ACS/NSTA Web Seminar: Entropy, Energy, and Temperature
Wednesday, December 15, 2010
If the entropy of a liquid is greater than that of its solid, why do solids ever form? Why can salts be used to melt ice in winter and cool old-fashioned ice-cream makers in summer? The answers to these questions (and many more) are tied up in the interplay of entropy, energy, and temperature.
In this web seminar, learn about the molecular level entropy model introduced in the previous seminar, extended to include energy and temperature effects. This molecular level view of entropy provides a more physically understandable and concrete picture than is often taught. You will begin with a model that is simple enough to visualize and count how entropy changes involving energy are characterized. Then you extrapolate the results to understand macroscopic, observable systems like phase changes for pure substances and solutions. These topics may be especially useful for honors, AP, or IB courses. You and your students can apply the model to understand how entropy, energy, and temperature can result in ice cream.
Presenters: Jerry Bell, Pat Deibert and Bonnie Bloom
Grade level: Middle School, High School
This web seminar is one of a series designed to provide secondary teachers insights into presenting difficult chemistry concepts in the context of every-day experiences students can relate to. These seminars are sponsored by the American Chemical Society (ACS) Education Division, Office of High School Chemistry. For more information about ACS resources for high school teachers, please visit acs.org/highschool.
Each web seminar is a unique, stand-alone, program. Archives of the Web Seminars and the presenters’ PowerPoint presentations will be available through the links on this web page.