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ISU CHEM 178 - CHEM_178_Verkade_ac5849_chapter15-2_worksheet

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Supplemental Instruction 1060 Hixson-Lied Student Success Center  294-6624  www.si.iastate.edu Chapter 15 Chemical Equilibrium-2 Supplemental Instruction Iowa State University Leader: Alarm Cho Course: Chem 178 Instructor: John Verkade Date: Sep. 20, 2009 Chemical Equilibrium - Heterogeneous Equilibria PbCl2(s) Pb2+(aq) + 2Cl-(aq) Kc = CaCo3(s) CaO(s) + CO2(g) Kc = - Calculating Equilibrium Constants  When concentrations are known  ICE table sample exercise 15.9 H2(g) + I2(g) HI(g) Initial 1 x 10-3 M 2 x 10-3 M 0M Change Equilibrium 1.87 x 10-3 M - Applications of Equilibrium Constants  Reaction Quotient Q = K: Q << K: Q >> K:  Calculating Equilibrium concentrations  When concentrations are known  ICE table sample exercise 15.12 H2(g) + I2(g) HI(g) Initial 1 x 10-3 M 2 x 10-3 M 0M Change Equilibrium- Le Châtelier’s Principle  “If a system at equilibrium is disturbed by a change in temperature, pressure, or the concentration of one of the components, the system will shift its equilibrium position so as to counteract the effect of the disturbance.”  Change in concentration – Haber Process N2(g) + 3H2(g) 2NH3(g)  Change in volume or pressure N2O4(g) 2NO2(g)  Change in temperature Co(H2O)62+(aq) + 4Cl-(aq) CoCl42-(aq) +6H2O(l) ∆H > 0  Endothermic  Exothermic - Effect of


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