Final Review answers:
p. 255
25a. HCl(aq) is the limiting reagent
b. 0.166 g H2
p. 304
13. 6.64 kJ
14. 89.4 kJ
p. 337
12. 3.39 L
13. 8.36 L
p. 343
24. 2.53 g
25. 17.6 L
p. 351
37. 93.4 kPa
38. 3.3 kPa
p. 386
38. 3.85 x 10-19 J
51. 3.08 x 10-19 J
p. 528
50.a. 1.3 M KCl
b. 0.33 M MgCl2
52.a 29.2 g NaCl
c. 2.78 g CaCl2
55.a. 100.26 oC
b. 101.56 oC
58.a. - 4.46 oC
b. - 22.3 oC
p. 609
39.a pH = 2 acidic
b. pH = 12 basic
c. pH = 6 acidic
d. pH = 6 acidic
40.a. [OH-] = 1.0 x 10-10
42. [H+] = 1.58 x 10-4
63.a. [OH-] = 3.98 x 10-10
c. pH = 12.26
Answers to Stoichiometry worksheets posted on Wednesday 1/30/08
Stoichiometry Practice Worksheet
1) 355 grams Na2SO4
2) 314 grams LiNO3
Mass to Mass Stoichiometry Problems
1) 36 grams LiBr
2) 141 grams carbon dioxide
3) Skip - typo
4) 27 grams sulfuric acid
Limiting Reagent Worksheet
1) CuCl2 + 2 NaNO3 --> Cu(NO3)2 + 2 NaCl
2) 13.0 grams NaCl
3) CuCl2
4) ~ 1 gram
5) 86.9 %
Percent Yield Worksheet
1) 2 FePO4 + 3 Na2SO4 --> Fe2(SO4)3 + 2 Na3PO4
2) 33 grams iron (III) sulfate
3) 55.9%
4) yes
Chapter 10 review problems posted on Tues 2/13/07
39. a. about 50 mm Hg
b. about 93 degrees Celsius
c. 760 mm Hg = standard pressure
42. escaping molecules have more KE than remaining molecules
this lowers the average KE
45. The forces between molecules of molecular solids are weaker
47. molecules are using the added heat to escape liquid; average KE stays
the same
48. see notes or text
Midterm Review Information:
Chemistry
Midterm Review Sheet
Text: Chapters 1-8; all notes, practice problems, homework
Topics:
Chemical and Physical Properties
Chemical and Physical Changes
Metric Prefixes
Significant Figures
Conversion factors and Dimensional Analysis
Density
Convert among Celsius, Fahrenheit, and the Kelvin temperature scale
Atomic theory ( Leucippus and Democritus,
Subatomic particles
Mass number, Atomic number, Isotope
Nuclear notation and Isotope notation
Calculate the atomic mass of an element given the percent abundance and relative atomic mass of the isotope(s)
Determine the relative mass and percent abundance of an unknown isotope given the atomic mass, the relative mass and percentage of the other isotope(s)
Organization of the Periodic Table
Ionic vs. Molecular compounds
Nomenclature
Convert among mass, representative particles, and mole of a given substance
Calculate percent composition of a substance from its chemical formula or experimental data
Derive the empirical formula of a compound from experimental data
Derive the molecular formula of a compound from experimental data
Chemical Reactions
Chemistry Review Problems
From Text
Chapter 2: Matter and Change: p. 47: 30, 32, 34, 35, 42
Chapter 3:
Scientific Measurement: p. 78-
Chapter 4: Problem
Solving: pp. 103-
Chapter 5: Atomic Structure and the Periodic Table: p. 129: 33 – 43
Chapter 6:
Chemical Names and Formulas: pp. 166-
Chapter 7: Chemical
Quantities (the MOLE): pp. 198-
Chapter 8: Sample
test
See Below for Notes Review on BONDING
2/23/06 see below for THERMOCHEMISTRY PROBLEMS
Mole Practice Quiz
Name the representative particle of the underlined substance:
a) a piece of aluminum foil
b) the carbon dioxide you exhale
c) an airbag full of nitrogen gas
d) baking soda, NaHCO3
How many O atoms are in the compound baking soda? See formula above in d)
Convert 0.05 grams of aluminum to moles.
Find the mass, in grams, of 2.7 moles of aluminum hydroxide.
Convert 5.00 x 1023 molecules of carbon dioxide to moles.
Nomenclature Review (answer key)
1. H2SO4 (aq)
2. N2O
3. K2CrO4
4. CuSO4 . 5H2O
5. Sn(OH)4
6. HNO3 (aq)
7. CO
8. H3PO4 (aq)
9. SnF2
10. Mg(NO3)2
11. NH4OH
12. SO3
13. Mg(OH)2
14. Fe(ClO3)3
15. NaHCO3
16. BaSO3
17. LiC2H3O2
18. N2O
19. AlN
20. RbMnO4
21. Sr(CN)2
22. Hydrochloric acid
23. Cesium chlorate
24. Magnesium sylfate heptahydrate
25. Dichlorine Heptoxide
26. Sulfur trioxde
27. Acetic acid
28. Carbonic acid
29. Calcium sulfate
30. Sodium phosphite
31. Barium sulfite
32. Ferrous chloride
Iron (II) chloride
33. Stannous oxide
Tin (II) oxide
34. Silver nitrite
35. Cadmium cyanide
36. Zinc chloride
37. Gold (III) chloride
38. Aluminum hydroxide
39. Lye or caustic soda
40. Potassium acetate
41. Sulfur dioxide
42. Plumbous fluoride
Lead (II) fluoride
GOOD LUCK!!
Practice Quiz: MOLES
THERMOCHEMISTRY HOMEWORK HOTLINE:
6. When 80.0 g of a certain metal at 90.0 degrees Celsius was mixed with 100.0 g of water at 30.0 degrees Celsius, the final equilibrium temperature
of the mixture was 36 degrees Celsius. What is the specific heat of the metal?
HINT: q (lost by the metal) = q (gained by the water)
Solve for C metal
7. What amount of ice must be added by 540.0 g of water at 25 degrees Celsius to cool the water to 0.0 degrees Celsius and have no ice remaining?
HINT: q (lost by the liquid water as it cools) = q (gained by the ice as it melts)
for the liquid water: q = mcDT for the ice: q = DHfusion x moles of ice
Set these two relationships equal to each other and solve for moles of ice!!
NOTES REVIEW: BONDING
1. unstable
2. configuration
3. bond
4. metallic
5. low, low
6. lose
7. 1s22s22p63s1 loses, Ne
8. +1, ion or cation
9. promote
10. overlap
11. cloud or sea of electrons
12. cations, electrons
13. upper right
14. 5, 6, 7, 1
15. high, high
16. covalent
17. nonpolar
18. H - H
19. 7, 3, 1
20.
21. sigma
22. 6, 2, 2
23.
24.
25. double
26. sigma, pi
27. 5, 1, 3
28.
29. triple
30. 1, 2