At Pressures Below Its Triple Point Water Would Sublime
If the vapor pressure of the ice is higher than the partial pressure of water in the atmosphere the water vapor will enter the atmosphere, and more ice will sublime to try and keep equilibrium.
At pressures below its triple point water would sublime. At pressures below the triple point (as in outer space), solid ice when heated at constant pressure is converted directly into water vapor in a process known as sublimation. Why is the Triple Point of Water Important. At pressures below this value solid and vapour will remain in equilibrium at temperatures indicated by the line along DE.
Because ice is less dense than liquid water, ice frozen at pressures below the triple point will sublime directly into water vapor. But at temperatures below that of the triple point, a decrease in pressure will result in a phase transition directly from the solid to the gaseous. Above the triple point, solid ice when heated at constant pressure first melts to form liquid water, and then evaporates or boils to form vapor at a higher temperature.
For example, if you were to freeze water into ice and cool it further and then reduce the pressure, you could get ice to sublime. Therefore, the solid sublimes if heated at any pressure below 5.1 atmospheric pressure. Water as a liquid does not sublime (go from solid to gas), but water ice does.
Snow and ice sublime, although more slowly, at temperatures below. It is also important to note that the triple point of water correlates with the pressure necessary for liquid water to exist. Any solid may be sublimed if its temperature and pressure are below its triple point.
The triple point temperature is – 57 0 C at 5.1 atmospheric pressure where liquid, solid and gaseous CO 2 co-exist. This agreement also sets the size of the kelvin as 1/273.16 of the difference between the triple-point temperature of water and absolute zero. This will occur at temperatures below 0°C, or between the boiling point (100°C) and the critical temperature (373.
It is also important to note that the triple point of water correlates with the pressure necessary for liquid water to exist. Because ice is less dense than liquid water, ice frozen at pressures below the triple point will sublime directly into water vapor. At pressures below the triple point (as in outer space), solid ice when heated at constant pressure is converted directly into water vapor in a process known as sublimation.
For most substances the gas–liquid–solid triple point is also the minimum temperature at which the liquid can exist. In general, sublimation is a phase change of a substance directly from the solid to the gas phase without passing through the intermediate liquid phase. Solid carbon dioxide sublimes everywhere along the line below the triple point (e.g., at the temperature of −78.5 °C (194.65 K, −109.30 °F) at atmospheric pressure, whereas its melting into liquid CO 2 can occur only along the line at pressures and temperatures above the triple point (i.e., 5.2 atm, −56.4 °C).
Also, at pressures below the triple point pressure, an increase in temperature will result in a solid being converted to gas without passing through the liquid region.
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