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MQ-2 on Monday, Feb. 21 at 6:30 pm Covering Chapters 13 (osmosis…), 14, and 15

MQ-2 on Monday, Feb. 21 at 6:30 pm Covering Chapters 13 (osmosis…), 14, and 15. Review session on Sunday, Feb 20 at 1:00 pm – 3:00 pm in Stillman 100. Alternate Exam time for students with scheduled class conflicts: 5:00 – 6:20 pm in 159 MacQuigg Labs sign up by email to mathews.

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MQ-2 on Monday, Feb. 21 at 6:30 pm Covering Chapters 13 (osmosis…), 14, and 15

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  1. MQ-2 on Monday, Feb. 21 at 6:30 pm Covering Chapters 13 (osmosis…), 14, and 15 Review session on Sunday, Feb 20 at 1:00 pm – 3:00 pm in Stillman 100 Alternate Exam time for students with scheduled class conflicts: 5:00 – 6:20 pm in 159 MacQuigg Labs sign up by email to mathews

  2. Second MQ exam – Chem 122 Monday, 21 February 6:30 pm LAB INSTRUCTORLOCATION Christopher Beekman* 250 Knowlton Hall Chitanya Patwardhan “ Ramesh Sharma “ Mark Lobas 180 Hagerty Hall Edwin Motari* “ Roxana Sierra “ Lin Sun “ All Others 131 Hitchcock Hall Knowlton Hall - 2073 Neil Avenue Hitchcock Hall - 2070 Neil Avenue Hagerty Hall - 1775 College Rd

  3. Chapter 15 Chemical Equilibrium • 15.1 The Concept of Equilibrium • 15.2 The Equilibrium Constant • The Magnitude of Equilibrium Constants • The Direction of the Chemical Equation and Keq • Other ways to Manipulate Chemical Equations and Keq • Units of Equilibrium Constants– Kp and Kc • 15.3 Heterogeneous Equilibria • 15.4 Calculating Equilibrium Constants • 15.5 Applications of Equilibrium Constants • Predicting the Direction of Reaction • Calculation of Equilibrium Concentrations • 15.6 Le Châtelier’s Principle • Change in Reactant or Product Concentrations • Effects of Volume and Pressure Changes • Effect of Temperature Changes • The Effect of Catalysts

  4. Completion of Chapter 15: 15.6 Le Châtelier’s Principle Change in Reactant or Product Concentrations Effects of Volume and Pressure Changes Effect of Temperature Changes The Effect of Catalysts

  5. Recall from last week: CO(g) + Cl2(g) = COCl2(g) 2 H2S(g) = 2 H2(g) + S2(g) C(s) + S2(g) = CS2(g) C(s) + CO2(g) = 2 CO(g) What happens if we increase PT ???

  6. Consider effect of Change in Temperature Exothermic reaction: CO + 3 H2 = CH4 + H2O ΔH = -206 kJ/mol or CO + 3 H2 = CH4 + H2O + 206 kJ therefore incr temp shifts eq to left!

  7. Where Kf is the equilibrium constant at temperature Tfand Kiis the equilibrium constant at temp. Ti .

  8. Example: Consider a reaction which has Keq = 1.38 x 105 at 800 K and Keq = 4.9 x 1027 at 298 K. What is ΔH for the reaction?

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