Thermo problem for a pressure vessel

My question has to do with heating water to a superheated state inside a constant volume vessel.

Given: A pressure vessel with a total volume of 36.77ft^3, is filled with 5 gal of water and heated from room temp. to a final temp. of 1100°F. Obvisouly the initial pressure is atmospheric and the initial temp. is room, or lets say 80°F.

Find: Final pressure of vessel.

In the end I will vary the amount of water in the vessel to obtain a curve relating the volume of water to the final pressure but we can assume 5 gal for the beggining. I have worked on this for some time and am sure that it is much simpler than I am making it out to be. I am aware that the Ideal Gas Law may not be applied since the gas will be water vapor at a high pressure. Hopefully one of you can enlighten me.

Thanks

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 I note that the container is not, in fact, filled with water, as 5 US gallons occupy only 0.664 ft2. Your first step is to look up the saturated vapour pressure, psat, of water at 1100°F. You should now use the ideal gas equation to calculate the number of moles of steam there would be in the container, at a (partial) pressure of psat. Make sure it's less than the number of moles in 5 gallons of water. If it is less, than the water, won't have run out, and to find the pressure in the container you simply add Psat (the partial pressure of the steam) to the partial pressure, pair, of the air at 1100 °F, which will be approximately $$p_{air} = \frac{1100 + 460}{80 + 460} \times p_{atmos}.$$ If the number of moles of steam in the container at 1100 °F and psat is greater than the number of moles in 5 gallons of water then the water will run out (all evaporated) at some temperature lower than 1100 °F and you will need to modify your calculation. If you can't figure out how to do this, ask again! Good luck!
 My saturated steam tables only go up to 705.1°F which I assume is the critical temperature. How would I find the Psat for 1100°F? Also, if I am well above the critical temperature is it not safe to assume that all the water is now evaporated?

Thermo problem for a pressure vessel

rkendrick. You are quite right. I'd simply find how many moles of water vapour there are in 5 gallons of water, and treat the water vapour as an ideal gas, in order to calculate the partial pressure at 1100 °F. Of course the ideal gas bit is an approximation, but to do anything else would be rather complicated. Incidentally, 1100 °F is too low a temperature for appreciable thermal dissociation of water molecules.