Lec14 - Announcements Learning Skills Center Last Time Equilibrium from initial conditions Practice practice practice Molar proportions Equilibrium

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1 Announcements • Learning Skills Center • Practice, practice, practice Last Time • Equilibrium from initial conditions – Molar proportions – Equilibrium tables – using “x” • Changing reaction conditions – LeChatelier’s principle Le Chatelier’s Principle • Equilibrium adjusts to release stress • Explains changes in reactions due to – n – number of moles used – P – pressure of components – T – temperature of reaction • Changes in n, P, and T effect Q and K Addition of Reagents • Changes Q, and returns to equilibrium, K aA bB K c = • Increase A, more B forms, K c is constant • Increase B, more A forms, K c is constant [B] b [A] a
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2 Reaction Compression • Reaction responds by decreasing pressure • Increase pressure – favors fewer particles • Decrease pressure – favors more particles 2SO 2 (g) + O 2 (g) 2SO 3 (g) 2HBr(g) H 2 (g) + Br 2 (g) Reaction Temperature • Depends on reaction enthalpy, Δ H Δ H < 0, exothermic reaction
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This note was uploaded on 04/23/2008 for the course CHEM 2B taught by Professor Clemens during the Winter '08 term at UC Davis.

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Lec14 - Announcements Learning Skills Center Last Time Equilibrium from initial conditions Practice practice practice Molar proportions Equilibrium

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