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Chem 113 Week 6

by: Caroline Hurlbut

Chem 113 Week 6 Chem 113

Caroline Hurlbut
GPA 3.7

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Intro to equilibrium, manipulating K values, and Le Chatelier's principle
General Chemistry II
Ingrid Marie Laughman
Class Notes
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This 2 page Class Notes was uploaded by Caroline Hurlbut on Friday February 26, 2016. The Class Notes belongs to Chem 113 at Colorado State University taught by Ingrid Marie Laughman in Spring 2016. Since its upload, it has received 15 views. For similar materials see General Chemistry II in Chemistry at Colorado State University.

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Date Created: 02/26/16
Intro to Equilibrium • reactants⁶products —forward rate=reverse rate • equilibrium is a constant state of movement and has nothing to do with the amount of reactants/products in a reaction —if there is a lot of product, the equilibrium leans to the right (direction of forward reaction) —if there is little product, the equilibrium leans to the left (direction of reverse reaction) • calculate equilibrium constant (K) = [B]^b/[A]^a = kf/kr —kf=forward rate constant —kr=reverse rate constant —only include gaseous and aqueous reactants and products calculate reaction quotient (Q) = [products]^coefficient • [reactants]^coefficient —K and Q do not have units —Q tell us relative amounts of reactants and products —at equilibrium Q=K • special cases of K —Kc refers to concentration in terms of molarity —Kp refers to concentration in terms of partial pressure: Kp=PB^b/PA^a • 2PbO2(s) + 8H^+(aq)⁶2Pb^4+(aq) + 4H2O(l) —Kc=[Pb^4+]^2 [H^+]^2 —equation multiplied by 2 from PbO2(s) + 4H^+(aq)⁶Pb^4+(aq) + 2H2O(l) —Kc2=(Kc1)^2 • rule for adding reactions - multiply K values —K3=K1 x K2 Le Chatelier’s Principle • Le Chatelier’s principle - if a dynamic equilibrium is disturbed by changing the conditions or adding stress to the system, the position of equilibrium shifts to counteract the change to reestablish an equilibrium • ex. Fe^3+(aq) + 3Cl^-(aq)⁶FeCl3(s) —Q = 1 *leave out solid FeCl3 [Fe^3+][Cl^-]^3 —adding more iron will shift equilibrium towards products—>Q increases • stoichiometric coefficients of the reactants/products must be different than 1 to affect Q • changing volume changes Q by the same factor volume changes by —ex. 2A(g)⁶B(g) volume is reduced by a factor of 3 —Q=K/3 —Q is small—>more reactants—>system shifts to the right to form more products • changing temperature changes K value and results in new equilibrium —ex. 2A⁶B temp is increased in this endothermic reaction —energy acts like a reactant, system shift to the right • ex. The system 2A(aq) + B(l)⁶C(aq) + D(g) is at equilibrium in a closed container. If the container is opened, what will happen to Q and the system? —if the container is opened, the gas component D will leave the system —loss of product—>Q decreases —because Q decreases, there are more reactants, so the system shifts to the right


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