Physical Principles: Difference between revisions

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The atmospheric pressure in Hannover, for example, fluctuates between 964 hPa and 1042 hPa.
The atmospheric pressure in Hannover, for example, fluctuates between 964 hPa and 1042 hPa.


The partial pressure of water vapor at a given temperature cannot exceed certain limits, i.e. saturation. When the saturation pressure p<sub>s</sub> is increased by additional water supply (humidification), the partial pressure stays the same, but the excess water vapor precipitates in the form of liquid water. This is called condensate.  
The partial pressure of water vapor at a given temperature cannot exceed certain limits, i.e., saturation. When the saturation pressure p<sub>s</sub> is increased by additional water supply (humidification), the partial pressure stays the same, but the excess water vapor precipitates in the form of liquid water. This processis called condensation.  
There is no simple physical relation between temperature and saturation pressure, which is why the relationship is expressed in graphical or in table form.
There is no simple physical relation between temperature and saturation pressure, which is why the relationship is expressed in either graphical or table form.


The saturation pressure increases considerably, when temperature rises. For instance, at 0 ºC it is 611 Pa and at 20 ºC already 2338 Pa.
When temperature rises the saturation pressure increases considerably. For instance, at 0 ºC it is 611 Pa and at 20 ºC it reaches 2338 Pa.


== WebLinks ==
== WebLinks ==

Revision as of 14:33, 5 January 2013

Author: Hans-Jürgen Schwarz
English Translation by Sandra Leithäuser
Back to Air humidity measurement

Abstract

Dalton's Law

The total pressure of a gas mixture is composed by the sum of the partial pressures of the constituents.[1]
In simplified terms: the air consists of dry air and water vapor

wherein Pw constitutes the partial pressure generated by water vapor and Pdry represents the sum of all partial pressures of all the other gases.


The total pressure of a mixture of ideal gases is equal to the sum of partial pressures of the individual gases in the mixture.


Water vapor partial pressure in the air

In a gas mixture (volume V, temperature T), each component gas has a partial pressure, pi, which is proportional to the number of molecules present in the mixture.[2].

For the relationship between pi, V and T, the following equation applies:


The total pressure is the sum of all partial pressures. Water vapor partial pressure is at

22 ºC and 100 %rF = 2645 Pa
22 ºC and 67 %rF = 1772 Pa

(1 Pa = 1N/m² = 0.01 mbar)

Figure1:Vapour pressure diagrams of water; data taken from Dortmund Data Bank. Graphics shows triple point, critical point and boiling point of water.

The atmospheric pressure in Hannover, for example, fluctuates between 964 hPa and 1042 hPa.

The partial pressure of water vapor at a given temperature cannot exceed certain limits, i.e., saturation. When the saturation pressure ps is increased by additional water supply (humidification), the partial pressure stays the same, but the excess water vapor precipitates in the form of liquid water. This processis called condensation. There is no simple physical relation between temperature and saturation pressure, which is why the relationship is expressed in either graphical or table form.

When temperature rises the saturation pressure increases considerably. For instance, at 0 ºC it is 611 Pa and at 20 ºC it reaches 2338 Pa.

WebLinks

Literature