Why does gas do work when it adiabatically expands into a vacuum?

Why does gas do work when it adiabatically expands into a vacuum? Physical Chemistry

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Warm-hearted netizen 

2017-08-20

The temperature of gas remains unchanged during vacuum expansion, which is a conclusion for ideal gases. Because in this process, the gas does no external work, and the gas is adiabatic, so according to the first law of thermodynamics, the internal energy of the gas remains unchanged. A characteristic of ideal gases is that internal energy is only related to temperature, so internal energy remains unchanged. This is an ideal situation. Ideal gases do not consider the mutual potential energy between gas molecules. Real gas molecules have potential energy between them; when they expand, they need to overcome the attractive forces between molecules to do work, so the temperature will decrease. Generally, this is the case, but if the gas is strongly compressed, an anomaly may occur; if the molecular forces manifest as repulsion, then the temperature will increase, but it's just a momentary thing. Generally, real gases will have a temperature decrease.

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