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...''U'' ([[internal energy]]), ''A'' ([[Helmholtz free energy]]), ''H'' ([[enthalpy]]), and ''G'' ([[Gibbs free energy]]). The thermodynamic parameters are: ''

...team of a turbine at a pressure below atmospheric pressure, increases that enthalpy difference and therefore increases the work output of turbine. The water-co

...H''_v is the molar [[heat of vaporization]] (also known as molar enthalpy of evaporation). Further, ''V''^&thinsp;I is the [[molar volume]] ...s larger than the molar volume ''V''^II of the liquid, while the enthalpy of melting ''Q''_melt = ''S''^II&minus;''S''<sup>III</s

...Joule-Thomson effect is an ''[[isenthalpic process]]'', meaning that the [[enthalpy]] of the fluid is constant (i.e., does not change) during the process. ...'''''&nbsp;) with a decrease of pressure ('''''P'''''&nbsp;) at constant [[enthalpy]] ('''''H'''''&nbsp;) in a Joule-Thomson process is the '''Joule-Thomson co

...Joule-Thomson effect is an ''[[isenthalpic process]]'', meaning that the [[enthalpy]] of the fluid is constant (i.e., does not change) during the process. ...'''''&nbsp;) with a decrease of pressure ('''''P'''''&nbsp;) at constant [[enthalpy]] ('''''H'''''&nbsp;) in a Joule-Thomson process is the '''Joule-Thomson co

...o be said that the specific heat ratio of an ideal gas is the ratio of the enthalpy to the internal energy:<ref name=Turns/>

...o be said that the specific heat ratio of an ideal gas is the ratio of the enthalpy to the internal energy:<ref name=Turns/>

{{Image|Steam Temperature-Enthalpy Diagram.png|right|310px}} ...ion|enthalpy of vaporization]] &nbsp; '''H_V''' = vapor specific enthalpy<br/>

|align=left|= source liquid [[enthalpy]] at source temperature and pressure, J/kg<br> |align=left|= flashed vapor enthalpy at atmospheric boiling point and pressure, J/kg

|align=left|= source liquid [[enthalpy]] at source temperature and pressure, J/kg<br> |align=left|= flashed vapor enthalpy at atmospheric boiling point and pressure, J/kg

===Relation to Gibbs free energy and enthalpy=== :H = [[enthalpy]]

#An isenthalpic process occurs at a constant [[enthalpy]]. |[[Enthalpy]]

...or all practical purposes is infinite) and "heat content" (a synonym for [[enthalpy]]) are commonly used and are incorrect by the same reasoning.

...higher the temperature of a system, the higher its [[internal energy]] and enthalpy are.

:<math> \Delta_{solv}H \,</math> is the [[enthalpy of solution]]

{{cite web |title= Chemistry tutorial 9.03: Entropy, enthalpy and spontaneous reactions |url=http://www.youtube.com/watch?v=m1nKEz2DPC0 |

...eter]]. It may also be calculated as the difference between the [[Standard enthalpy change of formation|heat of formation]] (Δ_fH⁰) of th

|align=left|is the [[enthalpy of solution]]

...heat of vaporization''' (<math>LH_v</math> or <math>L_v</math>) and the '''enthalpy of vaporization''' (<math>\Delta H_v</math> or <math>\Delta H_{vap}</math>

* [[Enthalpy of vaporization|Enthalpies of vaporization]] of organic compounds.

...h;pressure ''p''. The reaction heat ''Q'' is then equal to the change in [[enthalpy]] &Delta;''H'' of the reactants. Indeed, according to the first law of ther ...sub> < 0. Correspondingly, an endothermic reaction has a positive reaction enthalpy.

...extrapolated liquid vapor pressures (of the supercooled liquid), if the [[Enthalpy of fusion|heat of fusion]] is known, by using this particular form of the [

...nomial, which yields a complicated expression. Therefore, expressing the [[enthalpy]] and the [[Gibbs energy]] as functions of their natural variables will be

...bar (6.2 to 2.1 MPa) , which is an [[enthalpic]] process (i.e., a constant enthalpy process) that results in lowering the temperature of the stream from about

...rmodynamics)|characteristic function]]s, but expressing, for instance, the enthalpy ''H'' &equiv; ''A'' + ''TS'' + ''pV'' as function of its natural variables

*[[Enthalpy]] (''H'').

...c flash evaporation process is [[isenthalpic]] (i.e., occurs at constant [[enthalpy]]).

...hat is either produced or needed by the reaction is found from the total [[Enthalpy]] change. Other concerns include whether [[side reaction]]s occur from the

where the [[enthalpy of reaction]] &Delta;''H'' is &minus;571.6 kJ<ref>E. A. Guggenheim, ''Therm

...[http://lenr-canr.org/acrobat/MilesMcorrelatioa.pdf Correlation of excess enthalpy and helium-4 production]: A Review, in Tenth International Conference on Co