Equilibrium
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Lecture Date
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Learning Objective
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Before Class
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During Class
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After Class
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#1
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2.1. Characterize chemical reactions in terms of reversibility and
relative concentrations of reactants and products.
2.2. Determine equilibrium expressions for homogeneous and heterogeneous
chemical reactions from stoichiometry.
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View the following video Demonstration
1. Shifting Reactions (FeSCN2+)
2. Shifting Reactions (Chromate/dichromate)
3. Shifting Reactions (Cobalt chloride)
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Web Text (LO 2.1 and 2.2)
Problem Tutorial and practice problems
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#2
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2.3. Determine the stoichiometric relationship between initial and
equilibrium concentrations of reactants and products.
2.4. Determine the relationship between Kold and Knew when a chemical
reaction is reversed or multiplied by a constant factor of n.
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Web Text (LO 2.3 and 2.4)
Tutorial and practice problems
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#3
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2.5. Determine the relationship between Kc and Kp
for a chemical reaction involving gaseous components.
2.6. Determine value for K from equilibrium concentrations of reactants
and products in a chemical reaction.
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Do a PLE
Q1 is write the equilibrium expression for a given reaction (tell
them the value of K)
Q2. Reverse reaction and ask student to write the equilibrium expression
and compare to the equilibrium expression in Q1 and calculate K for
the new reaction
Q3. Give a new reaction and its K and ask student to write the equilibrium
expression.
Q4. same equation only multiuplied by a whole number ask student to
write the equilibrium expression and compare to the equilibrium expression
in Q3 and calculate K.
Q5 give two equations and a third equation that is the sum of the
first two ask student to write the equilibrium expressions for each
equation and explain the relationship
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Web Text (LO 2.5 and 2.6)
Problem Tutorial and practice problems
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#4
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2.7. Determine the equilibrium concentrations of reactants and products
of a chemical reaction from initial concentrations and value of K.
2.8. Determine if equilibrium has been reached in a chemical reaction;
determine the direction the reaction will shift if equilibrium has not
been reached.
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Web Text (LO 2.7 and 2.8)
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#5
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2.9. Use Le Ch‰telierŐs Principle to predict the direction a reaction
at equilibrium will shift as a result of changes in concentration, pressure/volume,
and temperature as it approaches a new equilibrium.
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Web Text (LO 2.9)
Problem Tutorial and practice problems
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