Isothermal vs Adiabatic Process

In an isothermal process the temperature is held constant. Heat flows freely between system and reservoir. For an ideal gas, internal energy U is constant, so Q = W = nRT ln(V2/V1).

In an adiabatic process no heat is exchanged (Q = 0). For an ideal gas the equation of state along the path is PVγ = const, with γ = CP/CV. Internal energy change equals the work done: ΔU = −W.

On a P–V diagram, isothermal curves PV = nRT are gentler than adiabatic curves PVγ = const through the same point. Adiabatic compression heats the gas; isothermal compression keeps T fixed by removing heat. The Carnot cycle alternates two isothermal legs and two adiabatic legs.

Recent research on this topic from arXiv

Preprints and papers indexed on arXiv.org. Links open the public abstract pages.

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