CH 112 Learning Objectives - Jones/Atkins Chapter 17:
The Direction of Chemical Change
(Handout 17.1: 3/12/01)

Special Notes

  • Assigned End-of-Chapter Exercises: #1, 7, 11, 23, 27, 33, 45, 57.
  • Problem strategies for these exercises should be handed in by 5 PM on Tuesday, March 20.

General Learning Objectives

  • You should be able to answer questions based on the Conceptual, Problem-Solving and Descriptive sections in the “Skills You Should Have Mastered” at the end of the chapter.

Classification of Material in Chapter 17

  • Facts
    • Sign conventions for entropy and free energy changes
  • Concepts
    • spontaneous and nonspontnaeous change
    • entropy or disorder
    • entropy of vaporization and fusion
    • standard molar entropies and standard reaction entropies
    • Gibbs free energy
    • standard free energy of formation
    • thermodynamicaly stable and unstable compound
  • Rules
    • The second and third law of thermodynamics.
    • Rules correlating ®S° or S° with chemical formulas, physical states, etc.
    • Free energy of elements in their standard state = 0.
    • ®S°(reaction) = án ®S°(products) -á m ®S°(reactants)
    • Rules for determining how ®G will change with temperature.
    • ®G° = ®H°-T®S° = án ®G°(products) -á m ®G°(reactants)
  • Generic Problems
    • Calculate the ®S° for any reaction from a table of standard entropy values.
    • Predict which substance or process has the higher entropy and why.
    • Calculate the entropy change in the surroundings.
    • Calculate the standard free energy change at constant temperature and pressure, ®G°, for any process from a table of standard thermodynamic values of ®G°, ®H° and ®S°.
    • Explain the magnitude and the sign of a free energy change and how it is affected by temperature.
    • Calculate the free energy change from an equilibrium constant or Q.

Back to Course List

This page has been accessed $hit_count times.

This page was last modified on $last_modified.