Definitions

1. Internal energy is a state function, which means it is solely dependant on the current conditions of the system. (Web site)
2. Internal energy is the sum of all microscopic forms of energy of a system.
3. Internal energy is the amount of energy that is stored at the atomic level of a molecule. (Web site)
4. Internal energy is defined as the energy associated with the random, disordered motion of molecules. (Web site)
5. The internal energy is associated with the motion, interaction and bonding of the molecules within a substance. (Web site)

Initial Energy

1. They may derive their internal energy from the initial energy of collapse. (Web site)

Average Translational Kinetic Energy

1. The internal energy per particle is equivalent to the average translational kinetic energy of each particle.

State Function

1. This introduces the enthalpy into the formalism, which is defined as H = U + p V. Enthalpy, like internal energy is another state function.

Exchange Internal Energy

1. When two bodies of different temperature come into thermal contact, they will exchange internal energy until the temperature is equalized.

Function

1. The internal energy of the system is a function of these state variables only. (Web site)

Measure

1. A calorimeter is a device which is used to measure and define the internal energy of a system.

Similarly

1. Similarly, the internal energy is a function of temperature and specific volume. (Web site)

Compression

1. In this cycle, internal energy is removed from the system as heat at the same rate that it is added by the mechanical work of compression. (Web site)

Substance

1. The temperature of a substance is directly related to its internal energy. (Web site)
2. When the internal energy of a solid is increased by the application of an external energy source, the molecular vibrations of the substance increases.

Motion

1. It represents the internal energy of the fluid due to its motion. (Web site)

Complexities

1. The above complexities make for rather cumbersome blanket statements regarding the internal energy in T =0 substances. (Web site)

Ideal

1. The transfer of heat to an ideal gas at constant pressure increases the internal energy and performs boundary work (i.e. (Web site)

Nucleus

1. They must have been shot out from the struck nucleus in such a way that part, at least, of their energy was derived from the internal energy of the nucleus. (Web site)
2. Similarly, a nucleus could be raised (excited) in its internal energy only to certain permitted levels.

Vacuum Energy

1. In the following we will calculate the internal energy of the box at temperature T relative to the vacuum energy. (Web site)

Normal Matter

1. Rutherford also suggested that this internal energy is stored within normal matter as well. (Web site)

Energy Required

1. This internal energy also includes the energy required for activation and the breaking of bonded compounds into gaseous species. (Web site)

Form

1. In the absence of work interactions, the heat that is transferred to an object ends up getting stored in the object in the form of internal energy. (Web site)

Kinetic Energy

1. In case of an ideal gas, the internal energy is exactly given by the kinetic energy of the constituent particles. (Web site)
2. The engine converts internal energy in the fuel to kinetic energy in the exhaust, producing thrust. (Web site)

Rotational Kinetic Energy

1. Internal energy does not include the translational or rotational kinetic energy of a body as a whole.

Means

1. This means that all the energy we add will go directly into internal energy, which in turn raises the temperature of the gas. (Web site)

Associated

1. Latent energy the internal energy associated with the phase of a system.

Work

1. The necessary work for the compression increases the internal energy of the mixtures - the temperature is increased. (Web site)
2. More specifically it is the sum of the internal energy and the work done by an applied pressure. (Web site)

State

1. The forces that act on objects influence their motion, shape, internal energy and state of equilibrium. (Web site)
2. The symbol e means internal energy per unit mass; thus if ideal gases are considered, the equation of state is p = ρ(γ − 1) e.

Normal State

1. When the internal energy of the atom exceeds that of its normal state it is said to be excited.

Change

1. A steady state process occurs without a change in the internal energy of a system. (Web site)
2. This change in internal energy results in a change in the temperature of the fluid element. (Web site)

Volume

1. The said quantity is amount of entropy that may be increased without changing an internal energy or increasing its volume. (Web site)
2. Here, U is internal energy, T is temperature, S is entropy, p is pressure, and V is volume. (Web site)
3. Therefore the total internal energy of a given ideal gas would be unaffected by any state change that only affected the volume. (Web site)

Constant Volume

1. The constant volume heat capacity - c v - is a measure of the change in internal energy at a particular temperature and constant volume. (Web site)

Atoms

1. Chemical energy the internal energy associated with the different kinds of aggregation of atoms in matter.

Individual Atoms

1. For monoatomic helium and other noble gases, the internal energy consists only of the translational kinetic energy of the individual atoms. (Web site)

Sum

1. Internal energy and the energy being denoted by the P*V term are different, and in fact there is another important property that is assigned to their sum. (Web site)
2. Enthalpy: The sum of the internal energy of a body and the product of its volume multiplied by the pressure.
3. Thermal energy the sum of sensible and latent forms of internal energy.

Molecule

1. The more complex a molecule is, the more possibilities it has to radiate its internal energy. (Web site)
2. Chemical energy the internal energy associated with the atomic bonds in a molecule. (Web site)

Molecules

1. All objects (matter) have a certain amount of internal energy that is related to the random motion of their atoms or molecules.
2. Thermal Energy, or heat, is the internal energy in substances��the vibration and movement of the atoms and molecules within substances. (Web site)
3. But wait, you said that internal energy was a reflection of energy contained by the molecules. (Web site)

Temperature

1. In such a gas, all the internal energy is in the form of kinetic energy and any change in internal energy is accompanied by a change in temperature.
2. This means that the internal energy of an ideal gas is dependant upon only one variable, temperature, giving us U(T). (Web site)
3. Helmholtz free energy A is defined as A = U - TS where U, T and S are the internal energy, temperature, and entropy.

System

1. The entropy of a system depends on its internal energy and the external parameters, such as the volume. (Web site)
2. If the internal energy remains unchanged, the amount of work done on a system must equal the heat given up by it. (Web site)
3. In terms of heat, the system originally contains a certain amount of internal energy due to the vibration of its molecules. (Web site)

Complex Systems

1. In more complex systems, it is preferable to use the concept of internal energy rather than that of thermal energy (see Chemical energy below).

Thermodynamics

1. Work done by a system decreases the internal energy of the system, as indicated in the First Law of Thermodynamics.
2. In thermodynamics, such a system is one in which the volume, number of molecules, and internal energy are fixed (the microcanonical ensemble). (Web site)
3. Energetics: Ist law of thermodynamics; Internal energy; enthalpy; Hess's law; heat of reaction, fusion, and vaporisation. (Web site)

Energy

1. The state of equilibrium involves a form of internal energy we call "binding energy" or "bond energy", and this energy contributes to the mass of the system. (Web site)
2. Therefore, the amount of energy added by heat or work had to increase the internal energy of the system, which in turn determined the temperature.
3. From the standpoint of statistical mechanics, the internal energy is equal to the ensemble average of the total energy of the system. (Web site)

Entropy

1. In the thermodynamic limit this fact leads to an equation relating the change in the internal energy to changes in the entropy and the external variables. (Web site)
2. In the thermodynamic limit this fact leads to an equation relating the change in the internal energy to changes in the entropy and the external parameters. (Web site)
3. The entropy of a system depends on its internal energy and the external variables, such as the volume. (Web site)

Enthalpy

1. Temperature is used as a measure of the internal energy or enthalpy, that is the level of elementary motion giving rise to heat transfer.
2. Temperature is also related to the amount of internal energy and enthalpy of a system. (Web site)
3. If the flow is accelerated (c increasing), the enthalpy decreases (and the internal energy and the temperature).

Internal Energy

1. Work and heat are processes which add or subtract energy, while the internal energy U is a particular form of energy associated with the system.
2. In the absence of work done, a change in internal energy per unit volume in the material, ΔQ, is proportional to the change in temperature, Δu. (Web site)
3. The second law affords another rigorous definition of temperature as the variation of the internal energy with respect to changes in entropy of the system.

Categories

1. Enthalpy
2. Chemical Energy
3. Thermal Energy
4. Encyclopedia of Finance. > Technology > Energy > Entropy
5. Kinetic Energy
6. Books about "Internal Energy" in Amazon.com
   

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