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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>[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. 29-42 (1803)]</ref> | ||
<ref>[http://dx.doi.org/10.1098/rstl.1803.0004 William Henry "Appendix: 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. 274-276 (1803)]</ref>, 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 this can be written as | |||
:<math>p = kc \,</math> | :<math>p = kc \,</math> | ||
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, [[pressure#units |atmospheres]] (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 | form a dimensionless expression by making use of the [[Equation_of_State:_Ideal_Gas | ideal gas equation of state]] (if applicable). | ||
==References== | |||
<references/> | |||
==External links== | ==External links== | ||
*[http://en.wikipedia.org/wiki/Henry's_law Henry's law | *[http://en.wikipedia.org/wiki/Henry's_law Henry's law entry on Wikipedia] | ||
[[Category:Equations of state]] | [[Category:Equations of state]] | ||
Latest revision as of 13:03, 28 September 2009
Henry's law, formulated by William Henry in 1803 [1] [2], 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 this can be written as
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, atmospheres (atm) and molarity are typical. A more elegant definition is to form a dimensionless expression by making use of the ideal gas equation of state (if applicable).
References[edit]
- ↑ 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. 29-42 (1803)
- ↑ William Henry "Appendix: 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. 274-276 (1803)