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'''Vapor pressure''' (also known as ''equilibrium vapor pressure'' or ''saturation vapor pressure''), is the [[pressure]] of a [[vapor]] in [[Thermodynamic equilibrium|equilibrium]] with its [[liquid]] or [[solid]] [[Phase (matter)|phase]]. At any given [[temperature]], for a specific substance, there is a [[pressure]] at which the gas of that specific substance is in dynamic equilibrium with its liquid or solid forms. This is the vapor pressure of the specific substance at that temperature.


The vapor pressure of a substance increases with increasing temperature.
==Volatility of liquids==
{{main|Relative volatility}}
The vapor pressure is an indication of a liquid's evaporation rate.  It relates to the tendency of [[molecule]]s and [[atom]]s to escape from a liquid or a solid. A substance with a high vapor pressure at normal temperatures is often referred to as ''[[volatility (chemistry)|volatile]]''.
''Relative volatility'' is a measure that compares the vapor pressures of the components in a liquid mixture of chemicals. This measure is widely used in designing large industrial [[Continuous distillation|distillation]], [[absorption process|absorption]] and  other separation processes that involve the contacting of vapor and liquid phases in a series of [[equilibrium stage]]s.<ref name=Kister>{{cite book|author=Kister, Henry Z.|title=[[Distillation Design]]|edition=1st Edition|publisher=McGraw-hill|year=1992|id=ISBN 0-07-034909-6}}</ref><ref name=Perry>{{cite book|author=Perry, R.H. and Green, D.W. (Editors)|title=[[Perry's Chemical Engineers' Handbook]]|edition=6th Edition|publisher=McGraw-hill|year=1984|id=ISBN 0-07-049479-7}}</ref><ref name=SeaderHenley>{{cite book|author= Seader, J. D., and Henley, Ernest J.|title=Separation Process Principles|publisher=Wiley| location=New York|year=1998|id=ISBN 0-471-58626-9}}</ref> In effect, it indicates the ease or difficulty of separating the more [[Volatility (chemistry)|volatile]] components from the less volatile components in a liquid mixture.
==Vapor pressures and normal boiling points of liquids ==
{{main|Boiling point}}
[[Image:Vapor Pressure Chart.png|thumb|right|301 px|A typical vapor pressure chart for various liquids]]
The [[atmospheric pressure]] boiling point of a liquid (also known as the [[normal boiling point]]) is the temperature where the vapor pressure equals the ambient atmospheric pressure. With any incremental increase in that temperature, the vapor pressure becomes sufficient to overcome atmospheric pressure and lift the liquid to form bubbles inside the bulk of the substance. Bubble formation deeper in the liquid requires a higher pressure, and therefore higher temperature, because the fluid pressure increases above the atmospheric pressure as the depth increases.
The higher the vapor pressure of a liquid at a given temperature, the lower the normal boiling point (i.e., the boiling point at atmospheric pressure) of the liquid.
The vapor pressure chart to the right has graphs of the vapor pressures versus temperatures for a variety of liquids.<ref name=Perry/> As can be seen in the chart, the liquids with the highest vapor pressures have the lowest normal boiling points.
For example, at any given temperature, [[propane]] has the highest vapor pressure of any of the liquids in the chart. It also has the lowest normal boiling point (–<small> </small>43.7 °C), which is where the vapor pressure curve of propane (the purple line) intersects the horizontal pressure line of one atmosphere ([[Atmosphere (unit)|atm]]) of absolute vapor pressure.
Although the relation between vapor pressure and temperature is non-linear, the chart uses a logarithmic vertical axis in order to obtain slightly curved lines so that one chart can graph many liquids.
==Units of vapor pressure==
The international [[SI]] unit for pressure is the [[pascal (unit)|pascal]] (Pa), equal to one [[newton]] per [[square meter]] (N·m<sup>-2</sup> or kg·m<sup>-1</sup>·s<sup>-2</sup>). The conversions to other pressure units are:
{{pressure}}
==Vapor pressure of solids==
In the case of solids, such as [[crystal]]s, vapor pressure can be defined as the pressure when the rate of [[sublimation (physics)|sublimation]] of a solid matches the rate of deposition of its vapor phase. For most solids this pressure is very low, but some notable exceptions are [[naphthalene]], water ice and [[dry ice]] which is solid [[carbon dioxide]] (CO<sub>2</sub>) and has a vapor pressure of 5.73 MPa (56.5 atm) at 20 degrees Celsius, meaning it will cause most sealed containers to explode).
All solid materials have a vapor pressure. However, due to their often extremely low values, measurement can be rather difficult. Typical techniques include the use of [[thermogravimetry]] and [[gas transpiration]].
==Vapor pressure of liquid mixtures==
{{main|Raoult's law}}
Raoult's law gives an approximation to the vapor pressure of mixtures of liquids.  It states that the vapor pressure of a liquid mixture is equal to the mole-fraction-weighted sum of the vapor pressures of the mixture's pure components:
:<math> P = \sum_i P_i^o\,x_i </math>
{|border="0" cellpadding="2"
|-
|align=right|where:
|-
!align=right|<math>P_i</math>
|align=left|= vapor pressure of a liquid mixture
|-
!align=right|<math>P_i^o</math>
|align=left|= vapor pressure of pure component <math>i</math> in the liquid mixture
|-
!align=right|<math>x_i</math>
|align=left|= [[mole fraction]] of component <math>i</math> in the liquid mixture
|-
!align=right|<math>P_i^o\,x</math>
|align=left|= <math>p_i</math> = the partial pressure of component <math>i</math> in the liquid mixture
|}
Raoult's law is applicable only to ideal liquids and to components that are fairly similar such as [[benzene]] and [[toluene]], [[hexane and heptane]] or [[o-xylene]] and [[p-xylene]].
Systems that have vapor pressures higher than indicated by the above equation are said to have ''positive deviations''.  Such a deviation suggests weaker [[Intermolecular force|intermolecular attraction]] than in the pure components, so that the molecules can be thought of as being "held in" the liquid phase less strongly than in the pure liquid.  An example is the [[azeotrope]] of approximately 95% ethanol and water.  Because the azeotrope's vapor pressure is higher than predicted by Raoult's law, it boils at a temperature below that of either pure component.
There are also systems with ''negative deviations'' that have vapor pressures that are lower than expected.  Such a deviation is evidence for stronger intermolecular attraction between the constituents of the mixture than exists in the pure components.  Thus, the molecules are "held in" the liquid more strongly when a second molecule is present.  An example is a mixture of [[trichloromethane]] (chloroform) and [[2-propanone]] (acetone), which boils above the boiling point of either pure component.
==Relative humidity==
{{main|Relative humidity}}
The ratio, often expressed as a percentage, of the partial pressure of water in the atmosphere at some observed temperature, to the vapor pressure of pure water at this temperature.<ref>[http://www.iupac.org/goldbook/R05267.pdf Relative Humidity] IUPAC Compendium of Chemical Terminology (Electronic version)</ref> It may be expressed as:
:<math>% RH = \Big(\frac{p_\mathrm{water}}{P^o_\mathrm{water}}\Big) 100</math>
{|border="0" cellpadding="2"
|-
|align=right|where:
|-
|align=right|<math>% RH</math>
|align=left|= percent relative humidity of the atmospheric air-water mixture
|-
|align=right|<math>p_\mathrm{water}</math>
|align=left|= partial pressure of water in the atmospheric air-water mixture
|-
|align=right|<math>P^o_\mathrm{water}</math>
|= vapor pressure of pure water at the temperature of the atmospheric air-water mixture
|}
At 100 percent relative humidity, the atmospheric air is said to be ''saturated'' with water. That occurs when the partial pressure of the water in the air, <math>p_\mathrm{water}</math>, is equal to the vapor pressure of pure water at the air temperature, <math>P^o_\mathrm{water}</math>.
Given the [[wet-bulb temperature ]] and the [[dry-bulb temperature]] of the atmosphere, which are readily measured by using a [[sling psychrometer]], the relative humidity can be obtained from a [[Psychrometry|psychrometric chart]].<ref name=Perry/>
==Vapor pressure terminology in meteorology==
{{main|Meteorology}}
The terminology defined and discussed in this article is the terminology used extensively by chemists, chemical engineers and others.
The terminology used by workers in the field of meteorology is unique to that field of science and it defines vapor pressure and similar terms quite a bit differently than is done in this article. For example, the [[American Meteorological Society]] (AMS) uses the following definitions:<ref>[http://www.ametsoc.org/amsedu/wes/glossary.html AMS Glossary of Atmospheric Terms]</ref>
* Vapor pressure: The portion of the total air pressure exerted by the water vapor component of air. (That would be the ''partial pressure'' of the water vapor in the air using the terminology defined in this article.)
* Saturation vapor pressure: The maximum vapor pressure in a sample of air at a specific temperature. (That is not the meaning of "saturation vapor pressure" as defined in this article. In the terminology defined in this article, it can be said that ''air at a specific temperature is saturated'' when the partial pressure of the water in the air is equal to the vapor pressure of pure water at that specific temperature. In other words, when relative humidity is 100%.)
To avoid any confusion, this article makes no attempt to go into any further detail concerning the terminology used in meteorology.
==References==
{{reflist}}
==See also==
* [[Partial pressure]]
* [[Relative volatility]]
* [[Boiling point]]
* [[Relative humidity]]
* [[Psychrometry]]
* [[Meteorology]]
* [[Raoult's law]]

Revision as of 14:57, 2 September 2008

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