Seeking help with the problem of saturated vapor pressure
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I need a simple explanation from an expert, as well as a systematic explanation, and the applications of saturated vapor pressure
This post was last edited by ylb913 on 2016-9-15 09:30. For example, when water boils at 100 degrees, the corresponding pressure is 1 atmosphere (absolute pressure), which is also the saturated vapor pressure of water at 100 degrees. We often say that it’s impossible to cook rice at high altitudes, and this is because the air pressure there is too low; the temperature at which water boils is far below 100 degrees. For example, at an altitude of 5,000 meters, the boiling point of water is approximately 83 degrees.
I heard that saturated vapor pressure can be understood as the rate at which water evaporates being equal to the rate at which steam condenses back into water, right?
Does it mean the balance between steam and water under a certain pressure? The relationship between boiling point and pressure is still clear.
This post was last edited by ylb913 on 2016-9-16 09:05. That is, at a certain temperature, the vapor pressure of a particular medium remains constant. For a pure substance, at a certain temperature, the pressure of its vapor is equal to the saturated vapor pressure of that liquid. For a mixture, the pressure in the gas phase is the sum of the saturated vapor partial pressures of each component (where these saturated vapor partial pressures are related to the mole percent composition of each component in the liquid phase).
Thank you! It’s been very helpful to me:handshake