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handout_L06_GibbsFreeEnery - Lecture 5 Summary sys < 0...

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Lecture 5 Summary sys surr univ ∆Η ° sys < 0 sys surr univ ∆Η ° sys < 0 sys surr 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: • Or : 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: – If S univ > 0…..process is spontaneous – If S univ < 0…..process is spontaneous in opposite direction. – If 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: – If S univ > 0…..process is spontaneous – If S univ < 0…..process is spontaneous in opposite direction.
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