Enthalpy: Difference between revisions
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'''Enthalpy''' (<math>H</math>) <ref>[http://www.dwc.knaw.nl/DL/publications/PU00013601.pdf J. P. Dalton "Researches on the Joule-Kelvin effect, especially at low temperatures. I. Calculations for hydrogen", KNAW Proceedings '''11''' pp. 863-873 (1909)]</ref><ref>[http://dx.doi.org/10.1021/ed079p697 Irmgard K. Howard "H Is for Enthalpy, Thanks to Heike Kamerlingh Onnes and Alfred W. Porter", Journal of Chemical Education '''79''' pp. 697-698 (2002)]</ref> is defined as: | |||
:<math>\left.H\right.=U+pV</math> | :<math>\left.H\right.=U+pV</math> | ||
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:<math>dH=\left(\frac{\partial H}{\partial S}\right)_p dS + \left(\frac{\partial H}{\partial p}\right)_S dp</math> | :<math>dH=\left(\frac{\partial H}{\partial S}\right)_p dS + \left(\frac{\partial H}{\partial p}\right)_S dp</math> | ||
==References== | |||
<references/> | |||
[[Category: Classical thermodynamics]] | [[Category: Classical thermodynamics]] | ||
Revision as of 15:54, 12 March 2012
Enthalpy () [1][2] is defined as:
where is the internal energy, is the pressure, is the volume and (-pV) is a conjugate pair. The differential of this function is
From the Second law of thermodynamics one obtains
thus we arrive at
For H(S,p) we have the following total differential
References
- ↑ J. P. Dalton "Researches on the Joule-Kelvin effect, especially at low temperatures. I. Calculations for hydrogen", KNAW Proceedings 11 pp. 863-873 (1909)
- ↑ Irmgard K. Howard "H Is for Enthalpy, Thanks to Heike Kamerlingh Onnes and Alfred W. Porter", Journal of Chemical Education 79 pp. 697-698 (2002)