## P-T graph of water

refer to
http://chemwiki.ucdavis.edu/Physical...Phase_Diagrams
say: This indicates that the liquid phase is more dense than the solid phase.

From that graph, how do we know the density and water expand when freezing from the graph?

Thank you

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Gold Member
It explains it in the link a bit further down.

 Normally the solid/liquid phase line slopes positively to the right (as in the diagram for carbon dioxide above). However for other substances, notably water, the line slopes to the left as the diagram for water shows. This indicates that the liquid phase is more dense than the solid phase. This phenomenon is caused by the crystal structure of the solid phase. In the solid forms of water and some other substances, the molecules crystalize in a lattice with greater average space between molecules, thus resulting in a solid with a lower density than the liquid. Because of this phenomenon, one is able to melt ice simply by applying pressure and not by adding heat.
 So can I say at higher pressure what is more likely to form will be denser? One thing I don't understand is let's say carbon dioxide, when we apply higher pressure, the freezing curve of CO2 slopes positively to the right , that means higher the pressure ,higher the freezing point, more difficult to form solid. Is this correct? But I always think that we need high pressure so that we can easily change from gas to liquid then to solid.

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