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Lecture 5: Dynamic Equilibrium

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Lecture 5: Dynamic Equilibrium Chem 31B

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Lecture 5 Notes: Dynamic Equilibrium given on January 13, 2016
COURSE
Principles of Chemistry II
PROF.
Jennifer Poehlmann
TYPE
Class Notes
PAGES
2
WORDS
CONCEPTS
Reaction Rates, dynamic equilibirum
KARMA
25 ?

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This 2 page Class Notes was uploaded by it's lit notes on Wednesday January 13, 2016. The Class Notes belongs to Chem 31B at Stanford University taught by Jennifer Poehlmann in Fall 2015. Since its upload, it has received 20 views. For similar materials see Principles of Chemistry II in Chemistry at Stanford University.

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Date Created: 01/13/16
Wednesday  January 13, 2016  2  Lecture 5: Dynamic Equilibrium  ● in dynamic equilibrium → there are two reactions going on (forward and reverse) with  equal rates  ○ A is being formed at the same rate that A is being consumed  ● dynamic equilibrium requires a ​closed system and a reversible system  ● the equilibrium concentrations do not change with time once they are in equilibrium →  does ​ot mean that A and B are equal  ● rate constants are kinetic parameters that depend on temperature so eq​epends on  temperature  ○ the only thing that can change Keq​for a reaction is temperature  kf=  C][D]=  Keq  kr [A][B] ● K​ eq​s a thermodynamic parameter that tells you how far a rxn proceeds before reaching  equilibrium  ● k​f​and kr​epend on a mechanism but their ration does not    Clicker Question #1  A + B  ⇔ C + D  If K​  >>> 1, the following must be true:  eq​ a.) the reaction occurs at a very high temperature  b.) [C]​[D]​ >>> 1  eq​ eq​ c.) products are favored at equilibrium  d.) equilibrium is reached very rapidly  e.) at equilibrium, fwd rate >>> reverse rate    ● aA (aq) + bB (aq) ⇔ cC (aq) + dD  c d K​   ​[C]  [D]    c​ [A]  [B] b ● K​ c​= equilibrium constant using concentrations (aqueous)  ● K​  = equilibrium constant using partial pressures (gases)  p​ ● pure solids and liquids are not included in theeq​xpression because their concentrations  do not change with reaction progress  Clicker Question #2  What is the correct expression for K​ :  eq​ CaCO​ 3​s) ⇔CaO (s) + CO​ 2​(g)  a.) [CaO][CO​2​ / [CaCO3​  b.) [CaCO​3​ / [CaO][CO2​  c.) [CaO] x P(CO​2​ / [CaCO3​  d.) P(CO​2​  e.) [CaO] / [CaCO​3​   Wednesday  January 13, 2016  2  ● for a series of reactions that add together to form a net reaction, the overall value oeq​  K​1​x K2​k K3    Clicker Question #3  At 25​C, if I start with [A] = 10M and [B]​  = 0M, at equilibrium [A]​  = 2M, [B]​  = 8M and  0​ 0​ eq​ eq​ K​eq​ x. If I start with [A0​= 20M and [B]​ 0​= 0M then K​ eq​t 25​C =?  a.) 2x  b.) x  1/2  c.) x​ d.) x  e.) insufficient information to answer  solution: at 25C, K​  is the same for the same reaction;   eq​ K​eq​oes not depend on [A]​0    Clicker Question #4  1.) at equilibrium, kf​= kr  2.) the equilibrium concentration of a reactant does not depend on its initial  concentration  3.) reaction rates depend on temperature; so temperature affects how quickly you  reach equilibrium, but it does not change K​ eq a.) all statements are correct  b.) all statements are wrong  c.) 1 and 3 are correct  d.) 2 and 3 are correct  e.) only 3 is correct 1.) at equilibrium, the forward rate = the reverse rate but the rate constants do not need to be  the same  2.) Keq​does not depend on initial concentration  3.) K​  does depend on temperature  eq​

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