StudentLecture_08

StudentLecture_08 - Announcements Lecture 08, Monday...

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Announcements Lecture 08, Monday February 7, 2011 Exam I TONIGHT: Feb. 7. 8 PM Elliott Hall of Music Plan to arrive by 7:35 pm. Bring your PU ID, your seat assignment, a simple calculator, and pencils. HW5 due this Fri. (HW6 released). Good Luck Tonight! 1
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Lecture 08 Feb 7, 2011 Chemical Equilibria Reading: Ch. 16. Principles of Reactivity 16.1 Chemical Equilibrium: A Review 16.2 The Equilibrium Constant and Reaction Quotient (K and Q) 16.3 Determining an Equilibrium Constant 16.4 Using Equilibrium Constants in Calculations 16.5 More About Balanced Equations and Equilibrium Constants 16.6 Disturbing a Chemical Equilibrium (Le Chatelier’s principle) See also the Haber Process: p. 749
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Learning Objectives Understand the nature of chemical equilibium (reactions are reversible and dynamic at equilibrium) Understand the significance of the equilibrium constant K and the reaction quotient Q. Understand the significance of the magnitude of K (K>>1 or K <<1) and of K c and K p Use Q to decide if a reaction is at equilibrium (Q=K), or if a net conversion of product to reactant (K<Q) or reactant to product (K>Q) is needed to reach equilibrium Be able to calculate K eq or use K eq to calculate concentrations at equilibrium Know how to predict, using Le Chatelier’s principle, the effect of a disturbance on equilibrium.
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___________ applies to the ___________ of a reaction, the concentration of product that appears (or of reactant that disappears) per unit time. ________________ applies to the ___________ of a reaction, the concentration of product that has appeared after an unlimited time in a closed system, or once no further change occurs. ________________ : rate forward = rate reverse A system at equilibrium is _______________ on the molecular level; no further _____________________ because changes in one direction are balanced by changes in the other. Kinetics vs. Equilibrium
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______________: virtually all HCl dissociates to ions HCl H+ + Cl - _______________: less than 10% dissociates to ions CH 3 COOH CH 3 COO - + H + Speed of a reaction : both complete in ________ Kinetics vs. Equilibrium
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City A City B Not at equilibrium Rate fwd : 3 cars/min Rate rev : 0 cars/min Equilibrium is reached when opposing rates are equal
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Equilibrium is reached when opposing rates are equal City A City B Not at equilibrium: Rate fwd : 3 cars/min Rate rev : 1 cars/min
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Equilibrium is reached when opposing rates are equal City A City B 2 cars/min in both directions At equilibrium: rate forward = rate reverse
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Clicker question City A City B At equilibrium: rate forward = rate reverse What can we say, qualitatively about the _________________ for both directions?
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This note was uploaded on 02/27/2012 for the course CHEM 116 taught by Professor Stevenson during the Spring '08 term at Purdue.

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StudentLecture_08 - Announcements Lecture 08, Monday...

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