19.9
Phase Diagram
The phase of a given substance depends on the pressure and temperature. Thus, plots of pressure versus temperature showing the phase in each region pr…
In nature, matter exists in three phases: solid, liquid, and gas. The transition between phases requires phase equilibrium between two phases and occurs at a specific temperature for a given pressure.
These conditions can be represented graphically with pressure and temperature as the axes, known as a phase diagram.
A phase diagram represents the phases of a substance that coexist in thermodynamic equilibrium and undergo phase transition under different conditions, such as temperature, pressure, or volume.
Water exists in the liquid phase at room temperature and atmospheric pressure. At temperature 0oC or below, the phase changes from liquid to solid, whereas when the temperature is above 100oC, it changes to a gas phase.
The transition between solid and gas is called sublimation, while the transitions from solid to liquid and from liquid to gas are known as fusion and vaporization, respectively.
The point when all three phases coexist is known as the triple point, and the point when the properties of two phases become indistinguishable is known as a critical point.
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Q1: What is a phase diagram and why is it useful?
A phase diagram graphically represents the phases of a substance in thermodynamic equilibrium using pressure and temperature as axes. It shows which phase exists under specific conditions and identifies phase transition boundaries. Phase diagrams provide considerable insights into the thermal properties of substances, allowing scientists to predict how matter behaves across different temperature and pressure ranges.
Q2: What are the three main phase transitions and how do they differ?
The three main phase transitions are fusion (solid to liquid), vaporization (liquid to gas), and sublimation (solid to gas). Each transition occurs at specific temperature and pressure conditions shown as boundary curves on a phase diagram. These transitions represent points where two phases coexist in equilibrium, and the conditions required depend on the substance's properties and its kinetic theory of an ideal gas behavior.
Q3: What happens to water's boiling point when pressure increases?
As pressure increases, water's boiling temperature rises gradually, reaching 374°C at 218 atm pressure. This principle is demonstrated in a pressure cooker, which cooks food faster than an open pot because water can exist as a liquid at temperatures greater than 100°C without completely boiling away. The boiling point curve illustrates this pressure-temperature relationship.
Q4: What is the critical point on a phase diagram?
The critical point is where the boiling point curve ends, representing the temperature and pressure above which liquid and gas phases become indistinguishable. At this point, a substance is called a supercritical fluid. Above the critical point, a gas has the density of a liquid but does not condense, even at high pressure. For water, this occurs at 374°C and 218 atm.
Q5: What is the triple point and why is it significant?
The triple point is the unique condition where all three phases—solid, liquid, and gas—coexist in thermodynamic equilibrium. For water, this occurs at 273.16 K (0.01°C) and 611.2 Pa. The triple point serves as a more accurate calibration temperature for scientific measurements than the melting point at standard atmospheric pressure, making it essential for precise thermodynamic studies.
Q6: How does pressure affect the phase of matter according to phase diagrams?
Phase diagrams show that pressure directly influences which phase a substance occupies at a given temperature. The solid curves representing phase boundaries indicate the exact pressures and temperatures where phases coexist. By reading a phase diagram, you can determine whether a substance is solid, liquid, or gas at any combination of pressure and temperature within the diagram's range.
Q7: What is a supercritical fluid and where does it appear on a phase diagram?
A supercritical fluid is a substance existing above its critical point, where the distinction between liquid and gas phases disappears. Carbon dioxide, for example, is supercritical at all temperatures above 31.0°C. On a phase diagram, the region above and to the right of the critical point represents supercritical conditions, where the substance exhibits unique properties combining characteristics of both liquids and gases.