What is thermal energy?
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Thermal energy refers to several distinct physical concepts, such as the internal energy of a system; heat or sensible heat, which are defined as types of energy transfer; or for the characteristic energy of a degree of freedom in a thermal system, where is temperature and is the Boltzmann constant.
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In thermodynamics, heat is energy in transfer to or from a thermodynamic system, by mechanisms other than thermodynamic work or transfer of matter.[1][2][3] Heat refers to a quantity transferred between systems, not to a property of any one system, or 'contained' within it.[4] On the other hand, internal energy is a property of a single system. Heat and work depend on the way in which an energy transfer occurred, whereas internal energy is a property of the state of a system and can thus be understood without knowing how the energy got there.
In a statistical mechanical account of an ideal gas, in which the molecules move independently between instantaneous collisions, the internal energy is the sum total of the gas's independent particles' kinetic energies, and it is this kinetic motion that is the source and the effect of the transfer of heat across a system's boundary. For a gas that does not have particle interactions except for instantaneous collisions, the term 'thermal energy' is effectively synonymous with 'internal energy'. In many statistical physics texts, "thermal energy" refers to
k
T
kT, the product of Boltzmann's constant and the absolute temperature, also written as
k
B
T
{\displaystyle k_{\text{B}}T}.[5] In a material, especially in condensed matter, such as a liquid or a solid, in which the constituent particles, such as molecules or ions, interact strongly with one another, the energies of such interactions contribute strongly to the internal energy of the body, but are not simply apparent in the temperature.
The term 'thermal energy' is also applied to the energy carried by a heat flow,[6] although this can also simply be called heat or quantity of heat.
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In a statistical mechanical account of an ideal gas, in which the molecules move independently between instantaneous collisions, the internal energy is the sum total of the gas's independent particles' kinetic energies, and it is this kinetic motion that is the source and the effect of the transfer of heat across a system's boundary. For a gas that does not have particle interactions except for instantaneous collisions, the term 'thermal energy' is effectively synonymous with 'internal energy'. In many statistical physics texts, "thermal energy" refers to
k
T
kT, the product of Boltzmann's constant and the absolute temperature, also written as
k
B
T
{\displaystyle k_{\text{B}}T}.[5] In a material, especially in condensed matter, such as a liquid or a solid, in which the constituent particles, such as molecules or ions, interact strongly with one another, the energies of such interactions contribute strongly to the internal energy of the body, but are not simply apparent in the temperature.
The term 'thermal energy' is also applied to the energy carried by a heat flow,[6] although this can also simply be called heat or quantity of heat.
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