The discussion revolves around the question of whether water can be compressed to the point of freezing under extreme pressure. Participants explore the implications of pressure on the state of water, including temperature changes and phase transitions, while considering the complexities of water's behavior under such conditions.
Participants express multiple competing views regarding the effects of pressure on water's state and the conditions under which it may freeze. The discussion remains unresolved, with no consensus on the implications of pressure and temperature interactions for water.
Participants highlight the limitations of using the ideal gas law for liquids and the need for more complex equations of state when discussing water under extreme conditions. The discussion also reflects varying interpretations of phase diagrams and their implications for water's behavior under pressure.
ChmDudeCB said:Exactly. What we call "frozen water" isn't the only solid form of water, it's just the crystal structure that happens to form at atmospheric pressure. If you compress anything below its supercritical temperature it will eventually become solid (or a glass).
However, are you sure your phase diagram is accurate? IIRC once you pass the supercritical points of temperature and pressure, that is all that exists. I could be wrong and/or my P-chem professor left something out.
DaveC426913 said:Freezing the water requires that the molecules have a chance to crystalize. Crystalizing requires that the molecules have enough elbow room to do so. It's not that water wil NOT freeze under extrreme pressure, it's just that water is very complex. There are actually almost a dozen forms of ice water. Ice I (naturally-formed water-ice) is only one.