handout_L06_GibbsFreeEnery

handout_L06_GibbsFreeEnery - Lecture 5 Summary sys < 0...

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Lecture 5 Summary S°sys S°surr S°univ ∆Η °sys < 0 S°sys S°surr S°univ ∆Η °sys < 0 S°sys S°surr S°univ ∆Η °sys > 0 Lecture 6: Gibbs Free Energy • Reading: Zumdahl 10.7, 10.9 • Outline – Defining the Gibbs Free Energy ( G) – Calculating G – Pictorial Representation of G Defining G • Recall, the second law of thermodynamics: S univ = S total = S system + S surr • Also recall: S surr = - H sys /T • Then , ∆ S total = S system + S surr - H sys /T −Τ∆ S total = -T S system + H sys Defining G (cont.) • We then define: G = -T S total • Then: •O r : G = H - T S G= ±-T S sys + H sys G = The Gibbs Free Energy w/ P const G and Spontaneous Processes • Recall from the second law the condititions of spontaneity: • Three possibilities: –I f S univ > 0…. .process is spontaneous f S univ < 0…. .process is spontaneous in opposite direction. f S univ = 0….equilibrium • In our derivation of G, we divided by -T; therefore, the direction of the inequality changes relative to entropy. G and Spontaneous Processes (cont.) • Three possibilities: f S univ > 0…. .process is spontaneous f S univ < 0…. .process is spontaneous in opposite direction.
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This note was uploaded on 01/18/2012 for the course CHEM 152A taught by Professor Chiu during the Winter '12 term at University of Washington.

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handout_L06_GibbsFreeEnery - Lecture 5 Summary sys &lt; 0...

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