The discussion centers on the adiabatic process in thermodynamics, specifically addressing the relationship between changes in volume and pressure. When volume increases and pressure decreases, the process can be classified as adiabatic if the product of pressure (P) and volume (V) remains constant. However, this scenario indicates that work is done by the gas, leading to a change in internal energy and temperature, which implies that heat flow must occur. Thus, while the initial assumption of zero heat change is challenged, the adiabatic nature of the process is confirmed under specific conditions.
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PV can remain constant (for an ideal gas) only if T is constant. But if V changes, then work is done on or by the gas, so its internal energy, hence temperature, cannot be constant without some flow of heat.LowlyPion said:I think it's indeterminate without more information.
If the product of P*V remains the same with the increase of one and the decrease of the other then, all other things being equal, you could say it was adiabatic.