Henry's law: Difference between revisions
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(New page: '''Henry's law''', formulated by William Henry, states that ''the amount of a given gas dissolved in a liquid is directly proportional to the partial pressure of that gas in equilibrium w...) |
Carl McBride (talk | contribs) (Added a reference and an internal link.) |
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'''Henry's law''', formulated by William Henry, states that ''the amount of a given gas dissolved in a liquid is directly proportional to the partial pressure of that gas in equilibrium with that liquid.'' | '''Henry's law''', formulated by William Henry in 1803 (Ref. 1), states that ''the amount of a given gas dissolved in a liquid is directly proportional to the partial pressure of that gas in equilibrium with that liquid.'' | ||
Mathematically, | Mathematically, | ||
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where ''k'', the constant of proportionality, is termed Henry's constant. | where ''k'', the constant of proportionality, is termed Henry's constant. | ||
This constant is, of course, dependent on the dimensions employed for the pressure and | This constant is, of course, dependent on the dimensions employed for the [[pressure]] and | ||
the concentration. In chemistry, atm and molarity are typical. A more elegant definition is to | the concentration. In chemistry, atm and molarity are typical. A more elegant definition is to | ||
make it dimensionless making use of the [[Equation_of_State:_Ideal_Gas | ideal gas equation of state]] (if applicable). | make it dimensionless making use of the [[Equation_of_State:_Ideal_Gas | ideal gas equation of state]] (if applicable). | ||
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==External links== | ==External links== | ||
*[http://en.wikipedia.org/wiki/Henry's_law Henry's law at wikipedia] | *[http://en.wikipedia.org/wiki/Henry's_law Henry's law at wikipedia] | ||
==References== | |||
#[http://dx.doi.org/10.1098/rstl.1803.0004 William Henry "Experiments on the Quantity of Gases Absorbed by Water, at Different Temperatures, and under Different Pressures", Philosophical Transactions of the Royal Society of London '''93''' pp. 29- (1803)] | |||
[[Category:Equations of state]] | [[Category:Equations of state]] | ||
Revision as of 12:25, 26 June 2008
Henry's law, formulated by William Henry in 1803 (Ref. 1), states that the amount of a given gas dissolved in a liquid is directly proportional to the partial pressure of that gas in equilibrium with that liquid.
Mathematically,
where k, the constant of proportionality, is termed Henry's constant.
This constant is, of course, dependent on the dimensions employed for the pressure and the concentration. In chemistry, atm and molarity are typical. A more elegant definition is to make it dimensionless making use of the ideal gas equation of state (if applicable).