When steam or gas is depressurized or released into a large open space, its temperature must drop, right?
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When steam or gas is depressurized or released into a large open space, its temperature must drop, right? In other words, the expansion of a gas does work on its surroundings, resulting in a loss of internal energy and a decrease in temperature
If the process of gas decompression or release does not involve expansion into a vacuum environment (that is, free expansion), it necessarily involves doing work on the surroundings, and the temperature will drop. :$
The work done on the outside is P*V, so can the decrease in temperature be calculated? ? ? ? The relationship between energy and temperature
In the case of adiabatic expansion, given the PVT parameters of the initial state, the P parameter of the final state, as well as the gas composition or specific heat ratio, for an ideal gas it is possible to use the equation PT^r=C to calculate the modal temperature; of course, using the equation of state will yield more accurate results.
A reminder: the calculations above apply to adiabatic reversible processes and are only approximate. Using DU = CvΔT might yield more accurate results