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It is written on Wikipedia: (https://en.wikipedia.org/wiki/Thermal_energy)

The thermal energy of a system scales with its size and is therefore an extensive property. It is not a state function of the system unless the system has been constructed so that all changes in internal energy are due to changes in thermal energy, as a result of heat transfer (not work). Otherwise thermal energy is dependent on the way or method by which the system attained its temperature.

My question is: Why thermal energy is dependent on the way or method by which the system attained its temperature? You only need to give me an example proving that. Thanks in advance.

Trần Nhật Quang
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    "Heat" is not a state function but energy is a state function, and so is "thermal energy" which is just another expression for "internal energy". Some people would like to banish the word "heat " as a noun from English and use it only as a verb, that is to heat something. Use it as a verb and then you will not get confused. – hyportnex Feb 01 '16 at 13:23
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    Wiki does not confuse between heat and thermal energy. – Trần Nhật Quang Feb 02 '16 at 07:52
  • I think this is a good question. Why can't we use $U_{\rm thermal}$, $U_{\rm non-thermal}$, $V$, and $N$ as state variables instead of $U$, $V$, $N$? Wouldn't that make things less confusing? – Eric David Kramer Mar 11 '19 at 13:31
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    My advice is to call the state variable $U$ by the name "internal energy". Do not call it "thermal energy"; that will just lead to confusion. – Andrew Steane May 24 '21 at 11:17
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    P.S. to increase the internal energy of a system without supplying any heat, simply consider any process where the system is thermally isolated and work is done on it. e.g. slowly compress a gas in an insulated cylinder. – Andrew Steane May 24 '21 at 11:25
  • From the Wikipedia link in the OP question: "The term "thermal energy" is used loosely in various contexts in physics and engineering. It can refer to several different well-defined physical concepts. " So, to have an answer you should make clear the exact definition of the quantity you are interested in. This may help: https://physics.stackexchange.com/q/278539/226902 (Thermal energy vs. internal energy?) – Quillo Sep 20 '22 at 16:21

2 Answers2

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An example you asked for :

Consider a system of an ideal gas where volume of the gas is constant (call it system A) and one where the pressure is constant (System B). Because the internal energy of the system is a state variable, same change in temperature would cause same change in internal energy. Now, $$ \Delta U = Q + W$$ In A volume is constant so W=0 and hence Thermal energy $Q$ is equal to $\Delta U$. But in B the gas will expand, doing some work (say $-W$) and hence for the same change in $U$ we need to supply more thermal energy, equal to $\Delta U +W$.

ParadigmShift
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Thermal energy is not a state variable because work can also contribute to thermal energy, e.g. through friction. Work can also contribute to other internal degrees of freedom. In general, work contributes to the total energy $$U = U_{\rm thermal} + U_{\rm non-thermal}.$$ Since work should be considered as contributing only to the total internal energy $U$, so should the heat $Q$, and therefore $$Q+W = \Delta U.$$ I think $Q$ could even contribute to non-thermal degrees of freedom if accompanied by an additional increase in entropy. I'm not 100% sure about this last statement.

Eric David Kramer
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