Aero formulas: Difference between revisions

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(Heat equations)
(First law of thermodynamics)
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|-
| H
| H
| [https://en.wikipedia.org/wiki/Enthalpy Enthalpy]: energy of a thermodynamic system.
| [https://en.wikipedia.org/wiki/Enthalpy Enthalpy]: total energy of a thermodynamic system.
| J (Joule)
| J (Joule)
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| Temperature
| Temperature
| K (Kelvin)
| K (Kelvin)
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| U
| [https://en.wikipedia.org/wiki/Internal_energy Internal energy] of a system (see first law of Thermodynamics below)
| J (Joule)
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|-
| V
| V
| Volume
| Volume
| m<sup>3</sup> (cubic meter)
| m<sup>3</sup> (cubic meter)
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| W
| [https://en.wikipedia.org/wiki/Work_(thermodynamics) Work]: mechanical constraints on the system.
| J (Joule)
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| n
| n
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|style="background:white"| {{SERVER}}/images/formulas_mirror/QeqmL.png
|style="background:white"| {{SERVER}}/images/formulas_mirror/QeqmL.png
|Heat at [https://en.wikipedia.org/wiki/Latent_heat#Specific_latent_heat state change] for an ideal gas.
|Heat at [https://en.wikipedia.org/wiki/Latent_heat#Specific_latent_heat state change] for an ideal gas.
|The heat required to change the state of a some matter, L being the latent heat.
|The heat required to change the state of a some matter, L being the latent heat. Delta H equals Q only when pressure is constant (isobaric).
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|style="background:white"| {{SERVER}}/images/formulas_mirror/dUeqdQmindW.png
|[https://en.wikipedia.org/wiki/First_law_of_thermodynamics First law of Thermodynamics]
|Variations of internal energy of a system between two states is the sum of the received heat and work (minus the ''given'' work).
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|style="background:white"| {{SERVER}}/images/formulas_mirror/enthalpy.png
|[https://en.wikipedia.org/wiki/Enthalpy Enthalpy]
|Total amount of energy of a system, defined as the sum of the internal energy U and pressure * volume.
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|style="background:white"| {{SERVER}}/images/formulas_mirror/workExpand.png
|Work of gas expansion.
|Work done by expanding an ideal gas.
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|}

Revision as of 02:21, 29 March 2012

Resources on physics related to aerodynamics

The List of elementary physics formulae on wikipedia is useful.

List of variables

Variable Meaning Unit (SI)
γ (gamma) Surface tension N.m-1 (Newton per meter)
μ (mu) or η (eta) Viscosity Pa·s (Pascal second) or P (Poise, 1 Poise is 0.1 Pa.s)
H Enthalpy: total energy of a thermodynamic system. J (Joule)
heat_vap.png or L Vaporization heat or Latent heat of vaporization: energy required to vaporize a mole of liquid at a given temperature. J.mol-1 (Joule per mole)
Q Amount of Heat J (Joule)
T Temperature K (Kelvin)
U Internal energy of a system (see first law of Thermodynamics below) J (Joule)
V Volume m3 (cubic meter)
W Work: mechanical constraints on the system. J (Joule)
n Quantity of matter mol (mole)
p Pressure Pa (Pascal)

List of constants

Constant Meaning Value Unit (SI)
NA or N Avogadro constant, number of atoms or molecules in a mole. 6.02214129.1023 mol-1
R ideal gas constant 8.3144621 J.K−1.mol−1
kB or k Boltzmann constant, gas constant R divided by Avogadro number. 1.3806488.10-23 J.K-1

List of equations

Equation Name Meaning
pvnrtk.png Ideal gas equation Relation between properties of an ideal gas (state equation). k is kB.
clausius-clapeyron.png Clausius-Clapeyron relation Relation between the pressure, latent heat of vaporization and temperature of a vapour at two temperatures (approximation, at low temperatures).
Qdefinition.png Definition of Heat for an ideal gas. The heat required to change the temperature of a system from an initial temperature T0, to a final temperature, Tf.
QeqmL.png Heat at state change for an ideal gas. The heat required to change the state of a some matter, L being the latent heat. Delta H equals Q only when pressure is constant (isobaric).
dUeqdQmindW.png First law of Thermodynamics Variations of internal energy of a system between two states is the sum of the received heat and work (minus the given work).
enthalpy.png Enthalpy Total amount of energy of a system, defined as the sum of the internal energy U and pressure * volume.
workExpand.png Work of gas expansion. Work done by expanding an ideal gas.