Skip to main content
Ch.12 - Liquids, Solids & Intermolecular Forces
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Not the one you use?Change textbook
All textbooksTro 6th EditionCh.12 - Liquids, Solids & Intermolecular ForcesProblem 79
Chapter 12, Problem 79

Consider the phase diagram shown here. Identify the states present at points a through g.

Verified step by step guidance
1
Identify the axes of the phase diagram. Typically, the x-axis represents temperature and the y-axis represents pressure.
Locate each point (a through g) on the phase diagram.
Determine the regions separated by the lines on the phase diagram. These regions usually represent different states of matter: solid, liquid, and gas.
For each point (a through g), identify which region it falls into to determine the state of matter present at that point.
If any point lies on a line or at a triple point, note that it represents equilibrium between phases or all three phases coexisting, respectively.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
2m
Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Phase Diagram

A phase diagram is a graphical representation that shows the states of a substance (solid, liquid, gas) at various temperatures and pressures. It illustrates the conditions under which distinct phases occur and coexist, helping to visualize transitions such as melting, boiling, and sublimation.
Recommended video:
Guided course
03:22
Phase Changes in Diagrams

Triple Point

The triple point of a substance is the specific condition at which all three phases (solid, liquid, and gas) coexist in equilibrium. This unique point is critical for understanding phase transitions and is used as a reference for defining temperature and pressure scales.
Recommended video:
Guided course
03:05
Boiling Point Elevation

Critical Point

The critical point marks the end of the phase boundary between the liquid and gas phases. Beyond this point, the substance cannot exist as a liquid regardless of pressure, leading to a supercritical fluid state where distinct liquid and gas phases do not exist.
Recommended video:
Guided course
03:05
Boiling Point Elevation
Related Practice
Textbook Question

Nitrogen has a normal boiling point of 77.3 K and a melting point (at 1 atm) of 63.1 K. Its critical temperature is 126.2 K and its critical pressure is 2.55×104 torr. It has a triple point at 63.1 K and 94.0 torr. Sketch the phase diagram for nitrogen. Does nitrogen have a stable liquid state at 1 atm?

2550
views
Textbook Question

Water is a good solvent for many substances. What is the molecular basis for this property, and why is it significant?

649
views
Textbook Question

A 10.5-g ice cube at 0°C is placed into 245-g of water. Calculate the temperature change in the water upon the complete melting of the ice. Assume that all of the energy required to melt the ice comes from the water.

Textbook Question

The phase diagram for sulfur is shown here. The rhombic and monoclinic states are two solid states with different structures. b. Which of the two solid states of sulfur is more dense?

525
views
Textbook Question

Calculate the amount of heat required to completely sublime 75.0 g of solid dry ice (CO2) at its sublimation temperature. The heat of sublimation for carbon dioxide is 32.3 kJ/mol.

Textbook Question

How much ice (in grams) would have to melt to absorb 155 kJ of energy?