Question

(a) What is the significance of the critical point in a phase diagram? (b) Why does the line that separates the gas and liquid phases end at the critical point?

Short answer

The critical point in a phase diagram is significant because it marks the end of the phase boundary between the gas and liquid states and represents the highest temperature and pressure at which the liquid and gas phases can coexist in equilibrium. At the critical point, the liquid and gas phase possess the same density, and no distinction can be made between the two phases. Moreover, beyond the critical point, the substance exists as a supercritical fluid exhibiting properties intermediate between those of a gas and a liquid, which are widely used in various industrial applications. The line separating the gas and liquid phases, known as the vapor-liquid equilibrium curve, ends at the critical point because the liquid and gas phases become indistinguishable due to their identical densities and properties at that specific point. Beyond the critical point, the substance exists as a single supercritical fluid.

Step-by-step solution

(Explain what a phase diagram is)

A phase diagram is a graphical representation of the equilibrium between different states of matter (solid, liquid, and gas) as a function of pressure and temperature. It helps visualize the boundaries between different states of matter and understand the transitions between those states for a given substance.

(Define the critical point in a phase diagram)

The critical point is a specific point in the phase diagram that marks the end of the phase boundary between the gas and liquid states. At the critical point, the liquid and gas phase possess the same density, and no distinction can be made between the two phases. The critical point is characterized by the critical temperature (Tc) and critical pressure (Pc) of the substance and represents the highest temperature and pressure at which the liquid and gas phases can coexist in equilibrium.

(Explain the significance of the critical point)

The critical point plays a crucial role in understanding the properties and behavior of a substance under varying temperature and pressure conditions. At conditions beyond the critical point, the substance exists as a supercritical fluid that exhibits properties intermediate between those of a gas and a liquid. These supercritical fluids have unique solvating properties and are widely used in various industrial applications such as extraction processes, chemical reactions, and as solvents for substances that are insoluble in conventional solvents.

(Reason for the line separating the gas and liquid phases ending at the critical point)

The line that separates the gas and liquid phases in the phase diagram is called the vapor-liquid equilibrium curve or the coexistence curve. This line represents the set of conditions (pressure and temperature) at which the liquid and gas phases are in equilibrium with each other. The vapor-liquid equilibrium curve meets the critical point because, at that specific point, the liquid and gas phases become indistinguishable due to their identical densities and properties. Beyond the critical point, we cannot differentiate between the two phases, and the substance exists as a single supercritical fluid. Hence, the line separating the gas and liquid phases ends at the critical point.