 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 NaNO-->   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:

Physical States of Matter; Heterogeneous and Homogeneous Matter

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, Dalton , Thomson, Millikan, Rutherford , Chadwick)

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- 9:  39 , 42, 43, 44, 61, 65

Chapter 4: Problem Solving:  pp. 103- 4:  43 , 44, 48

Chapter 5: Atomic Structure and the Periodic Table: p. 129:  33 – 43

Chapter 6:  Chemical Names and Formulas: pp. 166- 7:  49 , 64

Chapter 7: Chemical Quantities (the MOLE): pp. 198- 9: 45 , 49, 51, 55, 56, 60, 62, 66

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.  CuSO5H2O

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

36.  Zinc chloride

37.  Gold (III) chloride

38.  Aluminum hydroxide

39.  Lye or caustic soda

40. Potassium acetate

41. Sulfur dioxide

42. Plumbous 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

HOMEPAGE