At Pressures Below Its Triple Point Water Would Sublime

Why is the Triple Point of Water Important.

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At pressures below its triple point water would sublime. 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. Snow and ice sublime, although more slowly, at temperatures below. 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).

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. It is also important to note that the triple point of water correlates with the pressure necessary for liquid water to exist. The triple point temperature is – 57 0 C at 5.1 atmospheric pressure where liquid, solid and gaseous CO 2 co-exist.

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. Because ice is less dense than liquid water, ice frozen at pressures below the triple point will sublime directly into water vapor. 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. 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. 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.

Therefore, the solid sublimes if heated at any pressure below 5.1 atmospheric pressure. At pressures below this value solid and vapour will remain in equilibrium at temperatures indicated by the line along DE. 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.

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. 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. 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.

Water as a liquid does not sublime (go from solid to gas), but water ice does.

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