South Pasadena • Honors Chemistry
Name
8 • Equilibrium
Period
Date
STUDY GUIDE
8.1 Equilibrium Constant
Lesson Objectives
I can:
 explain how reversible reactions can reach
equilibrium when rates of forward and reverse
reactions are equal.
 describe what is observed when a system reaches
equilibrium.
 write the equilibrium constant of a chemical
equation.
 describe the relative amounts of substances of a
system at equilibrium using the magnitude of the
value of the equilibrium constant.
 calculate the concentration of a substance at
equilibrium using the value of the equilibrium
constant.
 determine whether a reversible reaction proceeds
toward the right or the left by comparing the
reaction quotient Q to Keq.
Reading Guide
Read sections 16.1-16.3 (p. 747-761).
1. How can we tell when a reaction has reached
equilibrium? (p. 748)
2. How do we write the equilibrium constant
expression? What do we do with solids or water?
(p. 750-751)
3. What does the magnitude of K tell us (i.e. what
does it mean if K >> 1 or if K << 1)? (p. 757)
4. What is the difference between Kc and the reaction
quotient Q? (p. 759-760)
5. What does the comparison between Q and K tell us
about our reaction mixture (i.e. what does it mean if
Q < K, Q = K, or Q > K)? (p. 761)
Additional Practice
Chapter 16: Study Questions 8, 16, 18, 20, 22, 24, 44,
46, 54.
8.2 Equilibrium Problems
Lesson Objectives
I can:
 find the amounts of each substance in a reaction
mixture at equilibrium given initial amounts and
value of K using an ICE Chart.
Reading Guide
Read sections 16.4-5 (p. 762-769).
Additional Practice
Chapter 16: Study Questions 30, 32, 34, 44, and 46.
8.3 Le Châtelier’s Principle
Lesson Objectives
I can:
 predict the direction a reaction will shift and how
the amounts of substances in the reaction mixture
will change if reactants/products are
added/removed, the pressure/volume of a gas
sample is changed, or if the temperature is changed.
Reading Guide
Read sections 16.6 (p. 770-776).
1. What does Le Châtelier’s Principle say? (p. 770)
2. How does changing the temperature affect the
direction of a system at equilibrium? (p. 771)
3. Why does adding or removing a reactant or product
shift the position of a reaction? (p. 772)
4. How does changing the volume of a gas sample
affect the direction of a system at equilibrium? (p.
776)
Additional Practice
Chapter 16: Study Questions 38 and 40.