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


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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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slide1

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

slide2

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

slide3

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
slide17

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

slide18

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 ???

slide19

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!

slide21

Where Kf is the equilibrium constant at temperature Tfand

Kiis the equilibrium constant at temp. Ti .

slide22

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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