text: The adiabatic (no heat exchanged) expansion of a gas may be carried out in a number of ways. The change in temperature experienced by the gas during expansion depends not only on the initial and final pressure, but also on the manner in which the expansion is carried out.
  *If the expansion process is reversible, meaning that the gas is in thermodynamic equilibrium at all times, it is called an isentropic expansion. In this scenario, the gas does positive work during the expansion, and its temperature decreases.
  *In a free expansion, on the other hand, the gas does no work and absorbs no heat, so the internal energy is conserved. Expanded in this manner, the temperature of an ideal gas would remain constant, but the temperature of a real gas decreases, except at very high temperature.
  *The method of expansion discussed in this article, in which a gas or liquid at pressure P flows into a region of lower pressure P without significant change in kinetic energy, is called the Joule–Thomson expansion. The expansion is inherently irreversible. During this expansion, enthalpy remains unchanged (see proof below). Unlike a free expansion, work is done, causing a change in internal energy. Whether the internal energy increases or decreases is determined by whether work is done on or by the fluid; that is determined by the initial and final states of the expansion and the properties of the fluid.
  The temperature change produced during a Joule–Thomson expansion is quantified by the Joule–Thomson coefficient, . This  coefficient may be either positive (corresponding to cooling) or negative (heating); the regions where each occurs for molecular nitrogen, N, are shown in the figure. Note that most conditions in the figure correspond to N being a supercritical fluid, where it has some properties of a gas and some of a liquid, but can not be really described as being either. The coefficient is negative at both very high and very low temperatures; at very high pressure it is negative at all temperatures. The maximum inversion temperature (621 K for N) occurs as zero pressure is approached. For N gas at low pressures,  is negative at high temperatures and positive at low temperatures. At temperatures below the gas-liquid coexistence curve, N condenses to form a liquid and the coefficient again becomes negative. Thus, for N gas below 621 K, a Joule–Thomson expansion can be used to cool the gas until liquid N forms.