The phase diagram of a hypothetical substance is shown...

The phase diagram of a hypothetical substance is shown below. (a) Estimate the normal boiling point and freezing point of the substance. (b) What is the physical state of the substance under the following conditions? (i) $T=150 \mathrm{~K}, P=0.2 \mathrm{~atm}$ (ii) $T=100 \mathrm{~K}, P=0.8 \mathrm{~atm}$ (iii) $T=300 \mathrm{~K}, P=1.0 \mathrm{~atm}$ (c) What is the triple point of the substance? [Section 11.6]

The phase diagram of a hypothetical substance is shown below.
(a) Estimate the normal boiling point and freezing point of the substance.
(b) What is the physical state of the substance under the following conditions?
(i) $T=150 \mathrm{~K}, P=0.2 \mathrm{~atm}$
(ii) $T=100 \mathrm{~K}, P=0.8 \mathrm{~atm}$
(iii) $T=300 \mathrm{~K}, P=1.0 \mathrm{~atm}$
(c) What is the triple point of the substance? [Section 11.6]

Key Concepts

Phase Diagram

A phase diagram is a graphical representation that shows the conditions of temperature and pressure under which a substance exists in different phases (solid, liquid, and gas). It delineates the boundaries between phases and identifies regions where one phase is stable as well as lines where two or more phases coexist in equilibrium.

Normal Boiling Point

The normal boiling point is defined as the temperature at which a substance transitions from the liquid phase to the gas phase under a standard pressure of 1 atmosphere. It is found on the phase diagram at the intersection of the liquid–gas coexistence line and the line corresponding to 1 atm.

Normal Freezing Point

The normal freezing point is the temperature at which a substance changes from liquid to solid at a standard pressure of 1 atmosphere. On the phase diagram, it is located where the liquid–solid boundary meets the 1 atm pressure line, indicating the transition condition between these phases.

Triple Point

The triple point is the unique set of conditions (specific temperature and pressure) at which the three phases of a substance—solid, liquid, and gas—coexist in equilibrium. It is a fixed point on the phase diagram and is critical for understanding phase transitions.

Phase Equilibrium

Phase equilibrium refers to the state where different phases of a substance coexist without any net change in their proportions over time. This is depicted in the phase diagram by the coexistence curves, which separate regions of stability for each phase and indicate the conditions at which phase transitions occur.

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