Honors Chemistry
Final Exam Review
Name ____________________________________________
Test Date: ____________ Time: ______________________
Room #: ______________ Proctor: ____________________
Unit 1: Measurement
1. A block of sodium with measurements 4.00 cm x 3.00 cm x 6.25 cm has a measured mass of 76.1 g. The accepted
density for sodium if 0.971 g/cm3. Calculate the percent error.
2. A 49.5 gram sample of tin at 95.0°C is placed into 145 grams of water. The water and tin reach thermal equilibrium
at a temperature of 26.1°C. What was the initial temperature of the water?
a. 22.4 °C
b. 24.9 °C
c. 27.3 °C
d. 29.8 °C
3. If 145 J of heat are added to an unknown metal of mass 121 g, the temperature of the metal goes from 22.2°C to
24.3°C. Calculate the specific heat of the metal.
Unit 2: Matter & Energy
4. Benzene, C6H6, boils at 80.1˚C and has a density of 0.877 g/cm3. Determine the quantity of heat that is required to
vaporize a 45.6 mL sample of benzene at 35.0˚C.
a. 3140 J
b. 4370 J
c. 15800 J
d. 18900 J
5. If a gas’s temperature increases, what happens to the pressure and volume?
a. Pressure increases and volume increases
c. Pressure decreases and volume increases
b. Pressure decreases and volume decreases
d. Pressure increases and volume decreases
7. Which of the following occurs during a phase change?
a. Temperature increases
b. Kinetic energy increases
c. Heat energy increases
d. All of the above
8. Which lettered region represents the phase with the highest
intermolecular forces?
a. A
b. B
c. C
d. D
e. E
Increasing Temperature
6. A gas is collected over water in a eudiometer tube until the pressure is equilibrated with the atmospheric pressure.
The volume of gas in the eudiometer is 28.5 mL. The temperature of the water is 36.0°C and the barometric pressure
is 758 mm Hg. What is the volume of this gas at STP?
a. 23.6 mL
b. 25.1 mL
c. 30.3 mL
d. 32.2 mL
D
C
B
A
Time
9. A balloon is filled to a volume of 745 mL with 158 grams of steam at 112°C. After a brief period of cooling, the
balloon’s volume is measured to be 735 mL. How much heat energy did the steam lose?
E
Unit 3: Atomic Theory & Nuclear
10. Complete the following chart:
Isotopic
Symbol
Isotope Name
Atomic
Number
Mass
Number
# protons
# electrons
# neutrons
16
8O
a
b
manganese-56
11. If samples of two different elements each represent one mole, then
a. they are equal in mass.
b. they contain the same number of atoms
c. their molar masses are equal
d. they have the same atomic mass
12. Calculate the number of atoms in 10.0 g of aluminum.
13.
Determine the mass in grams of 5.00 x 1023 mol of oxygen atoms.
14. Write balanced nuclear equations for the following:
a. Alpha-particle bombardment of plutonium-239 produces a neutron and another isotope.
b. With what particle would you bombard sulfur-32 with to produce hydrogen-1 and phosphorus-32?
15. A 900. mg sample of platinum-197 is found to have a mass of 56.3 mg after exactly 3 days. What is the half-life of
platinum-197 in hours?
a. 24 hrs
b. 18 hrs
c. 0.75 hrs
d. 16 hrs
Unit 4: Chemical Compounds
16. Write the name if given the formula or the formula if given the name.
a. HBr(aq)
_____________________________
m. Ga2(WO3)3 _____________________________
b. Cu2C2O4
_____________________________
n. molybdous acid ___________________________
c. Cl2O7
_____________________________
o. calcium phosphate _________________________
d. Al(ClO4)3
_____________________________
p. arsenic triiodide ___________________________
q. magnesium sulfate heptahydrate ______________
e. Fe(NO3)3 • 9H2O ___________________________
r. iron(III) carbonate _________________________
f. SO3
_____________________________
g. HNO2 (aq)
_____________________________
t. manganese(IV) telluride ____________________
h. Pb(Cr2O7)2
_____________________________
u. scandium arsenite _________________________
i. N2O5
_____________________________
v. tetraphosphorous decoxide ___________________
j. H3BO2 (aq)
_____________________________
k. SnBr4
_____________________________
l. Ti(IO)3
_____________________________
s. sodium acetate
___________________________
w. phosphorous acid ________________________
x. hydroselenic acid __________________________
y. acetic acid
______________________________
z. platinum(II) perbromate _____________________
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17. Determine the percent composition of manganese(VII) arsenate.
18. How many electrons are present in a 20.54 gram sample of calcium ions?
19. What mass of aluminum hypochlorite contain 1.574 x 1023 hypochlorite ions?
20. An unknown gas has an effusion rate that is 0.845 times that of dinitrogen pentoxide. What is the molar mass of the
unknown gas?
Unit 5: Mole
21. The following pertains to the compound, potassium hypomolybdite.
a. Calculate the mass of oxygen in potassium hypomolybdite if there are 3.91x1024 formula units.
b. Calculate the total number of ions in 154.3 g of potassium hypomolybdite.
c. Calculate the mass of potassium hypomolybdite needed to make 250. mL of a 0.500 M solution.
22. An unknown gas was collected over water. Determine the molar mass of the unknown gas if a 0.167 g sample
occupies a volume of 69.8 mL at 60.0°C. The barometric pressure is 752.8 torr.
23. An unknown gas is determined to have an empirical formula of CH2. If a 0.176 g sample of this gas occupies a
volume of 35.0 mL at 134 kPa and 175°C, determine its molecular formula.
24. 123g of sucrose is dissolved in 568g of water. The solution has a density of 1.34g/ mL. Determine the molarity and
molality of the solution.
25. A compound is found to be 47.1% carbon, 6.54%H, and 46.4% chlorine. The rate of effusion of this compound in the
gaseous state was measured relative to oxygen gas. Nitrogen was found to effuse at rate that was 2.34 times faster
than this compound. Determine the molecular formula of the compound.
Unit 6: Chemical Equations
26. Calculate ∆H for the reaction 2Al (s) + 3Cl2 (g)  2AlCl3 (s) from the data.
2Al (s) + 6 HCl (aq) →2 AlCl3 (aq) + 3 H2 (g)
HCl (aq) →HCl (g)
2 H2 (g) + 2 Cl2 (g) → 4 HCl (g)
AlCl3 (s) →AlCl3 (aq)
∆H = -1049.0 kJ
∆H = +74.8 kJ
∆H = -3690.0 kJ
∆H = -323.0 kJ
27. Using bond energies, calculate the enthalpy change for the following reactions:
28. Using bond energies, calculate molar heat of combustion for 1 mole of methane (CH4):
3
29. Write complete balanced chemical equations. Indicate precipitate for double replacement reactions.
a.
b.
c.
d.
e.
f.
g.
h.
i.
j.
k.
l.
m.
n.
Zinc carbonate decomposes.
Strontium is mixed with chlorine gas.
Combustion of octane.
Iron is added to acetic acid.
Potassium oxide is mixed with water.
Lithium chlorate decomposes.
Potassium hydroxide is added to sulfuric acid.
Sulfur trioxide is bubbled through water.
Zinc is dropped into hydrochloric acid.
Decomposition of calcium oxide.
Gold metal dropped into sulfurous acid.
Silver nitrate is added to ammonium phosphate.
Fluorine is added to sodium bromide.
Carbonic acid is heated.
Unit 7: Stoichiometry
30. Given the reaction of propane (C3H8) burning in air, how many grams of oxygen gas are required to burn 3.01 1023
propane molecules?
a. 80.0 g
b. 40.0 g
c. 160 g
d. 16.0 g
e. 64.0 g
31. The following statements apply to the interpretation of chemical equations. Not all of the statements are true.
Which response includes all of the true statements, and no others?
I.
The sum of the number of moles of the reactants must equal the sum of the number
of moles of products in a balanced equation.
II.
The sum of the number of grams of the reactants that react must equal the sum of
the number of grams of the products produced by the reaction.
III. The following equation for the reaction involving hypothetical substances, A, B, C,
and D, implies that the products C and D are always produced in a three to one
mole ratio. A + 2B  3C + D
IV. The equation shown in III implies that in any reaction involving A and B as
reactants, A must be the limiting reactant.
V. The total number of atoms in the reactants that react must always equal the total
number of atoms in the products produced by the reaction.
a. I and V
b. I, II, and III
c. II, IV, and V
d. II, III, and V
e. III, IV, and V
32. The thermite reaction is performed using 8.6 g iron(III) oxide and 1.8 g powdered aluminum metal. Which
reactant is in excess and by how much?
a. Al, 0.3 g
b. Fe2O3, 2.0 g
c. Al, 2.1 g
d. Al, 1.1 g
e. Fe2O3, 3.3 g
33. Suppose 600. g of phosphorus reacts with 1300. g of sulfur in a synthesis reaction. How many grams of
tetraphosphorus decasulfide can be produced, assuming an 80.0% yield for the reaction
a. 4.62x102 g
b. 1.44x103 g
c. 2.16x103g
d. 4.92x103g
e. 6.50x102g
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34. Sulfuric acid can be produced by a three step process. First, sulfur is burned in air to give sulfur dioxide.
Second, the sulfur dioxide is converted to sulfur trioxide by passing the sulfur dioxide over a catalyst in the
presence of oxygen at a high temperature. Third, the sulfur trioxide is reacted with water to form sulfuric acid.
What mass of sulfuric acid would be formed from 1.00 x 103 kg of sulfur, if the three steps gave yields as listed
below?
S + O2 → SO2
92.5%
2SO2 + O2 → 2SO3
72.6%
SO3 + H2O → H2SO4
98.2%
a. 4.03 x 103 kg
b. 2.02 x 103 kg
c. 3.06 x 103kg
d. 2.84 x 103kg
35. What mass of a 25.0% barium nitrate solution contains 40.0 grams of barium nitrate?
a. 117 g
b. 160 g
c. 321 g
d. 10.0 g
e. 2.22 x 103kg
e. 62.5 g
36. If 45.0 mL of 0.250 M lead(IV) chloride solution reacts with 20.0 mL of ammonium sulfate, what is the
molarity of the ammonium sulfate solution?
a. 0.502 M
b. 1.25 M
c. 2.25 M
d. 1.13 M
e. 0.563 M
37. What mass of calcium carbonate is required to react with 100. mL of a 2.00 M hydrochloric acid solution?
a. 5.00 g
b. 10.0 g
c. 15.0 g
d. 20.0 g
e. 23.0 g
38. What volume of 0.0750M barium hydroxide will completely react with 125 mL of 0.0350M hydrochloric acid?
a. 29.2 mL
b. 42.0 mL
c. 230. mL
d. 536 mL
e. 53.6 mL
39. What is the molarity of a sulfurous acid solution if 23.7 mL of this solution requires 16.8 mL of 0.296M sodium
hydroxide for titration to its endpoint?
a. 0.210 M
b. 0.358 M
c. 0.105 M
d. 0.421 M
e. 0.0525 M
40. How much heat is evolved in the formation of 35.0 grams of iron(III) oxide from its elements at 25°C and 1.00
atm pressure?
a. 90.4 kJ
b. 180.7 kJ
c. 151 kJ
d. 360.1 kJ
e. 243. 9 kJ
Unit 8: Electrons
41. Calculate and determine the type of EMR:
a.
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the energy of a photon with a frequency of 8.77x10 s−1 b. the frequency of a photon with an energy of 1.88x10 −25 J.
42. Write the shortened configuration and orbital notation for Cadmium.
43. What is the total number of electrons that will be in p orbitals in 8.31 moles of ground state zinc atoms?
44. In the hydrogen atom, the energy associated with the fifth energy level is −8.72x10−20 J while the energy of the first
energy level is −2.18x10−18 J.
a. Calculate the energy change from n=5 to n=1?
B. Calculate the wavelength of the emitted photon?
45. Which of the following colors has the highest frequency?
a. blue
b. red
c. violet
d. yellow
46. Which of the following has the longest wavelength?
a. U.V.
b. I.R.
c. X-ray
d. gamma
47. An 18.36 g sample of hydrogen cyanide gas (C = 1.328 J/g•°C) is at STP in a 5.00 L expandable container. When
1.609 x 1021 photons of light with a wavelength of 945Å are added to the gas, the pressure of the gas changes to 1168
torr. What is the new volume of the gas after the addition of the photons?
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Unit 9: Bonding
48. Draw the Lewis dot structure for strontium nitride.
49. By use of electronegativity, identify each of the following bonds as: nonpolar, polar covalent, or ionic.
CH4
H2O
RbI
O2
50. How many single bonds are present in 6.93 x 1024 molecules of perchloric acid?
51. Draw the electron geometry, molecular geometry and bond angle for the carbonate ion?
52. Complete the following table using your knowledge of Lewis Structures and VSEPR theory.
Lewis Structure
Structural Formula
(indicate polarity)
electron
geometry
bond
angle
molecular
geometry
CH2Cl2
H2S
BF3
NF3
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Unit 10: Solutions
53. Consider the three statements below. Which numbered response contains all the statements that are true and no false
statements?
I.
Hydration is a special case of solvation in which the solvent is water.
II.
The oxygen end of water molecules is attracted toward Ca2+ ions.
III. The hydrogen end of water molecules is attracted toward Cl- ions.
a. I
b. II
c. III
d. I and II
e. I, II, and III
54. Which of the following solutions would not be expected to exist?
a. NaCl in CCl4 (a nonpolar solvent)
d. Methyl alcohol, CH3OH, in water
b. NaCl in water
e. Vegetable oil in mineral oil
c. Pentane, C5H12, in CCl4
55. Calculate the molality of a solution that contains 25 g of H2SO4 dissolved in 80. g of H2O.
a. 1.6 m
b. 2.2 m
c. 3.2 m
d. 6.3 m
e. 7.0 m
56. Calculate the molality of a 10.0% phosphoric acid solution in water.
a. 0.380 m
b. 0.760 m
c. 1.13 m
e. 1.89 m
d. 1.51 m
57. Which aqueous solution would have the lowest vapor pressure at 25 C?
a. 1 M NaCl
d. 1 M MgCl2
b. 1 M Na3PO4
e. 1 M glucose, C6H12O6
c. 1M sucrose, C12H10O11
58. If 4.27 grams of sucrose, C12H22O11, are dissolved in 15.2 grams of water, what will be the boiling point of the
resulting solution?
a. 101.64C
b. 100.42C
c. 99.626C
d. 100.73C
e. 101.42C
59. Which of the following statements regarding a 1 M sucrose solution is not correct?
a. The boiling point is greater than 100C.
b. The freezing point is less than that of a 1 M NaCl solution.
c. The freezing point is less than 0.0C.
d. The boiling point is less than that of a 1 M NaCl solution.
e. The vapor pressure at 100C is less than 760 torr.
60. When 35.0 g of an unknown nonelectrolyte is dissolved in 220.0 g of benzene, the solution boils at 83.2C.
Calculate the molecular weight of the unknown nonelectrolyte. The Kb for benzene = 2.53C/m. The boiling point
of pure benzene is 80.1C.
a. 130 g/mol
b. 20.3 g/mol
c. 183 g/mol
d. 156 g/mol
e. 194 g/mol
61. The following describe properties of substances. Which one is not a property of acids?
a. They have a sour taste.
d. Their aqueous solutions conduct an electric current.
b. They react with metal oxides to form salts and water.
e. They react with active metals to liberate H2.
c. They react with other acids to form salts and water.
62. Which of the following is not a common property of aqueous solutions of most bases?
a. They have a bitter taste.
b. They have a slippery feeling.
c. They change the colors of many indicators.
d. They react with protonic acids to form salts and stronger bases.
e. Their aqueous solutions conduct an electric current.
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63. According to the Arrhenius theory, which of the following is an acid?
a. NH3
b. CH4
c. HCl
d. H2
64. Which one of the following species could not react as a Brønsted-Lowry acid?
a. HCl
b. H2O
c. CaO
d. NH3
65. Which of the following does not represent a conjugate acid-base pair?
a. H2O/OHb. H3O+/OHc. HCl/Cl66. A solution having a pH of 1.4 would be described as __________.
a. distinctly basic
b. slightly basic
c. neutral
67. In the equation:
HF + H2O
H3O+ + Fa. H2O is a base, and HF is its conjugate acid.
b. H2O is an acid, and HF is the conjugate base.
c. HF is an acid, and F- is its conjugate base.
d. HNO3/NO3-
d. slightly acidic
e. NaOH
e. CH3COOH
e. NH4+/NH3
e. distinctly acidic
d. HF is a base, and H3O+ is its conjugate acid.
e. HF is a base, and F- is its conjugate acid.
68. Which of the following reactions is the net ionic equation for the acid-base reaction between H2CO3 and Sr(OH)2?
a. H2CO3 + Sr2+ + 2 OH-  SrCO3 + 2 H2O
d. H2CO3 + 2 OH-  2 H2O+ CO32b. H3O+ + OH-  2 H2O
e. H2CO3 + Sr(OH)2 2H2O+ Sr2+ + CO32+
2+
2+
c. 2 H3O + Sr + 2 OH  Sr + 4 H2O
69. The molar concentration of the Ca2+ ion is ________ and the molar concentration of OH- ion is ________ in 0.015
M calcium hydroxide.
a. 0.015 M; 0.015 M
d. 0.030 M; 0.030 M
b. 0.015 M; 0.030 M
e. not enough information to calculate
c. 0.030 M; 0.015 M
70. Calculate the pH of a solution in which [OH-] = 2.50  10-4 M.
a. 0.40
b. 3.60
c. -3.60
d. 10.40
e. 13.60
71. What is the concentration of H3O+ ions in a solution in which pH = 4.32?
a. 4.8  10-5 M
b. 6.2  10-4 M
c. 5.1  10-4 M
d. 8.6  10-5 M
e. 3.5  10-4 M
72. What is the pH of 500. mL of solution containing 0.0124 gram of calcium hydroxide?
a. 2.96
b. 3.17
c. 9.68
d. 10.83
e. 11.04
73. A laboratory stock solution is 1.50 M sodium hydroxide. Calculate the volume of this stock solution that would be
needed to prepare 300. mL of 0.200 M sodium hydroxide.
a. 2.25 mL
b. 10.0 mL
c. 40.0 mL
d. 1.00 mL
e. 0.100 mL
74. When a solution is diluted, what is the relationship of the number of moles of solute in the more concentrated
initial volume of solution to the number of moles of solute in the less concentrated final volume of solution?
a. The ratio of the numbers is directly proportional to the two volumes.
b. The ratio of the numbers is inversely proportional to the two volumes.
c. The number of moles of solute in the more concentrated initial volume is always greater.
d. The number of moles of solute in the less concentrated final volume is always greater.
e. The number of moles of solute in both solutions is the same.
75. Calculate the molarity of the resulting solution if 25.0 mL of 2.40 M sulfuric acid solution is diluted to 300.mL.
a. 0.200 M
b. 29.0 M
c. 2.00 M
d. 0.400 M
e. 0.0400 M
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