Chemistry II Week 6 Notes
Chemistry II Week 6 Notes CHEM 1120
University of Memphis
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This 1 page Class Notes was uploaded by Annika Coley on Sunday March 6, 2016. The Class Notes belongs to CHEM 1120 at University of Memphis taught by Dr. Brewster in Spring 2016. Since its upload, it has received 11 views. For similar materials see GENERAL CHEMISTRY II in Chemistry at University of Memphis.
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Date Created: 03/06/16
Chemistry II Notes – Week 5 Ch. 16: Chemical Equilibrium Dynamic equilibrium o Both sides of a chemical equation are happening at the same rate Equilibrium constant o K o K is unitless o Ratio of products and reactants at equilibrium o Changing the concentration of anything changes everything o Law of mass action c d a b K = [C] [D] / [A] [B] aA+bB↔cC+dD o K is products over reactants o Reciprocal of reverse reaction As product concentration increases, the reverse reaction rate increases o At equilibrium, concentrations are constant Reactants and products aren’t necessarily equal in amount There can be product or reactant favored reactions When K is greater than one o Product favored reaction o Less reactants used When K is less than one o Reactant favored reaction o Less product remaining For gases o K p P xcP dd/ Paax P b o Partial pressures in atm o K p K xc(RT) Δn Delta n is the change in moles between reactants and products If it is zero then P will equal Kc Heterogeneous Equilibrium o Liquids and+solids don-t count o H 2(l) ↔ H (g) + OH (g) K c [H ][OH ] -
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