Primary Word |
Secondary Word |
Definition |
Tutorial Page Link |

efficiency | 6A7 | ||

efficiency | Carnot | 6E1 , 3 - 22 | |

efficiency | isothermal | 8C15 , 16 | |

efficiency | second law | 8D6 | |

efficiency | thermal | 6B4 | |

effluent | 5B4 | ||

electrical work | 4C5 | ||

emissivity | The ratio of the radiation emitted by a real surface to the radiation emitted by a blackbody. It is a measure of how effectively the surface radiates. | 4B22 | |

energy | The capacity to do work. | 3C1 | |

energy | conservation of | First law of Thermodynamics. In the absence of nuclear reactions, energy cannot be created or destroyed. Energy can only change form or be transferred. | 1A3 |

energy | internal | The sum of all of the energies associated with moleules of a piece of matter. This includes the energies associated with the molecular structure and all of the microscopic forms of energy of a group of molecules: vibrational, translational and rotational energies. | 3A2 - 3 |

energy | kinetic | The energy associated with any piece of matter that is attributed to the macroscopic or average velocity of the molecules that make up the piece of matter. | 4C7 |

energy | potential | The energy of a piece of matter associated with the position of the matter within a potential field. The field is usually gravitational. | 4C7 |

energy | rotational | The energy associated with the atoms of a polyatomic molecule rotating about an axis. | 2A4 |

energy | total | 4C1 , 5 | |

energy | translational | The energy associated with a molecule of gas traveling through space with a linear velocity, thus possessing kinetic energy. | 2A4 |

energy | vibrational | The energy associated with the atoms of a polyatomic molecule vibrating about their common center of mass. This refers to the stretching, flexing and deformation the molecule and its bonds. | 2A4 |

energy balance | 5B1 - 6 , 9 - 11 | ||

energy balance | differential | 5B2 | |

enthalpy | From the Greek word enthalpien, which means to heat: H = U + PV | 3A5 | |

enthalpy | definition | 3A5 | |

enthalpy | ideal gas | 3A7 | |

enthalpy | incompressible liquids | 3A8 | |

enthalpy | of Fusion | Also known as the Heat of Fusion, Latent Heat of Fusion and Latent Enthalpy of Fusion. Enthalpy of Fusion is the amount of energy released when a substance makes the transition from the liquid phase to the solid phase. Values of the Enthalpy of Fusion are typically tabulated at the normal melting point (temperature). [kJ/kmol] | 3E13 |

enthalpy | of Sublimation | Also known as the Heat of Sublimation, the Latent Heat of Sublimation and the Latent Enthalpy of Sublimation. Enthalpy of Sublimation is the amount of energy required when a substance makes the transition directly from the solid phase to the vapor phase. The Enthalpy of Sublimation is a function of temperature. [kJ/kmol] | 3E13 |

enthalpy | of Vaporization | Also known as the Heat of Vaporization, the Latent Heat of Vaporization and the Latent Enthalpy of Vaporization. Represents the amount of energy required to vaporize a unit mass of saturated liquid at a given temperature or pressure. [kJ/kmol] | 3E2 |

enthalpy | real substance | 3A6 | |

enthalpy | solids | 3A8 | |

enthalpy | specific | 5B10 | |

entropy | 7A1 | ||

entropy | how to evaluate | 7B3 | |

entropy | integral form of the definition | 7D1 - 3 | |

entropy | units | 7B3 | |

entropy balance | 8A1 , 4 | ||

entropy balance | closed system | 8A4 | |

entropy balance | differential form | 8A4 | |

entropy balance | integral form | 8A4 | |

entropy balance | open system | 8B1 , 2 , 4 - 11 | |

entropy balance | rate form | 8A4 | |

entropy balance | single inlet, single outlet | 8B5 | |

entropy balance | steady-state | 8B4 , 5 | |

entropy change | closed system | 8A3 | |

entropy change | ideal gas | 7D8 - 14 | |

entropy change | incompressible liquids | 7D6 , 7 | |

entropy change | internally reversible, isothermal | 7B4 | |

entropy change | irreversible process | 7B5 | |

entropy change | negative | 7C7 | |

entropy change | non-isothermal process | 7D2 | |

entropy change | reversible process | 7B5 | |

entropy change | solids | 7D6 , 7 | |

entropy change | thermal reservoir | 7B4 | |

entropy change | universe | 7C6 , 7 | |

entropy generation | 7C1 , 7 | ||

entropy generation | external | 8D4 | |

entropy generation | inexact differential | 7C3 | |

entropy generation | internal | 8D4 | |

entropy generation | irreversibility | 7C3 | |

entropy generation | irreversible process | 7C3 | |

entropy generation | path variable | 7C3 | |

entropy generation | reversible process | 7C3 | |

entropy generation | total | 8D4 , 5 | |

entropy inequality | 7C2 | ||

equation of state (EOS) | An EOS is an equation that relates pressure, volume and temperature. Given any 2 of the 3 variables (P, V, T) an equation of state can be used to determine the unknown third variable. | 2E1 | |

equation of state (EOS) | generalized compressibility factor | A graphical EOS based on the principle of corresponding states. The Generalized Compressibility Factor EOS manifests itself in the Generalized Compressibility Charts. The key parameter in the Generalized Compressibility Factor EOS is the Compressibility Factor, Z. | 2E7 |

equation of state (EOS) | ideal gas | The simplest EOS : PV=nRT. It is accurate to within 1% when the molar volume of a gas exceeds 20 L/mole. It can be used accurately for diatomic gases and most noble gases as long as the molar volume exceeds 5 L/mole | 4A18 |

equation of state (EOS) | Redich-Kwong | A cubic, empirical EOS that accurately represents the behavior of a wide variety of systems. Its two parameters are empirical functions of the critical temperature and pressure. | 2F7 |

equation of state (EOS) | Soave-Redlich-Kwong (SRK) | A cubic, empirical EOS that accurately represents the behavior of a wide variety of systems, especially hydrocarbons. Its three parameters are empirical functions of the critical temperature and pressure and the Pitzer Accentric Factor. | 2F8 |

equation of state (EOS) | van der Waals | The original cubic EOS, the van der Waals EOS is not empirical in nature, but has a theoretical basis. The derivation of the van der Waals EOS yields two parameters that are functions of the critical temperature and pressure. One of the parameters accounts for the attractive forces between the molecules and the other parameter represents the volume that the molecules themselves occupy. | 2F4 |

equation of state (EOS) | Virial | The Virial EOS is a power series expansion in terms of the inverse of the molar volume. The parameters of the Virial EOS can be interpreted in terms of statistical mechanics. The 2nd Virial Coefficient, B, is widely tabulated and its value for a pure compound at a given temperature can be estimated using the critical temperature and pressure and the Pitzer Accentric Factor. | 2F2 |

equilibrium | Equilibrium is a state of balance. No unbalanced potentials (or driving forces) exist within the system. If isolated from its surroundings a system at Equilibrium experiences no changes. | 1D5 | |

equilibrium | chemical | 1D5 | |

equilibrium | mechanical | 1D5 , 6 | |

equilibrium | phase | In a system at Phase Equilibrium, the rate at which molecules are making the transition OUT of each and every phase is exactly equal to the rate at which molecules are making the transition INTO the same phase. | 1D5 |

equilibrium | thermal | 1D5 | |

equilibrium | vapor-liquid | 2B2 | |

equilibrium state | 6A4 , 6 | ||

evaporation | Also known as vaporization. A process in which a molecule makes the transition from a liquid phase into the gas phase while the vapor pressure of the liquid phase is LESS than the total pressure of the system. | 2A8 | |

evaporator | 6B7 , 9 | ||

exact differential | The differentials of state variables or properties are exact differentials and they are represented by the prefix "d". For example: dV or dT. | 4A7 - 8 , 12 | |

expansion | 4A1 , 11 | ||

expansion | adiabatic | 6E6 , 10 , 11 | |

expansion | isothermal | 6E4 , 10 , 11 | |

expansion | reversible | 6E2 | |

expansion valve | 6B7 , 9 | ||

extensive property | Properties that depend on the size of the system. If you magically insert a divider that divides the system into two equal halves and consider just one of the half-systems, the value of any and all extensive properties will also be reduced by half. Examples of extensive variables include mass, volume and enthalpy. | 3C4 | |

external combustion | 9E2 , 3 | ||

externally reversible | 6D9 |