Textbook Chapters for Exam 2
Chapters 6 and 7. You’re responsible for any material covered in class whether it was on the homework or not. This review
sheet covers most everything we have done.
Also remember that no equations are given on the exams. Values for equilibrium
constants are given where needed although you should know
K
w
.
Chemical Equilibrium
• Know how to WRITE the
mass action expression
— same as
equilibrium equation
How does this expression change and the value of
K
when a
reaction is "flipped", doubled, halved?
When is this expression equal to
Q
? When is it equal to
K
?
• What is thermodynamic
K
? How does that relate to
K
p
and
K
c
?
• How does
K
p
relate to
K
c
?
When would they be equal?
• What is the relationship between
±
G
rxn
and
Q
?
between
±
G
0
rxn
and
K
?
• What are the units for an equilibrium constant? There are NO
units. Why?
• Calculations involving the equilibrium constant,
K
• Know how to calculate the equilibrium constant if given equi
librium amounts of reactants and products. This is where you
are given the entire bottom row (final equilibrium concentra
tions) of the equilibrium table (ICE Table) that we use.
• Know how to calculate the equilibrium constant if given ini
tial concentrations and ONE
f
nal concentration at equilib
rium. This is where you are given only ONE of the bottom
row concentrations of your equilibrium table.
• Know how to calculate
f
nal (equilibrium) concentrations if
given initial concentrations and the value of
K
c
. This is the
typical type problem where you must set up and solve the
equilibrium expression for
x
. Your entire bottom row will be
lots of concentration formulas containing
x
.
• Know how to predict the direction of a reaction if given con
This preview has intentionally blurred sections. Sign up to view the full version.
View Full Document
This is the end of the preview. Sign up
to
access the rest of the document.
 Spring '08
 FLOWERS
 pH, Kc, final equilibrium concentrations, Dr. McCord CH302

Click to edit the document details