Name: _________________________
Hr: ____
Semester 2 Review – Part 4
Chapter 17-18
Label the following as endothermic or exothermic
1. 2SO3(g) + 198 kJ qe 2SO2(g) + O2(g)
2. 4Fe(s) +3O2(g) qe 2Fe2O3(s) ΔH = -1625 kJ
3. Water condensing
4. Coffee cooling
5. H2O(l) qe H2O(g)
________________
________________
________________
________________
________________
6. Write the following as a thermochemical equation (like #1).
4Fe(s) +3O2(g)  2Fe2O3(s) ∆H = -1625 kJ
How do you know if it is endothermic or exothermic?
7. Write the following thermochemical equation as a heat of reaction (like #2).
2SO3(g) + 198 kJ  2SO2(g) + O2(g)
How do you know if it is endothermic or exothermic?
8. What are the 3 main parts of collision theory?
a.
Reacting substances must ______________________.
b.
Reacting substances must collide with the correct _________________.
c.
Reacting substances must collide with the sufficient ___________ to form the
________________complex.
9. Define the following terms.
activated complex:
activation energy:
10. Besides the nature of the reactants, name four ways to increase the rate of a reaction.
a. Increase _____________________
b. Increase _____________________
c.
Increase _____________________
d. Add a ___________________
11. Use the following reaction mechanism to answers a-d.
Step 1: A2 + D2  2AD
(fast)
Step 2: AD + BC  AC + BD
(fast)
Step 3: BD + BC  B2 + CD
(slow)
Step 4: CD + AD  AC + D2
(fast)
a. Find the overall reaction for the following reaction mechanism:___________________________________
b. What is the rate determining step? ___________
c.
What is the catalyst? _____
d. What are the intermediates? _____ _____ _____
Parts of a Reaction Graph: Use the key below to label the following graph:
KEY
Reactants
Products
Activation energy
Activated complex
Energy of the reaction
The effect of a catalyst
The effect of an inhibitor
R
P
AE
AC
E
-----
12. Is this reaction endothermic or exothermic?______________________
Parts of a Reaction Graph: Use the key below to label the following graph:
KEY
Reactants
Products
Activation energy
Activated complex
Energy of the reaction
A
B
C
D
E
13. Is this reaction endothermic or exothermic?____________________
14. How does a catalyst speed up a reaction? Lowers the _____________________________________.
15. Complete the statements using the following word bank (words may be used more than once or not at all!)
equal
unequal
fast
constant
reversible
larger
smaller
In order for a reaction system to be in equilibrium,
a. the reaction must be ________________.
b. the forward and reverse rates must be ____________.
c. the concentrations of the reactants and products must be _____________, but not necessarily ____________.
d. If a reaction shifts to the right, the forward rate is ___________________ than the reverse rate.
16. State Le Chatelier’s principle.
17.
What are the 3 stresses that shift the equilibrium of a chemical system?
a.
b.
c.
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18.
Use the data in the following table for the formation of hydrochloric acid.
H2 + Cl2  2 HCl
[H2] (M)
[Cl2] (M)
[HCl] (M)
Time (s)
0.00
0.030
0.050
0.000
4.00
0.020
0.040
0.020
a. Calculate the average reaction rate for H2.
b. Calculate the average reaction rate for HCl.
19.
For the reaction below tell how the amount of O2 (g) present at equilibrium would be affected by each of the
following:
2 H2(g) + O2(g)  2 H2O(g)
H= 240 kJ
Change
Shift
(left, right, or no change)
[O2 ]
(increase, decrease, no change)
a) Some H2 is added.
b) Temperature is raised.
c) The volume is decreased.
d) The pressure decreased.
e) A catalyst is added.
f) Some H2O is removed.
20. Does adding a catalyst stress a system at equilibrium? __________
21.
For the reaction below tell how the amount of C (g) present at equilibrium would be affected by each of the
following:
2 A(g) + 2 B(g)  4 C(g)
H= -65 kJ
Change
Shift
(left, right, or no change)
[C]
(increase, decrease, no change)
a) Increase temperature
b) Decrease pressure
c) Adding B(g)
d) Removing A(g)
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Chapter 19: Acids and Bases
22. What are common properties that distinguish acids from bases?
Acid Properties
Base Properties
a. How does it taste?
____________
____________
b. How does it feel on your skin?
____________
____________
c.
____________
____________
d. Formula usually contains:
____________
____________
e. Litmus (what color to what color):
_________________
_________________
f.
_________________
_________________
Metal Reactivity:
Phenophthalein (what color to what color):
23. What is an Arrhenius
Acid: Compound that ionizes to make ______ (this ion is also called a ______________)
Base: Compound that ionizes to make ______
24. For the following equation, predict the products and balance. Include states of matter.
HNO3(aq)
+
Ca(OH)2(aq)

base ______________
acid _______________
salt ________________
25. What is a Brønsted-Lowry
Acid: proton (hydrogen ion) ________________
Base: proton (hydrogen ion) ________________
26. For the following reactions, label the acid (A), base (B), conjugate acid (CA), and conjugate base (CB):
NH4+ +
HF
OH-
+ H2O

NH3
+
H2O

F-
+
H3O+
27. What is the difference between a strong and weak acid/base? How much it ______________________.
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28. How is the hydrogen ion and the hydroxide ion concentration related to the acidity of a solution and its pH?
Acidic:
Basic:
Neutral:
[H+] (>,<,or =) [OH-] and pH (>, <, or =) 7
[H+] (>,<,or =) [OH-] and pH (>, <, or =) 7
[H+] (>,<,or =) [OH-] and pH (>, <, or =) 7
29. Identify each acid (HA,
) as strong or weak AND concentrated or dilute.
_________________
__________________
_________________
__________________
30. Circle one: The conductivity of a strong acid would be stronger / weaker than the conductivity of a weak acid.
31. Circle one: A single/double sided arrow is use to show the dissociation of a strong acid.
32. Circle one: A single/double sided arrow is use to show the dissociation of a weak acid.
33. pH =
35. pH + pOH = ____________
34. pOH =
36. [____]x[____] = 1x10-14
37. Fill in the following chart:
[H+]
[OH-]
pH
pOH
Acidic/Basic/Neutral
1  10-6
1  10-7
12.20
13.10
9.4  10-3
8.7  10-10
38.
If 43.4 mL of 0.10 M HCl was added to 52.3 mL of NaOH and reached equivalence point, what is the
concentration of the NaOH?
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