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) | ||
|- | |||
| U | |||
| [https://en.wikipedia.org/wiki/Internal_energy Internal energy] of a system (see first law of Thermodynamics below) | |||
| J (Joule) | |||
|- | |- | ||
| V | | V | ||
| Volume | | Volume | ||
| m<sup>3</sup> (cubic meter) | | m<sup>3</sup> (cubic meter) | ||
|- | |||
| W | |||
| [https://en.wikipedia.org/wiki/Work_(thermodynamics) Work]: mechanical constraints on the system. | |||
| J (Joule) | |||
|- | |- | ||
| 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). | |||
|- | |||
|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. | |||
|- | |- | ||
|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
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) |
 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 |
|---|---|---|
|
Ideal gas equation | Relation between properties of an ideal gas (state equation). k is kB. |
|
Clausius-Clapeyron relation | Relation between the pressure, latent heat of vaporization and temperature of a vapour at two temperatures (approximation, at low temperatures). |
|
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. |
|
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). |
|
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 | Total amount of energy of a system, defined as the sum of the internal energy U and pressure * volume. |
|
Work of gas expansion. | Work done by expanding an ideal gas. |
