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
Jan 19, 2016
MQ-2 on Monday, Feb. 21 at 6:30 pm
Covering Chapters 13 (osmosis…), 14, and 15
Review session on Sunday, Feb 20at 1:00 pm – 3:00 pm
in Stillman 100
Alternate Exam time for studentswith scheduled class conflicts:
5:00 – 6:20 pm in 159 MacQuigg Labssign up by email to mathews
Second MQ exam – Chem 122Monday, 21 February
6:30 pmLAB INSTRUCTOR LOCATION
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 AvenueHitchcock Hall - 2070 Neil AvenueHagerty Hall - 1775 College Rd
Chapter 15 Chemical Equilibrium
15.1 The Concept of Equilibrium
15.2 The Equilibrium ConstantThe Magnitude of Equilibrium ConstantsThe 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 ConstantsPredicting the Direction of Reaction
Calculation of Equilibrium Concentrations
15.6 Le Châtelier’s PrincipleChange in Reactant or Product ConcentrationsEffects of Volume and Pressure ChangesEffect of Temperature ChangesThe Effect of Catalysts
Completion of Chapter 15:
15.6 Le Châtelier’s PrincipleChange in Reactant or Product ConcentrationsEffects of Volume and Pressure ChangesEffect of Temperature ChangesThe Effect of Catalysts
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 ???
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!
ifi
f
TTR
H
K
K 11ln
Where Kf is the equilibrium constant at temperature Tf andKi is the equilibrium constant at temp. Ti .
Example: Consider a reaction which has Keq = 1.38 x 105 at 800 Kand Keq = 4.9 x 1027 at 298 K.
What is ΔH for the reaction?
molkJmolJxx
H
KKKmolJ
H
x
x
/214/1014.21011.2
84.450
298
1
800
1
)314.8(109.4
1038.1ln
53
1127
5