Chapter 17
Section 1:
1. When has a chemical reaction reached equilibrium?
2. What is a reversible reaction?
3. Which direction is a chemical reaction going in when equilibrium is reached?
4. Are the concentrations of reactants and products equal at equilibrium? Explain.
5. What is the equilibrium constant expression?
6. What is the equilibrium constant, Keq?
7. Describe the difference between a homogeneous equilibrium and a heterogeneous equilibrium.
8. How is a homogeneous equilibrium expressed?
Practice problem: Write the equilibrium expression for the following reaction:
N2O4(g)
2NO2(g)
9. How is a heterogeneous equilibrium expressed?
Practice problem: Write the equilibrium expression for the following reaction:
C10H8(s)
C10H8(g)
10. What does the data in Table 17.1 demonstrate about equilibrium constants (Keq)?
11. What does a large equilibrium constant tell you about the concentration of products and
reactants at equilibrium? Small equilibrium constant?
12. What are the three characteristics of all chemical reactions that reach equilibrium?
Complete practice problems:
#1b-e on p. 601
#3b-e on p. 603
#5,6,7 on p. 605
Section 2
13. What is Le Chatelier’s Principle?
14. How is O2 circulation in the body an example of Le Chatelier’s Principle?
15. List the five factors that influence equilibrium and describe their affect.
a. ________________________________ :
b. ________________________________:
c. _________________________________:
d. ______________________________:
e. _______________________________:
Section 3
Problem: The equilibrium constant for the reaction: 2H2S
2H2(g) + S2(g) is 2.27 X 10-3 at
1405K. What is the concentration of H2(g) if [S2]=0.540 mol/L and [H2S] = 0.184 mol/L?
p. 613 practice problem #18:
Ionic substances dissociate when they dissolve. Example: NaCl(aq)
Na+ + Cl- Table salt is
highly soluble in water so this process proceeds to the right and there is virtually no reverse process.
When substances do not readily dissolve, there is a reverse process. One example is barium sulfate,
BaSO4. Barium ions, Ba2+, are toxic to humans yet barium sulfate solution is safely ingested during X ray
procedures involving the digestive tract. Explain this. (p. 614-615)
16. How is a product solubility constant expressed?
17. What the Ksp value tell us about a substance?
Example problem: What is the solubility of AgI in mol/L at 298K?
In water, AgI(s)
Ag+(aq) + I-(aq).
Ksp = [Ag+][I-] = 8.5 X 10-17 at 298K
According to the chemical equation, one mole each of Ag+ and I+ are formed when one mole of AgI
dissolves. So we can substitute x for both Ag+ and I-:
(x)(x) = 8.5 X 10-17, x = 9.2 X 10-9 mol/L. This is the solubility.
18. Calculate the solubility for the following ionic compounds at 298K:
a. PbCrO4
Pb2+ + CrO42-13
Ksp = 2.3 X 10
b. AgCl
Ksp= 1.8 X 10-10
c. CaCO3
Ksp = 3.4 X 10-9
d. CaF2
Ksp = 3.5 X 10-11
e. Ag2CrO4
Ksp = 1.1 X 10-12
19. What is a common ion? The common ion effect?
20. How would adding K2CrO4 to a solution of PbCrO4 affect the solubility of PbCrO4? (hint: use the
common ion effect to answer this)
21. Would adding sodium sulfate, Na2SO4, to the BaSO4 that is ingested to X-ray the intestine make
the BaSO4 safer to ingest? Explain.