CZ:Featured article/Current: Difference between revisions

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== '''[[Subjective-objective dichotomy]]''' ==
== '''[[Partial pressure]]''' ==
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The '''subjective–objective dichotomy''', a longstanding [[Philosophy|philosophical]] topic, is concerned with the analysis of human experience, and of what within experience is "subjective" and what is "objective." The dichotomy arises from the premise that the world consists of ''objects'' (entities) which are [[perception|perceived]] or otherwise presumed to exist as entities, by ''subjects'' (observers). This division of experience results in questions regarding how subjects relate to objects. An important sub-topic is the question of how our own mind relates to other minds, and how to treat the "radical difference that holds between our access to our own experience and our access to the experience of all other human beings", known as the epistemological ''problem of other minds''.<ref name=Hyslop/>
[[Dalton's law]] states that each gas in a mixture of [[ideal gas]]es has a '''partial pressure''' which is the pressure that the gas would have if it alone occupied the same [[volume]] at the same [[temperature]]. The total [[pressure]] of a gas mixture is the sum of the partial pressures of each individual gas in the mixture.  


The subjective–objective dichotomy can be discussed from two standpoints. First is the question of "what" is known. The field of [[ontology]] deals with questions concerning what entities exist or can be said to exist, and how such entities can be grouped, related within a hierarchy, and subdivided according to similarities and differences. The second standpoint is that of "how" does one know what one knows. The field of [[epistemology]] questions what knowledge is, how it is acquired, and to what extent it is possible for a given entity to be known. It includes both subjects and objects.  
[[Henry's law]] states that at a constant temperature, the '''partial pressure''' of a gas in [[Chemical equilibrium|equilibrium]] with a liquid solution containing some of the gas is directly proportional to the concentration of that gas in the liquid solution.  


''[[Subjective-objective dichotomy|.... (read more)]]''
''[[Partial pressure|.... (read more)]]''


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Revision as of 00:31, 21 November 2013

Partial pressure

Dalton's law states that each gas in a mixture of ideal gases has a partial pressure which is the pressure that the gas would have if it alone occupied the same volume at the same temperature. The total pressure of a gas mixture is the sum of the partial pressures of each individual gas in the mixture.

Henry's law states that at a constant temperature, the partial pressure of a gas in equilibrium with a liquid solution containing some of the gas is directly proportional to the concentration of that gas in the liquid solution.

.... (read more)

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