Phase Interfaces and Surfaces - Physical Chemistry

While water exhibits hydrogen bonding and has metastable phases, these don't have anything to do with the density of water. The slope of the solid/liquid line is in fact negative. This tells something about the relative densities of the phases. For a phase diagram, moving along a line of constant temperature (vertically on a phase diagram tells us something about the densities. Moving up along the line indicates an increase in density (this makes sense, since gasses are the least dense, and occupy the bottom portion of a phase diagram). If you move along a constant temperature line, you will see that water has a higher density than ice, since the ordering goes vapor, ice, then water. This is a result of the packing in solid ice.

Condition I is true. The only place three phases can coexist is at the triple point.

Condition II is false. Water in fact can undergo deposition and move from the solid phase to the gas phase directly. This occurs at pressures below 0.006atm.

Condition III is false. A peculiar fact of the water phase diagram is the slope of the solid/liquid line. For most phase diagrams, the slope is sharply positive, but that of water is negative.

Condition IV is true. No distinct phases exist above the critical point.

While water exhibits hydrogen bonding and has metastable phases, these don't have anything to do with the density of water. The slope of the solid/liquid line is in fact negative. This tells something about the relative densities of the phases. For a phase diagram, moving along a line of constant temperature (vertically on a phase diagram tells us something about the densities. Moving up along the line indicates an increase in density (this makes sense, since gasses are the least dense, and occupy the bottom portion of a phase diagram). If you move along a constant temperature line, you will see that water has a higher density than ice, since the ordering goes vapor, ice, then water. This is a result of the packing in solid ice.

Condition I is true. The only place three phases can coexist is at the triple point.

Condition II is false. Water in fact can undergo deposition and move from the solid phase to the gas phase directly. This occurs at pressures below 0.006atm.

Condition III is false. A peculiar fact of the water phase diagram is the slope of the solid/liquid line. For most phase diagrams, the slope is sharply positive, but that of water is negative.

Condition IV is true. No distinct phases exist above the critical point.

While water exhibits hydrogen bonding and has metastable phases, these don't have anything to do with the density of water. The slope of the solid/liquid line is in fact negative. This tells something about the relative densities of the phases. For a phase diagram, moving along a line of constant temperature (vertically on a phase diagram tells us something about the densities. Moving up along the line indicates an increase in density (this makes sense, since gasses are the least dense, and occupy the bottom portion of a phase diagram). If you move along a constant temperature line, you will see that water has a higher density than ice, since the ordering goes vapor, ice, then water. This is a result of the packing in solid ice.

Condition I is true. The only place three phases can coexist is at the triple point.

Condition II is false. Water in fact can undergo deposition and move from the solid phase to the gas phase directly. This occurs at pressures below 0.006atm.

Condition III is false. A peculiar fact of the water phase diagram is the slope of the solid/liquid line. For most phase diagrams, the slope is sharply positive, but that of water is negative.

Condition IV is true. No distinct phases exist above the critical point.

While water exhibits hydrogen bonding and has metastable phases, these don't have anything to do with the density of water. The slope of the solid/liquid line is in fact negative. This tells something about the relative densities of the phases. For a phase diagram, moving along a line of constant temperature (vertically on a phase diagram tells us something about the densities. Moving up along the line indicates an increase in density (this makes sense, since gasses are the least dense, and occupy the bottom portion of a phase diagram). If you move along a constant temperature line, you will see that water has a higher density than ice, since the ordering goes vapor, ice, then water. This is a result of the packing in solid ice.

Condition I is true. The only place three phases can coexist is at the triple point.

Condition II is false. Water in fact can undergo deposition and move from the solid phase to the gas phase directly. This occurs at pressures below 0.006atm.

Condition III is false. A peculiar fact of the water phase diagram is the slope of the solid/liquid line. For most phase diagrams, the slope is sharply positive, but that of water is negative.

Condition IV is true. No distinct phases exist above the critical point.