene glycol as the water would evaporate faster.
BTW, take all the reading I make from that chart with a grain of salt. My eyes seem to cross every time I look at it.
Bob W.