“internal energy”的概念、定义、翻译、参考文献-科学参考

internal energy

Physics

Symbol U. The total of the kinetic energies of the atoms and molecules of which a system consists and the potential energies associated with their mutual interactions. It does not include the kinetic and potential energies of the system as a whole nor their nuclear energies or other intra-atomic energies. The value of the absolute internal energy of a system in any particular state cannot be measured; the significant quantity is the change in internal energy, Δ‎U. For a closed system (i.e. one that is not being replenished from outside its boundaries) the change in internal energy is equal to the heat absorbed by the system (Q) from its surroundings, less the work done (W) by the system on its surroundings, i.e. Δ‎U=Q−W. See also energy; heat.

Chemistry

The total of the kinetic energies of the atoms and molecules of which a system consists and the potential energies associated with their mutual interactions. It does not include the kinetic and potential energies of the system as a whole nor their nuclear energies or other intra-atomic energies. The value of the absolute internal energy of a system in any particular state cannot be measured; the significant quantity is the change in internal energy, Δ‎U. For a closed system (i.e. one that is not being replenished from outside its boundaries) the change in internal energy is equal to the heat absorbed by the system (Q) from its surroundings, less the work done (W) by the system on its surroundings, i.e. Δ‎U = Q – W. See also energy; thermodynamics.

Chemical Engineering

A conceptual state function whose absolute value can be neither measured nor calculated. It represents the total energy in a substance and includes the atoms and molecules and their intra-atomic, inter-atomic, and inter-molecular forces. It includes neither the kinetic energy nor the potential energy. It is used in energy balance equations in terms of its relative value to a reference state, whose internal energy is arbitrarily set to zero. For a closed system, the change in internal energy ΔU is equal to the difference between the heat absorbed from the surroundings, Q, and the work done, W, by the system on its surroundings ΔU = Q −W. The concept was proposed by American physicist Josiah Willard Gibb (1839–1903).

单词	internal energy
释义	internal energy Physics Symbol U. The total of the kinetic energies of the atoms and molecules of which a system consists and the potential energies associated with their mutual interactions. It does not include the kinetic and potential energies of the system as a whole nor their nuclear energies or other intra-atomic energies. The value of the absolute internal energy of a system in any particular state cannot be measured; the significant quantity is the change in internal energy, Δ‎U. For a closed system (i.e. one that is not being replenished from outside its boundaries) the change in internal energy is equal to the heat absorbed by the system (Q) from its surroundings, less the work done (W) by the system on its surroundings, i.e. Δ‎U=Q−W. See also energy; heat. Chemistry The total of the kinetic energies of the atoms and molecules of which a system consists and the potential energies associated with their mutual interactions. It does not include the kinetic and potential energies of the system as a whole nor their nuclear energies or other intra-atomic energies. The value of the absolute internal energy of a system in any particular state cannot be measured; the significant quantity is the change in internal energy, Δ‎U. For a closed system (i.e. one that is not being replenished from outside its boundaries) the change in internal energy is equal to the heat absorbed by the system (Q) from its surroundings, less the work done (W) by the system on its surroundings, i.e. Δ‎U = Q – W. See also energy; thermodynamics. Chemical Engineering A conceptual state function whose absolute value can be neither measured nor calculated. It represents the total energy in a substance and includes the atoms and molecules and their intra-atomic, inter-atomic, and inter-molecular forces. It includes neither the kinetic energy nor the potential energy. It is used in energy balance equations in terms of its relative value to a reference state, whose internal energy is arbitrarily set to zero. For a closed system, the change in internal energy ΔU is equal to the difference between the heat absorbed from the surroundings, Q, and the work done, W, by the system on its surroundings ΔU = Q −W. The concept was proposed by American physicist Josiah Willard Gibb (1839–1903).
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