Isotherms for Real Gases
Figure 2 shows an isothermal plot for a real gas. For large T, the isotherms look like those of an ideal gas. But as T falls, especially below a critical temperature TC, we see that the behavior is no longer ideal. The curves below Tc pass through a phase change of liquid to vapor.
The critical temperature TC has a inflection or critical point CP, where the pressure is transitioning from decreasing to increasing. As we go along an isotherm along or below TC, the pressure decreases, and begins increasing til we reach a maximum. Then the pressure begins falling again and becomes more or less constant. Because the pressure no longer increases as the volume becomes less, these regions are unstable.
Figure 3 shows an isotherm below TC that is labelled for clarification purposes. Starting at the right side of the diagram, the area after point c is where the pressure eventually becomes basically constant and the volume is small. Point c is where condensation occurs as the gas begins liquefying as we continue along the left of the plot. Between c and b is a phase where the liquid and vapor are in equilibrium. Point e is a maximum, and point d is a minimum. Ed is unstable and has not been observed in a lab. Pure supersaturated vapors have been measured along ec, and supercooled liquids have been measured along ad. Remember, supersaturated liquids have dissolved solute beyond the solubility limit, and supercooled liquids are those that are cooled to temperatures below that of their ordinary freezing points.
At point a, the substance is now wholly a liquid. The pressure begins rising rapidly because it takes a great deal of it to compress a liquid.
Is is important to note that above TC, no matter how large the pressure, it is not possible to liquefy a gas.
In the next part of the series, we will examine the van der Waals equation in light of carbon dioxide.
Figure 1 from Pezhe.com
Figure 2 from from Wikimedia Commons
Figure 3 from Answers.com