11.2 Phase Diagrams | General Chemistry

Chad provides a brief but comprehensive lesson on Phase Diagrams. He identifies the Lines of Equilibrium, how two phases are in equilibrium on these lines, and how a phase change occurs when one of these lines is crossed. He also identifies the Triple Point and the Critical Point i.e. the critical temperature and pressure above which a supercritical fluid exists. Finally, he identifies the normal melting point and the normal boiling point, and explains how to identify the various phase changes on a phase diagram. Chad then presents the phase diagram of CO2 revealing that CO2 in the solid phase is referred to as 'dry ice' as it undergoes sublimation at atmospheric pressure. He then presents the phase diagram of H2O showing that the solid-liquid line of equilibrium has a negative slope as the result of the solid phase being less dense than the liquid phase due to hydrogen bonding. This leads to some important characteristics of water that are essential for life and ice hockey.

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00:00 Lesson Introduction
00:38 Lines of Equilibrium, Phase Changes, & the Triple Point on a Phase Diagram
02:46 Critical Point and Supercritical Fluids on a Phase Diagram
07:34 Normal Melting Point and Normal Boiling Point on a Phase Diagram
08:18 Phase Diagram of CO2
09:16 Phase Diagram of H2O

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