Ch.11 - Liquids, Solids & Intermolecular ForcesWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Consider the phase diagram for carbon dioxide.If you increase the pressure of carbon dioxide that is at body temperature (37˚C), will it ever liquefy?

Problem

Consider the phase diagram for carbon dioxide.
The figure shows a phase diagram of a compound. X-axis is for temperature values, and y-axis is for pressure values. The triple point is at 5.1 atmospheres at minus 56.7 Celsius degrees. Critical point is at 72.9 atmospheres at 31 Celsius degrees. The fusion curve goes up at almost vertical and slightly positive slope. There is also a point at the sublimation curve at 1 atmosphere and minus 78.5 Celsius degrees.

If you increase the pressure of carbon dioxide that is at body temperature (37˚C), will it ever liquefy?