Download Use the following answers for questions 1

AP MULTIPLE CHOICE PROBLEMS
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QUESTION
4. Use the following answers for questions 4 - 7.
(A) Hydrofluoric acid
(B) Carbon dioxide
(C) Aluminum hydroxide
(D) Ammonia
(E) Hydrogen peroxide
4. Is a good oxidizing agent
5. Is used to etch glass chemically
6. Is used extensively for the production of fertilizers
7. Has amphoteric properties
63. Which of the following characteristics is common to elemental sulfur, chlorine,
nitrogen, and carbon?
(A) They are gaseous elements at room temperature.
(B) They have oxides that are acid anhydrides.
(C) They have perceptible color at room temperature.
(D) They form ionic oxides.
(E) They react readily with hydrogen at room temperature.
64. A solution is known to contain an inorganic salt of one of the following elements.
The solution is colorless. The solution contains a salt of
(A) Cu
(B) Mn
(C) Fe
(D) Ni
(E) Zn
11. Questions 11-13
(A) Pb
(B) Ca
(C) Zn
(D) As
(E) Na
11. Utilized as a coating to protect Fe from corrosion
12. Is added to silicon to enhance its properties as a semiconductor
13. Utilized as a shield from sources of radiation
1. Questions 1-4 refer to the following types of energy.
(A) Activation energy
(B) Free energy
(C) Ionization energy
(D) Kinetic energy
(E) Lattice energy
1. The energy required to convert a ground-state atom in the gas phase to a
gaseous positive ion
2. The energy change that occurs in the conversion of an ionic solid to widely
separated gaseous ions
3. The energy in a chemical or physical change that is available to do useful work
4. The energy required to form the transition state in a chemical reaction
Kim Duncan
Upper School Science Teacher
Flint Hill School
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AP MULTIPLE CHOICE PROBLEMS
59. When 70. milliliter of 3.0-molar Na2CO3 is added to 30. milliliters of 1.0-molar
NaHCO3 the resulting concentration of Na+ is
(A) 2.0 M
(B) 2.4 M
(C) 4.0 M
(D) 4.5 M
(E) 7.0 M
67. A student wishes to prepare 2.00 liters of 0.100-molar KIO3 (molecular weight
214). The proper procedure is to weigh out
(A) 42.8 grams of KIO3 and add 2.00 kilograms of H2O
(B) 42.8 grams of KIO3 and add H2O until the final homogeneous solution has a
volume of 2.00 liters
(C) 21.4 grams of KIO3 and add H2O until the final homogeneous solution has a
volume of 2.00 liters
(D) 42.8 grams of KIO3 and add 2.00 liters of H2O
(E) 21.4 grams fo KIO3 and add 2.00 liters of H2O
68. A 20.0-milliliter sample of 0.200-molar K2CO3 solution is added to 30.0
milliliters of 0.400-molar Ba(NO3)2 solution. Barium carbonate precipitates. The
concentration of barium ion, Ba2+, in solution after reaction is
(A) 0.150 M
(B) 0.160 M
(C) 0.200 M
(D) 0.240 M
(E) 0.267 M
69. What is the mole fraction of ethanol, C2H5OH, in an aqueous solution in which the
ethanol concentration is 4.6 molal?
(A) 0.0046
(B) 0.076
(C) 0.083
(D) 0.20
(E) 0.72
15. The weight of H2SO4 (molecular weight 98.1) in 50.0 milliliters of a 6.00-molar
solution is
(A) 3.10 grams
(B) 12.0 grams
(C) 29.4 grams
(D) 294 grams
(E) 300. grams
26. How many milliliters of 11.6-molar HCl must be diluted to obtain 1.0 liter of 3.0molar HCl?
(A) 3.9 mL
(B) 35 mL
(C) 260 mL
(D) 1,000 mL
(E) 3,900 mL
Kim Duncan
Upper School Science Teacher
Flint Hill School
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AP MULTIPLE CHOICE PROBLEMS
A 43. Which of the following does NOT behave as an electrolyte when it is dissolved in
water?
(A) CH3OH
(B) K2CO3
(C) NH4Br
(D) HI
(E) Sodium acetate, CH3COONa
A 72. How many moles of solid Ba(NO3)2 should be added to 300. milliliters of 0.20molar Fe(NO3)3 to increase the concentration of the NO3¯ ion to 1.0-molar? (Assume
that the volume of the solution remains constant.)
(A) 0.060 mole
(B) 0.12 mole
(C) 0.24 mole
(D) 0.30 mole
(E) 0.40 mole
E 28. Given that a solution is 5 percent sucrose by mass, what additional information is
necessary to calculate the molarity of the solution?
I. The density of water
II. The density of the solution
III. The molar mass of sucrose
(A) I only
(B) II only
(C) III only
(D) I and III
(E) II and III
D 47. Which of the following has the lowest conductivity?
(A) 0.1 M CuS04
(B) 0.1 M KOH
(C) 0.1 M BaCl2
(D) 0.1 M HF
(E) 0.1 M HNO3
E 53. If 87 grams of K2 SO4 (molar mass 174 grams) is dissolved in enough water to
make 250 milliliters of solution, what are the concentrations of the potassium and the
sulfate ions?
[K+]
[SO42¯]
(A) 0.020 M
0.020 M
(B) 1.0 M
2.0 M
(C) 2.0 M
1.0 M
(D) 2.0 M
2.0 M
(E) 4.0 M
2.0 M
Kim Duncan
Upper School Science Teacher
Flint Hill School
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AP MULTIPLE CHOICE PROBLEMS
33. A 1.0 sample of an aqueous solution contains 0.10 mol of NaCl and 0.10 mol of
CaCl2. What is the minimum number of moles of AgNO3 that must be added to the
solution in order to precipitate all of the Cl¯ as AgCl(s) ? (Assume that AgCl is
insoluble.)
(A) 0.10 mol
(B) 0.20 mol
(C) 0.30 mol
(D) 0.40 mol
(E) 0.60 mol
56. A yellow precipitate forms when 0.5 M NaI(aq) is added to a 0.5 M solution of
which of the following ions?
A) Pb2+(aq)
B) Zn2+(aq)
C) CrO42¯(aq)
D) SO42¯(aq)
E) OH¯(aq)
59. A 40.0 mL sample of 0.25 M KOH is added to 60.0 mL of 0.15 M Ba(OH)2.
What is the molar concentration of OH¯(aq) in the resulting solution? (Assume that the
volumes are additive)
A) 0.10 M
B) 0.19 M
C) 0.28 M
D) 0.40 M
E) 0.55 M
69. What is the final concentration of barium ions, [Ba2+], in solution when 100. mL of
0.10 M BaCl2(aq) is mixed with 100. mL of 0.050 M H2SO4(aq)?
A) 0.00 M
B) 0.012 M
C) 0.025 M
D) 0.075 M
E) 0.10 M
70. When 100 mL of 1.0 M Na3PO4 is mixed with 100 mL of 1.0 M AgNO3, a
yellow precipitate forms and [Ag+] becomes negligibly small. Which of the following
is a correct listing of the ions remaining in solution in order of increasing
concentration?
A) [PO43¯] < [NO3¯] < [Na+]
B) [PO43¯] < [Na+]<[NO3¯]
C) [NO3¯] < [PO43¯] < [Na+]
D) [Na+] < [NO3¯] < [PO43¯]
E) [Na+] < [PO43¯] < [NO3¯]
71. In a qualitative ananlysis for the presence of Pb2+, Fe2+, and Cu2+ ions in a
aqueous solution, which of the following will allow the separation of Pb2+ from the
other ions at room temperature?
A) Adding dilute Na2S(aq) solution
B) Adding dilute HCl(aq) solution
C) Adding dilute NaOH(aq) solution
D) Adding dilute NH3(aq) solution
E) Adding dilute HNO3(aq) solution
Kim Duncan
Upper School Science Teacher
Flint Hill School
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AP MULTIPLE CHOICE PROBLEMS
73. The volume of distilled water that should be added to 10.0 mL of 6.00 M
HCl(aq) in order to prepare a 0.500 M HCl(aq) solution is approximately
A) 50.0 mL
B) 60.0 mL
C) 100. mL
D) 110. mL
E) 120. mL
21. When a sample of oxygen gas in a closed container of constant volume is
heated until its absolute temperature is doubled, which of the following is also
doubled?
(A) The density of the gas
(B) The pressure of the gas
(C) The average velocity of the gas molecules
(D) The number of molecules per cm3
(E) The potential energy of the molecules
23. The density of an unknown gas is 4.20 grams per liter at 3.00 atmospheres
pressure and 127 °C. What is the molecular weight of this gas? (R = 0.0821 literatm / mole-K)
(A) 14.6
(B) 46.0
(C) 88.0
(D) 94.1
(E) 138
39. Equal masses of three different ideal Gas, X, Y, and Z, are mixed in a sealed
rigid container. If the temperature of the system remains constant, which of the
following statements about the partial pressure of gas X is correct?
(A) It is equal to 1/3 the total pressure
(B) It depends on the intermolecular forces of attraction between molecules of X, Y,
and Z.
(C) It depends on the relative molecular masses of X, Y, and Z.
(D) It depends on the average distance traveled between molecular collisions.
(E) It can be calculated with knowledge only of the volume of the container.
50. Two flexible containers for Gas are at the same temperature and pressure. One
holds 0.50 gram of hydrogen and the other holds 8.0 grams of oxygen. Which of
the following statements regarding these gas samples is FALSE?
(A) The volume of the hydrogen container is the same as the volume of the oxygen
container.
(B) The number of molecules in the hydrogen container is the same as the number of
molecules in the oxygen container.
(C) The density of the hydrogen sample is less than that of the oxygen sample.
(D) The average kinetic energy of the hydrogen molecules is the same as the
average kinetic energy of the oxygen molecules.
(E) The average speed of the hydrogen molecules is the same as the average speed
of the oxygen molecules.
Kim Duncan
Upper School Science Teacher
Flint Hill School
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AP MULTIPLE CHOICE PROBLEMS
52. 3 Ag(s) + 4 HNO3 <===> 3 AgNO3 + NO(g) + 2 H2O
The reaction of silver metal and dilute nitric acid proceeds according to the equation
above. If 0.10 mole of powdered silver is added to 10. milliliters of 6.0-molar nitric
acid, the number of moles of NO gas that can be formed is
(A) 0.015 mole
(B) 0.020 mole
(C) 0.030 mole
(D) 0.045 mole
(E) 0.090 mole
72. A compound is heated to produce a gas whose molecular weight is to be
determined. The gas is collected by displacing water in a water-filled flask inverted
in a trough of water. Which of the following is necessary to calculate the molecular
weight of the gas, but does NOT need to be measured during the experiment?
(A) Mass of the compound used in the experiment
(B) Temperature of the water in the trough
(C) Vapor pressure of the water
(D) Barometric pressure
(E) Volume of water displaced from the flask
78. When the actual gas volume is greater then the volume predicted by the ideal
gas law, the explanation lies in the fact that the ideal gas law does NOT include a
factor for molecular.
(A) volume
(B) mass
(C) velocity
(D) attractions
(E) shape
85. A sample of 9.00 grams of aluminum metal is added to an excess of
hydrochloric acid. The volume of hydrogen gas produced at standard temperature
and pressure is
(A) 22.4 liters
(B) 11.2 liters
(C) 7.46 liters
(D) 5.60 liters
(E) 3.74 liters
16. A gaseous mixture containing 7.0 moles of nitrogen, 2.5 moles of oxygen, and
0.50 mole of helium exerts a total pressure of 0.90 atmosphere. What is the partial
pressure of the nitrogen?
(A) 0.13 atm
(B) 0.27 atm
(C) 0.63 atm
(D) 0.90 atm
(E) 6.3 atm
24. A sample of 0.010 mole of oxygen gas is confined at 127 °C and 0.80
atmosphere. What would be the pressure of this sample at 27 °C and the same
volume?
(A) 0.10 atm
(B) 0.20 atm
(C) 0.60 atm
(D) 0.80 atm
(E) 1.1 atm
Kim Duncan
Upper School Science Teacher
Flint Hill School
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AP MULTIPLE CHOICE PROBLEMS
30. Hydrogen gas is collected over water at 24 °C. The total pressure of the sample
is 755 millimeters of mercury. At 24 °C, the vapor pressure of water is 22 millimeters
of mercury. What is the partial pressure of the hydrogen gas?
(A) 22 mm Hg
(B) 733 mm Hg
(C) 755 mm Hg
(D) 760 mm Hg
(E) 777 mm Hg
32. A 2.00-liter sample of nitrogen gas at 27 °C and 600. millimeters of mercury is
heated until it occupies a volume of 5.00 liters. If the pressure remains unchanged,
the final temperature of the gas is
(A) 68 °C
(B) 120 °C
(C) 477 °C
(D) 677 °C
(E) 950. °C
40. 2 K + 2 H2O ---> 2 K+ + 2 OH¯ + H2 When 0.400 mole of potassium reacts
with excess water at standard temperature and pressure as shown in the equation
above, the volume of hydrogen gas produced is
(A) 1.12 liters
(B) 2.24 liters
(C) 3.36 liters
(D) 4.48 liters
(E) 6.72 liters
62. As the temperature is raised from 20 ° C to 40 ° C, the average kinetic energy
of neon atoms changes by a factor of
(A) 1/2
(B) [square root of](313/293)
(C) 313/293
(D) 2
(E) 4
24. A sample of 0.0100 mole of oxygen gas is confined at 37° C and 0.216
atmosphere. What would be the pressure of this sample at 15° C and the same
volume?
(A) 0.0876 atm
(B) 0.175 atm
(C) 0.201 atm
(D) 0.233 atm
(E) 0.533 atm
33. A hydrocarbon gas with an empirical formula CH2 has a density of 1.88 grams
per liter at 0 °C and 1.00 atmosphere. A possible formula for the hydrocarbon is
(A) CH2
(B) C2H4
(C) C3H6
(D) C4H8
(E) C5H10
Kim Duncan
Upper School Science Teacher
Flint Hill School
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AP MULTIPLE CHOICE PROBLEMS
37R. A sample of 3.0 grams of an ideal gas at 121 °C and 1.0 atmosphere pressure
has a volume of 1.0 Iiters. Which of the following expressions is correct for the molar
mass of the gas? The ideal gas constant, R, is 0.08 (L-atm) / (mole K).
(A) [(0.08)(400)] / [(3.0)(1.0)(1.5)]
(B) [(l.O)(l.5)] / [(3.0)(0.08)(400)]
(C) [(O.O8)(1.0)(1.5)] / [(3.0)(400)]
(D) [(3.0)(0.08)(400)] / [(1.0)(1.5)]
(E) [(3.0)(0.08)(1.5)] / (1.0)(400)]
39. Samples of F2 gas and Xe gas are mixed in a container of fixed volume. The
initial partial pressure of the F2 gas is 8.0 atmospheres and that of the Xe gas is 1.7
atmospheres. When all of the Xe gas reacted, forming a solid compound, the
pressure of the unreacted F2 gas was 4.6 atmospheres. The temperature remained
constant. What is the formula of the compound?
(A) XeF
(B) XeF3
(C) XeF4
(D) XeF6
(E) XeF8
40. The system shown above is at equilibrium at 28
°C. At this temperature, the vapor pressure of
water is 28 millimeters of mercury. The partial
pressure of O2(g) in the system is
(A) 28 mm Hg
(B) 56 mm Hg
(C) 133 mm Hg
(D) 161 mm Hg
(E) 189 mm Hg
45. A sample of an ideal gas is cooled from 50.0 °C to 25.0 °C in a sealed
container of constant volume. Which of the following values for the gas will
decrease?
I. The average molecular mass of the gas
II. The average distance between the molecules
III. The average speed of the molecules
(A) I only
(B) II only
(C) III only
(D) I and III
(E) II and III
64. At 25 °C, a sample of NH3 (molar mass 17 grams) effuses at the rate of 0.050
mole per minute. Under the same conditions, which of the following Gas effuses at
approximately one-half that rate?
(A) O2 (molar mass 32 grams)
(B) He2 (molar mass 4.0 grams)
(C) CO2 (molar mass 44 grams)
(D) Cl2 (molar mass 71 grams)
(E) CH4 (molar mass 16 grams)
Kim Duncan
Upper School Science Teacher
Flint Hill School
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AP MULTIPLE CHOICE PROBLEMS
52. Under which of the following sets of
Pressure of O2(g)
Temperature of
conditions could the most O2(g) be
Above H2O(l) (atm) H2O(l) °(C)
dissolved in H2O(l)?
A) 5.0
80
B) 5.0
20
C) 1.0
80
D) 1.0
20
E) 0.5
20
23. A hot-air balloon, shown right, rises. Which of the following is the
best explanation for this observation?
(A) The pressure on the walls of the balloon increases with increasing
tempearature.
(B) The difference in temperature between the air inside and outside
the ballon produces convection currents.
(C) The cooler air outside the balloon pushes in on the walls of the
ballon.
(D) The rate of diffusion of cooler air is less than that of warmer air.
(E) The air density inside the ballon is less than that of the surrounding air.
44. A rigid metal tank contains oxygen gas. Which of the following applies to the
gas in the tank when additional oxygen is added at constant temperature?
(A) The volume of the gas increase.
(B) The pressure of the gas decreases.
(C) The average speed of the gas molecules remains th same.
(D) The total number of gas molecules remains the same.
(E) The average distance between the gas molecules increases.
53. W(g) + X(g) --> Y(g) + Z(g) Gas W and X react in a closed, rigid vessel to
form Gas Y and Z according to the equation above. The initial pressure of W(g) is
1.20 atm and that of X(g) is 1.60 atm. No Y(g) or Z(g) is initially present. The
experiment is carried out at constant temperature. What is the partial pressure of
Z(g) when the partial pressure of W(g) has decreased to 1.0 atm?
A) 0.20 atm
B) 0.40 atm
C) 1.0 atm
D) 1.2 atm
E) 1.4 atm
60. NH4NO3(s) --> N2O(g) + 2 H2O(g) A 0.03 mol sample of NH4NO3(s)
decomposes completely according to the balanced equation above. The total
pressure in the flask measured at 400 K is closest to which of the following? ( The
value of the gas constant,R, is 0.082 L atm mol¯1 K¯1)
(A) 3 atm
(B) 1 atm
(C) 0.5 atm
(D) 0.1 atm
(E) 0.03 atm
Kim Duncan
Upper School Science Teacher
Flint Hill School
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AP MULTIPLE CHOICE PROBLEMS
64. Equal numbers of moles of He(g), Ar(g), and Ne(g) are placed in a glass vessel
at room temperature. If the vessel has a pinhole-sized leak, which of the following
will be true regarding the relative values of the partial pressures of the Gas
remaining in the vessel after some of the gas mixture has effused?
A) PHe < PNe < PAr
B) PHe < PAr < PNe
C) PNe < PAr < PHe
D) PAr < PHe < PNe
E) PHe = PAr = PNe
74. Which of the following Gas deviates most from ideal behavior?
A) SO2
B) Ne
C) CH4
D) N2
E) H2
47. CH4(g) + 2 O2(g) ---> CO2(g) + 2 H2
- 889.1 kJ
°
H
O(l)
=
285.8
kJ
/
mole
f
2
f° CO2(g) = - 393.3 kJ / mole
f° CH4(g), as calculated
from the data above?
(A) -210.0 kJ/mole
(B) -107.5 kJ/mole
(C) -75.8 kJ/mole
(D) 75.8 kJ/mole
(E) 210.0 kJ/mole
48.Which of the following is a graph that describes the pathway of reaction that is
endothermic and has high activation energy?
A
B
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AP MULTIPLE CHOICE PROBLEMS
D 25R.
H2(g) + 1/2 O2(g) ---> H2O(l)
2 Na(s) + 1/2 O2(g) ---> Na2O(s)
Na(s) + 1/2 O2(g) + 1/2 H2(g) ---> NaOH(s)
Based on the information above, what is the standard enthalpy change for the
following reaction?
Na2O(s) + H2O(l) ---> 2 NaOH(s)
(A) x + y + z
(B) x + y - z
(C) x + y - 2z
(D) 2z - x - y
(E) z - x - y
D 30. The energy diagram for the
reaction X + Y ---> Z is shown
above. The addition of a catalyst
to this reaction would cause a
change in which of the indicated
energy differences?
(A) I only
(B) II only
(C) III only
(D) I and II only
(E) I, II, and III
C 19. Which of the following best describes the role of the spark from the spark plug
in an automobile engine?
(A) The spark decreases the energy of activation for the slow step.
(B) The spark increases the concentration of the volatile reactant.
(C) The spark supplies some of the energy of activation for the combustion reaction.
(D) The spark provides a more favorable activated complex for the combustion
reaction.
(E) The spark provides the heat of vaporization for the volatile hydrocarbon.
61. C2H4(g) + 3 O2(g) --> 2 CO2(g) + 2 H2O(g) For the reaction of ethylene
E
produced liquid water H2O (l), rather than water vapor H2
change H2O(g) --> H2O(l) is -44 kJ mol¯1.)
A) -1,235 kJ
B) -1,279 kJ
C) -1,323 kJ
D) -1,367 kJ
E) -1,411 kJ
E 22. 1s2 2s22p6 3s23p3 Atoms of an element, X, have the electronic configuration
shown above. The compound most likely formed with magnesium, Mg, is
(A) MgX
(B) Mg2X
(C) MgX2
(D) MgX3
(E) Mg3X2
Kim Duncan
Upper School Science Teacher
Flint Hill School
06
1
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9
4
06
TEST
Therm
06
1
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9
4
06
TEST
Therm
06
1
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06
TEST
Therm
1
9
9
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06
1
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8
4
07
06
TEST
Therm
07
TEST
Atomic
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E
A
D
E
B
E
B
A
E
D
AP MULTIPLE CHOICE PROBLEMS
43. The elements in which of the following have most nearly the same atomic radius?
(A) Be, B, C, N
(B) Ne, Ar, Kr, Xe
(C) Mg, Ca, Sr, Ba
(D) C, P, Se, I
(E) Cr, Mn, Fe, Co
58. Which of the following represents the ground state electron configuration for the
Mn3+ ion? (Atomic number Mn = 25)
(A) 1s2 2s22p6 3s23p63d4
(B) 1s2 2s22p6 3s23p63d5 4s2
(C) 1s2 2s22p6 3s23p63d2 4s2
(D) 1s2 2s22p6 3s23p63d8 4s2
(E) 1s2 2s22p6 3s23p63d3 4s1
66. Ca, V, Co, Zn, As
Gaseous atoms of which of the elements above are paramagnetic?
(A) Ca and As only
(B) Zn and As only
(C) Ca, V, and Co only
(D) V, Co, and As only
(E) V, Co, and Zn only
70. One of the outermost electrons in a strontium atom in the ground state can be
described by which of the following sets of four quantum numbers?
(A) 5, 2, 0, 1/2
(B) 5, 1, 1, 1/2
(C) 5, 1, 0, 1/2
(D) 5, 0, 1, 1/2
(E) 5, 0, 0, 1/2
Use the following answers for questions 1 - 3.
(A) F
(B) S
(C) Mg
(D) Ar
(E) Mn
1. Forms monatomic ions with 2¯ charge in solutions
2. Forms a compound having the formula KXO4
3. Forms oxides that are common air pollutants and that yield acidic solution in water
1. Use these answers for questions 1 - 3.
(A) O
(B) La
(C) Rb
(D) Mg
(E) N
1. What is the most electronegative element of the above?
2. Which element exhibits the greatest number of different oxidation states?
3. Which of the elements above has the smallest ionic radius for its most commonly
found ion?
Kim Duncan
Upper School Science Teacher
Flint Hill School
1
9
8
4
07
07
TEST
Atomic
1
9
8
4
07
07
TEST
Atomic
1
9
8
4
07
07
TEST
Atomic
1
9
8
4
07
07
TEST
Atomic
1
9
8
4
07
Basics
1
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8
9
07
07
TEST
Atomic
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A
C
E
B
B
C
E
B
A
C
D
AP MULTIPLE CHOICE PROBLEMS
33. Which of the following conclusions can be drawn from J. J. Thomson's cathode
ray experiments?
(A) Atoms contain electrons.
(B) Practically all the mass of an atom is contained in its nucleus.
(C) Atoms contain protons, neutrons, and electrons.
(D) Atoms have a positively charged nucleus surrounded by an electron cloud.
(E) No two electrons in one atom can have the same four quantum numbers.
4. Use these answers for questions 4 - 7.
(A) 1s2 2s22p5 3s23p5
(B) 1s2 2s22p6 3s23p6
(C) 1s2 2s22p62d10 3s23p6
(D) 1s2 2s22p6 3s23p63d5
(E) 1s2 2s22p6 3s23p63d3 4s2
4. An impossible electronic configuration
5. The ground-state configuration for the atoms of a transition element
6. The ground-state configuration of a negative ion of a halogen
7. The ground-state configuration of a common ion of an alkaline earth element
1. Questions 1-4
(A) Heisenberg uncertainty principle
(B) Pauli exclusion principle
(C) Hund's rule (principle of maximum multiplicity)
(D) Shielding effect
(E) Wave nature of matter
1. Can be used to predict that a gaseous carbon atom in its ground state is
paramagnetic
2. Explains the experimental phenomenon of electron diffraction
3. Indicates that an atomic orbital can hold no more than two electrons
4. Predicts that it is impossible to determine simultaneously the exact position and the
exact velocity of an electron
27. Which of the following sets of quantum numbers (n, l, ml, ms) best describes the
valence electron of highest energy in a ground-state gallium atom (atomic number
31) ?
(A) 4, 0, 0, 1/2
(B) 4, 0, 1, 1/2
(C) 4, 1, 1, 1/2
(D) 4, 1, 2, 1/2
(E) 4, 2, 0, 1/2
54. All of the following statements concerning the characteristics of the halogens are
true EXCEPT:
(A) The first ionization energies (potentials) decrease as the atomic numbers of the
halogens increase.
(B) Fluorine is the best oxidizing agent.
(C) Fluorine atoms have the smallest radii.
(D) Iodine liberates free bromine from a solution of bromide ion.
(E) Fluorine is the most electronegative of the halogens.
Kim Duncan
Upper School Science Teacher
Flint Hill School
1
9
8
9
07
Atomic
1
9
8
9
07
07
TEST
Atomic
1
9
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4
07
Atomic
1
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4
07
Atomic
07
07
TEST
Atomic
1
9
9
4
[email protected]
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D
A
C
E
D
E
C
A
E
E
AP MULTIPLE CHOICE PROBLEMS
5. Question 5-8 refer to atoms for which the
occupied atomic orbitals shown below.
5. Represents an atom that is chemically
unreactive
6. Represents an atom in an excited state
7. Represents an atom that has four valence electrons.
8. Represents an atom of a transition metal.
50. In the periodic table, as the atomic number increases from 11 to 17, what
happens to the atomic radius?
(A) It remains constant.
(B) It increases only.
(C) It increases, then decreases.
(D) It decreases only.
(E) It decreases, then increases.
51. Which of the following is a correct interpretation of the results of Rutherford's
experiments in which gold atoms were bombarded with alpha particles?
(A) Atoms have equal numbers of positive and negative charges.
(B) Electrons in atoms are arranged in shells.
(C) Neutrons are at the center of an atom.
(D) Neutrons and protons in atoms have nearly equal mass.
(E) The positive charge of an atom is concentrated in a small region.
37. The ionization energies for
Ionization Energies for element X (kJ mol¯1)
element X are listed in the table
First Second Third Fourth
Five
above. On the basis of the data,
580
1815 2740 11600 14800
element X is most likely to be
(A) Na
(B) Mg
(C) AI
(D) Si
(E) P
41. Which of the following molecules has the shortest bond length?
(A) N2
(B) O2
(C) Cl2
(D) Br2
(E) I2
51. Pi bonding occurs in each of the following species EXCEPT
(A) CO2
(B) C2H4
(C) CN¯
(D) C6H6
(E) CH4
60. Which of the following has a zero dipole moment?
(A) HCN
(B) NH3
(C) SO2
(D) NO2
(E) PF5
Kim Duncan
Upper School Science Teacher
Flint Hill School
1
9
9
9
07
07
TEST
Atomic
1
9
9
9
07
Atomic
1
9
9
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07
07
TEST
Atomic
1
9
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07
07
TEST
Atomic
1
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4
08
09
10
Bonds
1
9
8
4
08
09
10
Bonds
1
9
8
4
08
09
10
Bonds
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C
A
B
E
E
A
B
D
C
A
AP MULTIPLE CHOICE PROBLEMS
8. Use the following answers for questions 8 - 9.
(A) A network solid with covalent bonding
(B) A molecular solid with zero dipole moment
(C) A molecular solid with hydrogen bonding
(D) An ionic solid
(E) A metallic solid
8. Solid ethyl alcohol, C2H5OH
9. Silicon dioxide, SiO2
80. For which of the following molecules are resonance structures necessary to
describe the bonding satisfactorily?
(A) H2S
(B) SO2
(C) CO2
(D) OF2
(E) PF3
18. The liquefied hydrogen halides have the
Hydrogen Normal Boiling
normal boiling points given below. The relatively
Halide
Point, °C
high boiling point of HF can be correctly
HF
+19
explained by which of the followng?
HCl
- 85
(A) HF gas is more ideal.
(B) HF is the strongest acid.
HBr
- 67
(C) HF molecules have a smaller dipole moment.
HI
- 35
(D) HF is much less soluble in water.
(E) HF molecules tend to form hydrogen bonds.
11. Use these answers for questions 11 - 14.
(A) hydrogen bonding
(B) hybridization
(C) ionic bonding
(D) resonance
(E) van der Waals forces (London dispersion forces)
11. Is used to explain why iodine molecules are held together in the solid state
12. Is used to explain why the boiling point of HF is greater than the boiling point of
HBr
13. Is used to explain the fact that the four bonds in methane are equivalent
14. Is used to explain the fact that the carbon-to-carbon bonds in benzene, C6H6,
are identical
17. The Lewis dot structure of which of the following molecules shows only one
unshared pair of valence electron?
(A) Cl2
(B) N2
(C) NH3
(D) CCl4
(E) H2O2
31. The structural isomers C2H5OH and CH3OCH3 would be expected to have the
same values for which of the following? (Assume ideal behavior.)
(A) Gaseous densities at the same temperature and pressure
(B) Vapor pressures at the same temperature
(C) Boiling points
(D) Melting points
(E) Heats of vaporization
Kim Duncan
Upper School Science Teacher
Flint Hill School
1
9
8
4
08
09
10
Bonds
1
9
8
4
08
09
10
Bonds
1
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08
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Bonds
1
9
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08
09
10
Bonds
1
9
8
9
08
09
10
Bonds
1
9
8
9
08
09
10
Bonds
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D
C
E
E
D
E
AP MULTIPLE CHOICE PROBLEMS
42. The SbCl5 molecule has trigonal bipyramid structure. Therefore, the hybridization
of Sb orbitals should be
(A) sp2
(B) sp3
(C) dsp2
(D) dsp3
(E) d2sp3
47. CCl4, CO2, PCl3, PCl5, SF6 Which of the following does not describe any of the
molecules above?
(A) Linear
(B) Octahedral
(C) Square planar
(D) Tetrahedral
(E) Trigonal pyramidal
59. Which of the following compounds is ionic and contains both sigma and pi
covalent bonds?
(A) Fe(OH)3
(B) HClO
(C) H2S
(D) NO2
(E) NaCN
15. In a molecule in which the central atom exhibits sp3d2 hybrid orbitals, the electron
pairs are directed toward the corners of
(A) a tetrahedron
(B) a square-based pyramid
(C) a trigonal bipyramid
(D) a square
(E) an octahedron
32. CH3CH2OH boils at 78 °C and CH3OCH3 boils at - 24 °C, although both
compounds have the same composition. This difference in boiling points may be
attributed to a difference in
(A) molecular mass
(B) density
(C) specific heat
(D) hydrogen bonding
(E) heat of combustion
34.
X = CH3-CH2-CH2-CH2-CH3
Y = CH3-CH2-CH2-CH2-OH
Z = HO-CH2-CH2-CH2-OH
Based on concepts of polarity and hydrogen bonding, which of the following
sequences correctly lists the compounds above in the order of their increasing
solubility in water?
(A) Z < Y < X
(B) Y < Z < X
(C) Y < X < Z
(D) X < Z < Y
(E) X < Y < Z
Kim Duncan
Upper School Science Teacher
Flint Hill School
1
9
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08
09
10
Bonds
1
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08
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Bonds
1
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Bonds
1
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08
09
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Bonds
1
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08
09
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Bonds
1
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4
08
09
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Bonds
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A
A
A
C
D
C
B
AP MULTIPLE CHOICE PROBLEMS
57. Molecules that have planar configurations include which of the following?
I. BCl3
II. CHCl3
III. NCl3
(A) I only
(B) III only
(C) I and II only
(D) II and III only
(E) I, II, and III
62. The electron-dot structure (Lewis structure) for which of the following molecules
would have two unshared pairs of electrons on the central atom?
(A) H2S
(B) NH3
(C) CH4
(D) HCN
(E) CO2
68. Which of the following molecules has a dipole moment of zero?
(A) C6H6 (benzene)
(B) NO
(C) SO2
(D) NH3
(E) H2S
8. Questions 8-10 refer to the following diatomic species.
(A) Li2
(B) B2
(C) N2
(D) O2
(E) F2
8. Has the largest bond-dissociation energy
9. Has a bond order of 2
10. Contains 1 sigma (s) and 2 pi (p) bonds
60. R.
Bond
Average Bond Energy (kj/mole)
I2(g) + 3 Cl2(g) ---> 2 ICl3(g)
I---I
150
According to the data in the
table below, what is the value of Cl---Cl 240
I---Cl
210
represented above?
(A) - 870 kJ
(B) - 390 kJ
(C) + 180 kJ
(D) + 450 kJ
(E) + 1,260 kJ
Kim Duncan
Upper School Science Teacher
Flint Hill School
1
9
9
4
08
09
10
Bonds
1
9
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4
08
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Bonds
1
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Bonds
1
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08
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Bonds
1
9
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08
09
10
Bond
Therm
o
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B
D
D
C
C
AP MULTIPLE CHOICE PROBLEMS
28. The melting point of MgO is higher than that of NaF. Explanations for this
observation include which of the following?
I. Mg2+ is more positively charged than Na+
II. O2¯ is more negatively charged than F¯
III. The O2¯ ion is smaller than the F¯ ion
(A) II only
(B) I and II only
(C) I and III only
(D) II and III only
(E) I, II, and III
32. Types of hybridization exhibited by the C atoms in propene, CH3CHCH2, include
which of the following?
I. sp
II. sp2
III. sp3
(A) I only
(B) III only
(C) I and II only
(D) II and III only
(E) I, II, and III
40. Of the following molecules, which has the largest dipole moment?
(A) CO
(B) CO2
(C) O2
(D) HF
(E) F2
58. On a mountaintop, it is observed that water boils at 90°C, not at 100°C as at
sea level. This phenomenon occurs because on the mountaintop the
A) equilibrium water vapor pressure is higher due to the higher atmospheric pressure
B) equilibrium water vapor pressure is lower due to the higher atmospheric pressure
C) equilibrium water vapor pressure equals the atmospheric pressure at a lower
temperature
D) water molecules have a higher average kinetic energy due to the lower
atmospheric pressure
E) water contains a greater concentration of dissolved Gas
68. In which of the following processes are covalent bonds broken?
A) I2(s) --> I2(g)
B) CO2(s) --> CO2(g)
C) NaCl(s) --> NaCl(l)
D) C(diamond) --> C(g)
E) Fe(s) --> Fe(l)
Kim Duncan
Upper School Science Teacher
Flint Hill School
1
9
9
9
08
09
10
Bonds
1
9
9
9
08
09
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Org.
Bonds
1
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08
09
10
Bonds
1
9
9
9
08
09
10
Liquids
1
9
9
9
08
09
10
Bonds
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AP MULTIPLE CHOICE PROBLEMS
D 19. Which of the following
represents a pair of isotopes?
A
D
D
E
D
Atomic Number Mass Number
I.
6
14
(A)
II.
7
14
I.
6
7
(B)
II.
14
14
I.
6
14
(C)
II.
14
28
I.
7
13
(D)
II.
7
14
I.
8
16
(E)
II.
16
20
24. The formula for potassium hexacyanoferrate(II) is
(A) K4[Fe(CN)6]
(B) K3[Fe(CN)6]
(C) K2[Pt(CN)4]
(D) K2[Pt(CN)6]
(E) KCN
44. What number of moles of O2 is needed to produce 14.2 grams of P4O10 from P?
(Molecular weight P4O10 = 284)
(A) 0.0500 mole
(B) 0.0625 mole
(C) 0.125 mole
(D) 0.250 mole
(E) 0.500 mole
73. A 27.0-gram sample of an unknown hydrocarbon was burned in excess oxygen
to form 88.0 grams of carbon dioxide and 27.0 grams of water. What is a possible
molecular formula of the hydrocarbon?
(A) CH4
(B) C2H2
(C) C4H3
(D) C4H6
(E) C4H10
23. How many grams of calcium nitrate, Ca(NO3)2, contains 24 grams of oxygen
atoms?
(A) 164 grams
(B) 96 grams
(C) 62 grams
(D) 50. grams
(E) 41 grams
25. The simplest formula for an oxide of nitrogen that is 36.8 percent nitrogen by
weight is
(A) N2O
(B) NO
(C) NO2
(D) N2O3
(E) N2O5
Kim Duncan
Upper School Science Teacher
Flint Hill School
1
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1
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3
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06
& 07
TEST
Basics
Misc.
01-03
TEST
Stoich
01-03
TEST
Rxns
Stoich
01-03
TEST
Stoich
Stoich
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B
D
B
D
C
E
AP MULTIPLE CHOICE PROBLEMS
39. When a hydrate of Na2CO3 is heated until all the water is removed, it loses
54.3 percent of its mass. The formula of the hydrate is
(A) Na2CO3 . 10 H2O
(B) Na2CO3 . 7 H2O
(C) Na2CO3 . 5 H2O
(D) Na2CO3 . 3 H2O
(E) Na2CO3 . H2O
45. A measured mass of an unreactive metal was dropped into a small graduated
cylinder half filled with water. The following measurements were made.
Mass of metal = 19.611 grams
Volume of water before addition of metal = 12.4 milliliters
Volume of water after addition of metal = 14.9 milliliters
The density of the metal should be reported as
(A) 7.8444 grams per mL
(B) 7.844 grams per mL
(C) 7.84 grams per mL
(D) 7.8 grams per mL
(E) 8 grams per mL
19R. In which of the following compounds is the mass ratio of chromium to oxygen
closest to 1.6 to 1.0?
(A) CrO3
(B) CrO2
(C) CrO
(D) Cr20
(E) Cr2O3
42.
Mass of an empty container = 3.0 grams
Mass of the container plus the solid sample = 25.0 grams
Volume of the solid sample = 11.0 cubic centimeters
The data above were gathered in order to determine the density of an unknown
solid. The density of the sample should be reported as
(A) 0.5 g/cm3
(B) 0.50 g/cm3
(C) 2.0 g/cm3
(D) 2.00 g/cm3
(E) 2.27 g/cm3
47. When hafnium metal is heated in an atmosphere of chlorine gas, the product of
the reaction is found to contain 62.2 percent Hf by mass and 37.4 percent Cl by
mass. What is the empirical formula for this compound?
(A) HfCl
(B) HfCl2
(C) HfCl3
(D) HfCl4
(E) Hf2Cl3
49. Which of the following techniques is most appropriate for the recovery of solid
KNO3 from an aqueous solution of KNO3?
(A) Paper chromatography
(B) Filtration
(C) Titration
(D) Electrolysis
(E) Evaporation to dryness
Kim Duncan
Upper School Science Teacher
Flint Hill School
1
9
8
9
1
9
8
9
1
9
9
4
1
2
3
Stoich
1
2
3
Genl
Info
1
2
3
06
TEST
Stoich
01-03
TEST
1
9
9
4
1
2
3
1
9
9
9
1
2
3
1
9
9
9
1
2
3
Genl
Info
06
TEST
Stoich
Lab
[email protected]
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E
A
A
C
B
D
AP MULTIPLE CHOICE PROBLEMS
27. The critical temperature of a substance is the
(A) temperature at which the vapor pressure of the liquid is equal to the external
pressure
(B) temperature at which the vapor pressure of the liquid is equal to 760 mm Hg
(C) temperature at which the solid, liquid, and vapor phases are all in equilibrium
(D) Temperature at which liquid and vapor phases are in equilibrium at I atmosphere
(E) lowest temperature above which a substance cnnot be liquified at any applied
pressure
54. Which of the following statements is always true about the phase diagram of
any one-component system?
(A) The slope of the curve representing equilibrium between the vapor and liquid
phases is positive.
(B) The slope of the curve representing equilibrium between the liquid and solid
phases is negative.
(C) The slope of the curve representing equilibrium between the liquid and solid
phases is positive.
(D) the temperature at the triple point is greater than the normal freezing point.
(E) The pressure at the triple point is greater than 1 atmosphere.
21. Which of the following is true at the triple point of a pure substance?
(A) The vapor pressure of the solid phase always equal the vapor pressure of the
liquid phase.
(B) The temperature is always 0.01 K lower that the normal melting point.
(C) The liquid and gas phases of the substance always have the same density and
are therefore indistinguishable.
(D) the solid phase always melts if the pressure increases at constant temperature.
(E) The liquid phase always vaporizes if the pressure increases at constant
temperature.
49. Use the following diagram for 49-51.
49. The normal boiling point of the substanced
represented by the phase diagram above is
(A) -15 °C
(B) -10 °C
(C) 140 °C
(D) greater than 140 °C
(E) not determinable from the diagram
50. The phase diagram above provides sufficient information for determining the
(A) Entrop. change on vaporization
(B) conditions necessary for sublimation
(C) deviations from ideal gas behavior of the gas phase
(D) latent heat of vaporization
(E) latent heat of fusion
Most Dense
Least Dense
51. For the substance
(A) Solid
Gas
represented in the
(B) Solid
Liquid
diagram, which of the
phases is most dense and (C) Liquid
Solid
which is least dense at (D) Liquid
Gas
15 °C.
(E) The diagram gives no information about densities.
Kim Duncan
Upper School Science Teacher
Flint Hill School
1
9
8
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10
L&S
1
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8
4
10
L&S
1
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8
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L&S
1
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L&S
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C
A
B
B
A
D
C
C
C
AP MULTIPLE CHOICE PROBLEMS
26. Which of the following actions would be likely to change the boiling point of a
sample of a pure liquid in an open container?
I. Placing it in a smaller container
II. Increasing the number of moles of the liquid in the container
III. Moving the container and liquid to a higher altitude
(A) I only
(B) II only
(C) III only
(D) II and III only
(E) I, II, and III
5. Questions 5-7 refer to the phase diagram below of a pure substance.
(A) Sublimation
(B) Condensation
(C) Solvation
(D) Fusion
(E) Freezing
5. If the temperature increases from 10°
C to 60° C at a constant pressure of 0.4
atmosphcre, which of the processes
occurs?
6. If the temperature decreases from 110° C to 40° C at a constant pressure of 1.1
atmospheres, which of the processes occurs?
7. If the pressure increases from 0.5 to 1.5 atmospheres at a constant temperature of
50° C, which of the processes occurs?
13. Questions 13-16 refer to the following descriptions of bonding in different types
of solids.
(A) Lattice of positive and negative ions held together by electrostatic forces.
(B) Closely packed lattice with delocalized electrons throughout
(C) Strong single covalent bonds with weak intermolecular forces.
(D) Strong multiple covalent bonds (including bonds.) with weak intermolecular forces
(E) Macromolecules held together with strong polar bonds.
13. Cesium chloride, CsCl (s)
15. Carbon dioxide, CO2(s)
16. Methane, CH4(s)
25. The cooling curve for a pure substance as it changes
from a liquid to a solid is shown right. The solid and the
liquid coexist at
(A) point Q only
(B)
point R only
(C)
all points on the curve between Q and S
(D)
all points on the curve between R and T
(E)
no point on the curve
39. The phase diagram for a pure substance is shown above.
Which point on the diagram corresponds to the equilibrium
between the solid and liquid phases at the normal melting
point?
(A) A
(B) B
(C) C
(D) D
(E) E
Kim Duncan
Upper School Science Teacher
Flint Hill School
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AP MULTIPLE CHOICE PROBLEMS
10. Use the following answers for questions 10 - 13.
(A) CO32¯
(B) Cr2O72¯
(C) NH4+
(D) Ba2+
(E) Al3+
Assume that you have an "unknown" consisting of an aqueous solution of a salt that
contains one of the ions listed above. Which ions must be absent on the basis of each
of the following observations of the "unknown"?
10. The solution is colorless
11. The solution gives no apparent reaction with dilute hydrochloric acid.
12. No odor can be detected when a sample of the solution is added drop by drop
to a warm solution of sodium hydroxide.
13. No precipitate is formed when a dilute solution of H2SO4 is added to a sample
of the solution.
37. The molality of the glucose in a 1.0-molar glucose solution can be obtained by
using which of the following?
(A) Volume of the solution
(B) Temperature of the solution
(C) Solubility of glucose in water
(D) Degree of dissociation of glucose
(E) Density of the solution
55. At 20. °C, the vapor pressure of toluene is 22 millimeters of mercury and that of
benzene is 75 millimeters of mercury. An ideal solution, equimolar in toluene and
benzene, is prepared. At 20. °C, what is the mole fraction of benzene in the vapor in
equilibrium with this solution?
(A) 0.23
(B) 0.29
(C) 0.50
(D) 0.77
(E) 0.83
84. Which of the following aqueous solutions has the highest boiling point?
(A) 0.10 M potassium sulfate, K2SO4
(B) 0.10 M hydrochloric acid, HCl
(C) 0.10 M ammonium nitrate, NH4NO3
(D) 0.10 M magnesium sulfalte, MgSO4
(E) 0.20 M sucrose, C12H22O11
27.
I. Difference in temperature between freezing point of solvent and freezing point of
solvent and freezing point of solution
II. Molal freezing point depression constant, Kf, for solvent
In addition to the information above, which of the following gives the minimum data
required to determine the molecular mass of a nonionic substance by the freezing
point depression technique?
(A) No further information is necessary.
(B) Mass of solute
(C) Mass of solute and mass of solvent
(D) Mass of solute and volume of solvent
(E) Mass of solute, mass of solvent, and vapor pressure of solvent
Kim Duncan
Upper School Science Teacher
Flint Hill School
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AP MULTIPLE CHOICE PROBLEMS
28. Which of the following is probably true for a solid solute with a highly
endothermic heat of solution when dissolved in water?
(A) The solid has a low lattice energy.
(B) As the solute dissolves, the temperature of the solution increases.
(C) The resulting solution is ideal.
(D) The solid is more soluble at higher temperatures.
(E) the solid has a high energy of hydration.
71. A solution of toluene (molecular weight 92.1) in benzene (molecular weight 78.1)
is prepared. The mole fraction of toluene in the solution is 0.100. What is the
molality of the solution?
(A) 0.100 m
(B) 0.703 m
(C) 0.921 m
(D) 1.28 m
(E) 1.42 m
14. Which of the following is lower for a 1.0-molar aqueous solution of any solute
than it is for pure water?
(A) pH
(B) Vapor pressure
(C) Freezing point
(D) Electrical conductivity
(E) Absorption of visible light
44. Which of the following solutions has the lowest freezing point?
(A) 0.20 m C6H12O6, glucose
(B) 0.20 m NH4Br
(C) 0.20 m ZnSO4
(D) 0.20 m KMnO4
(E) 0.20 m MgCl2
31. If the temperature of an aqueous solution of NaCl is increased from 20 °C to 90
°C, which of the following statements is true?
(A) The density of the solution remains unchanged.
(B) The molarity of the solution remains unchanged.
(C) The molality of the solution remains unchanged.
(D) The mole fraction of solute decreases.
(E) The mole fraction of solute increases.
43. A sample of 61.8 g of H3BO3, a weak acid is dissolved in 1,000 g of water to
make a 1.0-molal solution. Which of the following would be the best procedure to
determine to molarity of the solution? (Assume no additional information is available.)
(A) Titration of the solution with standard acid
(B) Measurement of the pH with a pH meter
(C) Determination of the boiling point of the solution
(D) Measurement of the total volume of the solution
(E) Measurement of the specific heat of the solution
75. Which of the following pairs of liquids forms the solution that is most ideal (most
closely follows Raoult's law)?
A) C8H18(l) and H2O(l)
B) CH3CH2CH2OH(l) and H2O(l)
C) CH3CH2CH2OH(l) and C8H18(l)
D) C6H14(l) and C8H18(l)
E) H2SO4(l) and H2O(l)
Kim Duncan
Upper School Science Teacher
Flint Hill School
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AP MULTIPLE CHOICE PROBLEMS
25. Questions 25-26 H3AsO4 + 3I¯ + 2 H3O+ ---> H3AsO3 + I3¯ + H2O
The oxidation of iodide ions by arsenic acid in acidic aqueous solution occurs
according to the stoichiometry shown above. The experimental rate law of the
reaction is: Rate = k [H3AsO4] [I¯] [H3O+]
25. What is the order of the reaction with respect to I¯?
(A) 1
(B) 2
(C) 3
(D) 5
(E) 6
26. According to the rate law for the reaction, an increase in the concentration of
hydronium ion has what effect on this reaction?
(A) The rate of reaction increases.
(B) The rate of reaction decreases.
(C) The value of the equilibrium constant increases.
(D) The value of the equilibrium constant decreases.
(E) Neither the rate nor the value of the equilibrium constant is changed.
28. 2 A(g) + B(g) <===> 2 C(g)
When the concentration of substance B in the reaction above is doubled, all other
factors being held constant, it is found that the rate of the reaction remains
unchanged. The most probable explanation for this observation is that
(A) the order of the reaction with respect to substance B is 1
(B) substance B is not involved in any of the steps in the mechanism of the reaction
(C) substance B is not involved in the rate-determining step of the mechanism, but is
involved in subsequent steps
(D) substance B is probably a catalyst, and as such, its effect on the rate of the
reaction does not depend on its concentration
(E) the reactant with the smallest coefficient in the balanced equation Genlly has little
or no effecton the rate of the reaction
82. Nitramide, N2H2O2, decomposes slowly in aqueous solution. This decomposition is
believed to occur according to the reaction mechanism above. The rate law for the
decomposition of nitramide
fast
that is consistent with this
Step 1) N2H2O2 <===> N2HO2¯ + H+
equilibrium
mechanism is given by which
of the following?
Step 2) N2HO2¯ ---> N2O + OH¯
(slow)
(A) Rate = k [N2H2O2]
Step 3) H+ + OH¯ ---> H2O
(fast)
(B) Rate = k [N2H2O2] [H+]
(C) Rate = (k [N2H2O2]) / [H+]
(D) Rate = (k [N2H2O2]) / [N2HO2¯]
(E) Rate = k [N2H2O2] [OH¯]
57. rate = k[X]
For the reaction whose rate law is given above, a plot of which of the following is a
straight line?
(A) [X] versus time
(B) log [X] versus time
(C) 1/[X] versus time
(D) [X] versus 1/time
(E) log [X] versus 1/time
Kim Duncan
Upper School Science Teacher
Flint Hill School
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AP MULTIPLE CHOICE PROBLEMS
58. (CH3)3CCl(aq) + OH¯ ---> (CH3)3COH(aq) + Cl¯ For the reaction represented
above, the experimental rate law is given as follows. Rate = k [(CH3)3CCl]
If some solid sodium solid hydroxide is added to a solution that is 0.010-molar in
(CH3)3CCl and 0.10-molar in NaOH, which of the following is true? (Assume the
temperature and volume remain constant.)
(A) Both the reaction rate and k increase.
(B) Both the reaction rate and k decrease.
(C) Both the reaction rate and k remain the same.
(D) The reaction rate increases but k remains the same.
(E) The reaction rate decreases but k remains the same.
17. Relatively slow rates of chemical reaction are associated with which of the
following?
(A) The presence of a catalyst
(B) High temperature
(C) High concentration of reactants
(D) Strong bonds in reactant molecules
(E) Low activation energy
23. The proposed steps for a catalyzed reaction between Ce4+ and Tl+ are
represented above. The products of the overall catalyzed reaction are
Step 1: Ce4+ + Mn2+ ---> Ce3+ + Mn3+
Step 2: Ce4+ + Mn3+ ---> Ce3+ + Mn4+
Step 3: Mn4+ + Tl+ ---> Tl3+ + Mn2+
(A) Ce4+ and Tl+
(B) Ce3+ and Tl3+
(C) Ce3+ and Mn3+
(D) Ce3+ and Mn4+
(E) Tl3+ and Mn2+
49. The isomerization of cyclopropane to propylene is a first-order process with a
half-life of 19 minutes at 500 °C. The time it takes for the partial pressure of
cyclopropane to decrease from 1.0 atmosphere to 0.125 atmosphere at 500 °C is
closest to
(A) 38 minutes
(B) 57 minutes
(C) 76 minutes
(D) 152 minutes
(E) 190 minutes
63. The graph above shows the results of a study of the
reaction of X with a large excess of Y to yield Z. The
concentrations of X and Y were measured over a period
of time. According to the results, which of the following
can be concluded about the rate of law for the reaction
under the conditions studied?
A) It is zero order in [X].
B) It is first order in [X].
C) It is second order in [X].
D) It is the first order in [Y].
E) The overall order of the reaction is 2.
Kim Duncan
Upper School Science Teacher
Flint Hill School
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AP MULTIPLE CHOICE PROBLEMS
B 36. The initial-rate data
Initial Rate of
Initial [NO] Initial [O2]
in the table above were
Experiment
Formation of NO2
(mol L¯1
(mol L¯1
obtained for the reaction
(mol L¯1 s¯1)
represented below. What
1
0.10
0.10
2.5 x 10¯4
is the experimental rate
2
0.20
0.10
5.0 x 10¯4
la for the reaction?
(A) rate = k[NO] [O2]
3
0.20
0.40
8.0 x 10¯3
(B) rate = k[NO] [O2]2
(C) rate = k[NO]2 [O2]
(D) rate = k[NO]2 [O2]2
(E) rate = k[NO] / [O2]
C 36. CuO(s) + H2(g) <===> Cu(s) + H2
- 2.0 kilojoules
When the substances in the equation above are at equilibrium at pressure P and
temperature T, the equilibrium can be shifted to favor the products by
(A) increasing the pressure by means of a moving piston at constant T
(B) increasing the pressure by adding an inert gas such as nitrogen
(C) decreasing the temperature
(D) allowing some gases to escape at constant P and T
(E) adding a catalyst
B 57. For the reaction A(g)  B(g) + C(g), the equilibrium constant, Kp, is 2 x 10¯4 at
25 °C. A mixture of the three gases at 25 °C is placed in a reaction flask and the
initial pressures are PA = 2 atm, PB = 0.5 atm, and PC = 1 atm, At the instant of
mixing, which of the following is true for the reaction as written?
B 76. HgO(s) + 4 I¯ + H2O  HgI42
librium
above. Which of the following changes will increase the concentration of HgI42¯?
(A) Increasing the concentration of OH¯
(B) Adding 6 M HNO3
(C) Increasing the mass of HgO present
(D) Increasing the temperature
(E) Adding a catalyst
E 29. In which of the following systems would the number of moles of the substances
present at equilibrium NOT be shifted by a change in the volume of the system at
constant temperature?
(A) CO(g) + NO(g) <===> CO2(g) + 1/2 N2(g)
(B) N2(g) + 3 H2(g) <===> 2 NH3(g)
(C) N2(g) + 2 O2(g) <===> 2 NO2(g)
(D) N2O4(g) <===> 2 NO2(g)
(E) NO(g) + O3(g) <===> NO2(g) + O2(g)
Kim Duncan
Upper School Science Teacher
Flint Hill School
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AP MULTIPLE CHOICE PROBLEMS
A 48. PCl3(g) + Cl2(g)  PCl5(g) + energy
Some PCl3 and Cl2 are mixed in a container at 200 °C and the system reaches
equilibrium according to the equation above. Which of the following causes an
increase in the number of moles of PCl5 present at equilibrium?
I. Decreasing the volume of the container
II. Raising the temperature
III. Adding a mole of He gas at constant volume
(A) I only
(B) II only
(C) I and III only
(D) II and III only
(E) I, II, and III
D 51. 4 HCl(g) + O2(g)  2 Cl2(g) + 2 H2O(g) Equal numbers of moles of HCl and
O2 in a closed system are allowed to reach equilibrium as represented by the
equation above. Which of the following must be true at equilibrium?
I. [HCl] must be less than [Cl2].
II. [O2] must be greater than [HCl].
III. [Cl2] must equal [H2O].
(A) I only
(B) II only
(C) I and III only
(D) II and III only
(E) I, II, and III
A 73 R. 2 SO2(g) + O2(g)  2 SO3(g) When 0.40 mole of SO3 and 0.60 mole of O2
are placed in an evacuated 1.00-liter flask, the reaction represented above occurs.
After the reactants and the product reach equilibrium and the initial temperature is
restored, the flask is found to contain 0.30 mole of S03. Based on these results, the
expression for the equilibrium constant, Kc, of the reaction is
(A) (0.30)2 / [(0.45)(0.10)2]
(B) (0 30)2 / [(0.60)(0.40)2]
(C) (2 x 0.30) / [(0.45)(2 x 0.10)]
(D) (0.30) / [(0.45)(0.10)]
(E) (0.30) / [(0.60)(0.40)]
54. 2NO(g) + O2(g) 2 NO2
would cause a decrease in the value of Keq for the reaction represented above?
B A) Decreasing the temperature
B) Increasing the temperature
C) Decreasing the volume of the reaction vessel
D) Increasing the volume of the reaction vessel
E) Adding a catalyst
D 33. The pH of 0.1-molar ammonia is approximately
(A) 1
(B) 4
(C) 7
(D) 11
(E) 14
Kim Duncan
Upper School Science Teacher
Flint Hill School
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AP MULTIPLE CHOICE PROBLEMS
48. Which of the following ions is the strongest Lewis acid?
(A) Na+
(B) Cl¯
(C) CH3COO¯
(D) Mg2+
(E) Al3+
49. Each of the following can act as both a Brönsted acid and a Brönsted base
EXCEPT
(A) HCO3¯
(B) H2PO4¯
(C) NH4+
(D) H2O
(E) HS¯
53. Which, if any, of the following species is in the greatest concentration in a 0.100molar solution of H2SO4 in water?
(A) H2SO4 molecules
(B) H3O+ ions
(C) HSO4¯ ions
(D) SO42¯ ions
(E) All species are in equilibrium and therefore have the same concentrations.
71. Which of the following reactions does NOT proceed significantly to the right in
aqueous solutions?
(A) H3O+ + OH¯ ---> 2 H2O
(B) HCN + OH¯ ---> H2O + CN¯
(C) Cu(H2O)42+ + 4 NH3 ---> Cu(NH3)42+ + 4H2O
(D) H2SO4 + H2O ---> H3O+ + HSO4¯
(E) H2O + HSO4¯ ---> H2SO4 + OH¯
75. If the acid dissociation constant, Ka, for an acid HA is 8 x 10¯4 at 25 °C, what
percent of the acid is dissociated in a 0.50-molar solution of HA at 25 °C?
(A) 0.08%
(B) 0.2%
(C) 1%
(D) 2%
(E) 4%
34. All of the following species can function as Brönsted-Lowry bases in solution
EXCEPT
(A) H2O
(B) NH3
(C) S2¯
(D) NH4+
(E) HCO3¯
46. As the number of oxygen atoms increases in any series of oxygen acids, such as
HXO, HXO2, HXO3, ...., which of the following is generally true?
(A) The acid strength varies unpredictably.
(B) The acid strength decreases only if X is a nonmetal.
(C) The acid strength decreases only if X is a metal.
(D) The acid strength decreases whether X is a nonmetal or a metal.
(E) The acid strength increases.
Kim Duncan
Upper School Science Teacher
Flint Hill School
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[email protected]
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B
A
C
E
C
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AP MULTIPLE CHOICE PROBLEMS
54. Which of the following is the correct equilibrium expression for the hydrolysis of
CO32¯ ?
(A) K = [HCO3¯ ] / ( [CO32¯ ] [H3O+] )
(B) K = ( [HCO3¯] [OH¯] ) / [CO32¯]
(C) K = ( [CO32¯ ] [OH¯] ) / [HCO3¯]
(D) K = [CO32¯ ] / ( [CO2] [OH¯]2 )
(E) K = ( [CO32¯ ] [H3O+] ) / [HCO3¯]
55. H2PO4¯ + HBO32¯ <===> HPO42¯ + H2BO3¯
The equilibrium constant for the
reaction represented by the
Acids
Bases
equation above is greater than
(A) H2PO4¯ > H2BO3¯ and HBO32¯ > HPO42¯
1.0. Which of the following gives
(B) H2BO3¯ > H2PO4¯ and HBO32¯ > HPO42¯
the correct relative strengths of
(C) H2PO4¯ > H2BO3¯ and HPO42¯ > HBO32¯
the acids and bases in the
(D) H2BO3¯ > H2PO4¯ and HPO42¯ > HBO32¯
reaction?
(E) H2PO4¯ = H2BO3¯ and HPO42¯ = HBO32¯
56. A 0.20-molar solution of a weak monoprotic acid, HA, has a pH of 3.00. The
ionization constant of this acid is
(A) 5.0 x 10¯7
(B) 2.0 x 10¯7
(C) 5.0 x 10¯6
(D) 5.0 x 10¯3
(E) 2.0 x 10¯3
22. HSO4¯ + H2O <===> H3O+ + SO42¯ In the equilibrium represented above,
the species that act as bases include which of the following?
I. HSO4¯
II. H2O
III. SO42¯
(A) II only
(B) III only
(C) I and II
(D) I and III
(E) II and III
31. R. H2C2O4 + 2 H2O <===> 2 H3O+ + C2O42¯ Oxalic acid, H2C2O4, is a
diprotic acid with K1 = 5 x 10¯2 and K2 = 5 x 10¯5. Which of the following is equal
to the equilibrium constant for the reaction represented above?
(A) 5 x 10¯2
(B) 5 x 10¯5
(C) 2.5 x 10¯6
(D) 5 x 10¯7
(E) 2.5 x 10¯8
50. Which of the following acids can be oxidized to form a stronger acid?
(A) H3PO4
(B) HNO3
(C) H2CO3
(D) H3BO3
(E) H2SO3
Kim Duncan
Upper School Science Teacher
Flint Hill School
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AP MULTIPLE CHOICE PROBLEMS
61. A 1-molar solution of which of the following salts has the highest pH ?
(A) NaNO3
(B) Na2CO3
(C) NH4Cl
(D) NaHSO4
(E) Na2SO4
66. What is the pH of a 1.0 x 10¯2-molar solution of HCN? (Ka = 4.0 x 10¯10.)
(A) 10
(B) Between 7 and 10
(C) 7
(D) Between 4 and 7
(E) 4
38. A molecule or an ion is classified as a Lewis acid if it
(A) accepts a proton from water
(B) accepts a pair of electrons to form a bond
(C) donates a pair of electrons to form a bond
(D) donates a proton to water
(E) has resonance Lewis electron-dot structures
45. What is the H+(aq) concentration in 0.05 M HCN (aq) ? (The Ka for HCN is 5.0 x
10¯10)
(A) 2.5 x 10¯11
(B) 2.5 x 10¯10
(C) 5.0 x 10¯10
(D) 5.0 x 10¯6
(E) 5.0 x 10¯4
64. The net ionic equation for the reaction that occurs during the titration of nitrous
aicd with sodium hydroxide is
(A) HNO2 + Na+ + OH¯ ---> NaNO2 + H2O
(B) HNO2 + NaOH ---> Na+ + NO2¯ + H2O
(C) H+ + OH¯ --->H2O
(D) HNO2 + H2O ---> NO2¯ + H3O+
(E) HNO2 + OH¯ ---> NO2¯ + H2O
74. How many moles of NaF must be dissolved in 1.00 liter of a saturated solution of
PbF2 at 25 °C to reduce the [Pb2+] to 1 x 10¯6 molar? (Ksp of PbF2 at 25 °C = 4.0 x
10¯8)
(A) 0.020 mole
(B) 0.040 mole
(C) 0.10 mole
(D) 0.20 mole
(E) 0.40 mole
81. What is the net ionic equation for the reaction that occurs when aqueous
copper(II) sulfate is added to excess 6-molar ammonia?
(A) Cu2+ + SO42¯ + 2 NH4+ + 2 OH¯ ---> (NH4)2SO4 + Cu(OH)2
(B) Cu2+ + 4 NH3 + 4 H2O --> Cu(OH)42¯ + 4 NH4+
(C) Cu2+ + 2 NH3 + 2 H2O --> Cu(OH)2 + 2 NH4+
(D) Cu2+ + 4 NH3 --> Cu(NH3)42+
(E) Cu2+ + 2 NH3 + H2O --> CuO + 2 NH4+
Kim Duncan
Upper School Science Teacher
Flint Hill School
1
9
9
4
14
Acid
Base
1
9
9
4
14
Acid
Base
1
9
9
9
14
Acid
Base
1
9
9
9
14
Acid
Base
1
9
8
4
Rxns
15
1
9
8
4
15
Ksp
1
9
8
4
15
Rxns
06
TEST
[email protected]
703-584-2204
D
C
D
E
C
D
AP MULTIPLE CHOICE PROBLEMS
63. On the basis of the information below, a buffer
Acid Dissociation
Acid
with a pH = 9 can best be made by using
Constant, Ka
(A) pure NaH2PO4
H3PO4
7 x 10¯3
(B) H3PO4 + H2PO4¯
H2PO4¯
8 x 10¯8
(C) H2PO4¯ + PO43¯
2
(D) H2PO4¯ + HPO4 ¯
HPO42¯
5 x 10¯13
(E) HPO42¯ + PO43¯
19. In the titration of a weak acid of unknown concentration with a standard solution
of a strong base, a pH meter was used to follow the progress of the titration. Which
of the following is true for this experiment?
(A) The pH is 7 at the equivalence point.
(B) The pH at the equivalence point depends on the indicator used.
(C) The graph of pH versus volume of base added rises gradually at first and then
much more rapidly.
(D) The graph of pH versus volume of base added shows no sharp rise.
(E) The [H+] at the equivalence point equals the ionization constant of the acid.
35. When phenolphthalein is used as the indicator in a titration of an HCl solution
with a solution of NaOH, the indicator undergoes a color change from clear to red at
the end point of the titration. This color change occurs abruptly because
(A) phenolphthalein is a very strong acid that is capable of rapid dissociation
(B) the solution being titrated undergoes a large pH change near the end point of
the titration
(C) phenolphthalein undergoes an irreversible reaction in basic solution
(D) OH¯ acts as a catalyst for the decomposition of phenolphthalein
(E) phenolphehalein is involved in the rate-determining step of the reaction between
H3O+ and OH¯
52. The test for the presence of Ag+ in an unknown solution involves the treatment of
the solver-ammonia complex with dilute hydrochloric acid. The appearance of a
white precipitate at this point indicates the presence of silver ion in the original
sample. The net ionic equation that represents this test is
(A) Ag(NH4)4+ + 4 H+ <===> Ag(s) + 4 NH4+
(B) Ag(NH4)4+ + Cl¯ <===> AgCl(s) + 4 NH4+
(C) Ag(NH3)4+ + 4 HCl <===> AgCl(s) + 4 NH4+ + 3 Cl#175;
(D) Ag(NH3)4+ + Cl¯ <===> Ag(NH3)2Cl(s)
(E) Ag(NH3)4+ + 2 H+ + Cl#175; <===> AgCl(s) + 2 NH4+
65. The solubility of CuI is 2 x 10¯6 molar. What is the solubility product constant,
Ksp, for CuI?
(A) 1.4 x 10¯3
(B) 2 x 10¯6
(C) 4 x 10¯12
(D) 2 x 10¯12
(E) 8 x 10¯18
66. MnS(s) + 2 H+ <===> Mn2+ + H2S(g) At 25 °C the solubility product constant,
Ksp, for MnS in 5 x 10¯15 and the acid dissociation constants K1 and K2 for H2S are 1
x 10¯7 and 1 x 10¯13, respectively. What is the equilibrium constant for the reaction
represented by the equation above at 25 °C?
(A) 1 x 10¯13 / 5 x 10¯15
(B) 5 x 10¯15 / 1 x 10¯7
(C) 1 x 10¯7 / 5 x 10¯20
(D) 5 x 10¯15 / 1 x 10¯20
(E) 1 x 10¯20 / 5 x 10¯15
Kim Duncan
Upper School Science Teacher
Flint Hill School
1
9
8
4
15
Acid
Base
1
9
8
9
15
Lab
1
9
8
9
15
Lab
1
9
8
9
15
Aque.
Equil.
1
9
8
9
15
Ksp
1
9
8
9
15
Ksp
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A
B
A
D
B
B
A
A
AP MULTIPLE CHOICE PROBLEMS
69. A white solid is observed to be insoluble in water, insoluble in excess ammonia
solution, and soluble in dilute HCl. Which of the following compounds could the solid
be?
(A) CaCO3
(B) BaSO4
(C) Pb(NO3)2
(D) AgCl
(E) Zn(OH)2
74. Equal volumes of 0.10-molar H3PO4 and 0.20-molar KOH are mixed. After
equilibrium is established, the type of ion an solution in largest concentration, other
than the K+ ion, is
(A) H2PO4¯
(B) HPO42¯
(C) PO43¯
(D) OH¯
(E) H3O+
8. Use these answers for questions 8 - 10.
(A) a solution with a pH less than 7 that is not a buffer solution
(B) a buffer solution with a pH between 4 and 7
(C) a buffer solution with a pH between 7 and 10
(D) a solution with a pH greater than 7 that is not a buffer solution
(E) a solution with a pH of 7
Ionization Constants
CH3COOH = 1.8 x 10¯5
NH3 = 1.8 x 10¯5
H2CO3; K1 = 4 x 10¯7
H2CO3; K2 = 4 x 10¯11
8. A solution prepared to be initially 1 M in NaCl and 1 M in HCl.
9. A solution prepared to be initially 1 M in Na2CO3 and 1 M in CH3COONa
10. A solution prepared to be initially 0.5 M in CH3COOH and 1 M in CH3COONa
16. R. Commercial vinegar was titrated with NaOH solution to determine the content
of acetic acid, HC2H3O2. For 20.0 milliliters of the vinegar, 32.0 milliliters of 0.500molar NaOH solution was required. What was the concentration of acetic acid in the
vinegar if no other acid was present?
(A) 1.60 M
(B) 0.800 M
(C) 0.640 M
(D) 0.600 M
(E) 0.400 M
65. Barium sulfate is LEAST soluble in a 0.01-molar solution of which of the following?
(A) Al2(SO4)3
(B) (NH4)2SO4
(C) Na2SO4
(D) NH3
(E) BaCl2
74. A solution of calcium hypochlorite, a common additive to swimming-pool water, is
(A) basic because of the hydrolysis of the OCl¯ ion
(B) basic because Ca(OH)2 is a weak and insoluble base
(C) neutral if the concentration is kept below 0.1 molar
(D) acidic because of the hydrolysis of the Ca2+ ions
(E) acidic because the acid HOCl is formed
Kim Duncan
Upper School Science Teacher
Flint Hill School
1
9
8
9
15
Aque.
Equil.
1
9
8
9
15
Rxns
1
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15
Acid
Base
1
9
9
4
Rxns
15
1
9
9
4
15
Aque.
Solns
Precip
1
9
9
4
15
Acid
Base
06
TEST
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B
D
A
C
E
A
C
AP MULTIPLE CHOICE PROBLEMS
62. HC2H3O2(aq) + CN¯(aq) <===> HCN(aq) + C2H3O2¯(aq)
The reaction represented above has an equilibrium constant equal to 3.7 x 104.
Which of the following can be concluded from this information?
A) CN¯(aq) is a stronger base than C2H3O2¯(aq)
B) HCN(aq) is a stronger acid than HC2H3O2(aq)
C) The conjugate base of CN¯(aq) is C2H3O2¯(aq)
D) The equilibrium constant will increase with an increase in temperature.
E) The pH of a solution containing equimolar amounts of CN¯(aq) and HC2H3O2(aq)
is 7.0.
65. Which of the following compounds is NOT appreciably soluble in water but is
soluble in dilute hydrochloric acid?
A) Mg(OH)2(s)
B) (NH4)2CO3(s)
C) CuSO4(s)
D) (NH4)2SO4(s)
E) Sr(NO3)2(s)
67. What is the molar solubility in water of Ag2CrO4? (The Ksp for Ag2CrO4 is 8 x
10¯12.)
A) 8 x 10¯12 M
B) 2 x 10¯12 M
C) (4 x 10¯12 M)1/2
D) (4 x 10¯12 M)1/3
E) (2 x 10¯12 M)1/3
9. -12 refer to aqueous solutions containing 1:1 mole ratios of the following pairs of
substances. Assume all concentrations are 1 M.
(A) NH3 and NH4Cl
(B) H3PO4 and NaH2PO4
(C) HCl and NaCl
(D) NaOH and NH3
(E) NH3 and HC2H3O2 (acetic acid)
9. The solution with the lowest pH
10. The most nearly neutral solution
11. A buffer at a pH > 8
56. A cube of ice is added to some hot
Energy
Entrop.
water in a rigid, insulated container, which (A) Remains constant Remains constant
is then sealed. There is no heat exchange
with the surroundings. What has happened (B) Remains constant Decreases
(C) Remains constant Increases
to the total energy and the total Entrop.
when the system reaches equilibrium?
(D) Decreases
Increases
(E) Increases
Decreases
1
9
9
9
15
Acid
Base
1
9
9
9
15
Solns
Precip
1
9
9
9
15
Ksp
1
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9
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Acid
Base
1
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16
Test
Entrop
Therm
D
of Cl2
(A) H2(g) + Cl2(g) ---> 2 HCl(g)
(B) Cl2(g) + 1/2 O2(g) ---> Cl2O(g)
(C) Mg(s) + Cl2(g) ---> MgCl2(s)
(D) 2 NH4Cl(s) ---> N2(g) + 4 H2(g) + Cl2(g)
(E) Cl2(g) ---> 2 Cl(g)
Kim Duncan
Upper School Science Teacher
Flint Hill School
1
9
8
9
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Test
Entrop
Therm
[email protected]
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AP MULTIPLE CHOICE PROBLEMS
C 53. Which of the following must be true for a reaction that proceeds spontaneously
from initial standard state conditions?
eq > 1
eq < 1
eq > 1
eq > 1
(E
eq = 1
E 70. H2O(s) ---> H2O(l) When ice melts at its normal melting point, 273.16 K and 1
atmosphere, which of the following is true for the process shown above?
0
1
9
8
9
16
Test
Equil
Therm
1
9
8
9
16
17
Equil
Therm
1
9
9
4
16
Test
Entrop
Therm
16
Test
Entrop
Gibbs
Therm
1
9
9
9
16
Test
Entrop
Therm
1
9
9
9
16
Test
Entrop
Therm
D
I. 2 Fe2O3(s) ---> 4 Fe(s) + 3 O2(g)
II. Mg2+ + 2 OH¯ ---> Mg(OH)2(s)
III. H2(g) + C2H4(g) ---> 3 C2H6(g)
(A) I only
(B) I and II only
(C) I and III only
(D) II and III only
(E) I, II, and III
B 58. N2(g) + 3 H2(g) ---> 2 NH3(g)
The reaction indicated above is thermodynamically spontaneous at 298 K, but
becomes nonspontaneous at higher temperatures. Which of the following is true at
298 K?
A 66. When solid ammonium chloride, NH4Cl(s) is added
to water at 25 °C, it dissolves and the temperature of
the solution decreases. Which of the following is true
A) Postive Positive
B) Positive Negative
C) Positive Equal to zero
process?
D) Negative Positive
E) Negative Negative
E 22. Of the following reaction, which involves the largest decrease in Entrop.?
(A) CaCO3(s) ---> CaO(s) + CO2(g)
(B) 2 CO(g) + O2(g) ---> 2 CO2
(C) Pb(NO3)3 + 2 KI ---> PbI2 + 2 KNO3
(D) C3H8 + O2 ---> 3 CO2 + 4 H2O
(E) 4 La + 3 O2 ---> 2 La2O3
Kim Duncan
Upper School Science Teacher
Flint Hill School
1
9
9
4
[email protected]
703-584-2204
AP MULTIPLE CHOICE PROBLEMS
B
D
C
B
14. Questions 14-17
The spontaneous reaction that occurs when the
cell above operates is:
2Ag+ + Cd(s) ---> 2 Ag(s) + Cd2+
(A) Voltage increases.
(B) Voltage decreases but remains at zero.
(C) Voltage becomes zero and remains at zero.
(D) No change in voltage occures.
(E) Direction of voltage change cannot be
predicted without additional information.
Which of the above occurs for each of the
following circumstances?
14. A 50-milliliter sample of a 2-molar Cd(NO3)2 solution is added to the left
beaker.
15. The silver electrode is made larger.
16. The salt bridge is replaced by a platinum wire
17. Current is allowed to flow for 5 minutes
A 29. Cu(s) + 2 Ag+ ---> Cu2+ + 2 Ag(s) If the equilibrium constant for the reaction
above is 3.7 x 1015, which of the following correctly describes the standard voltage,
E°, and the standard free
B 46. If 0.060 faraday is passed through an electrolytic cell containing a solution of
In3+ ions, the maximum number of moles of In that could be deposited at the cathode
is
(A) 0.010 mole
(B) 0.020 mole
(C) 0.030 mole
(D) 0.060 mole
(E) 0.18 mole
A 83. NH3(g) + 2 CH4(g) + 5/2 O2(g) <===> H2NCH2COOH(s) + 3 H2O(l)
approximately equal to
- (11/2)RT
- (7/2)RT
D 75. If a copper sample
containing some zinc
impurity is to be purified by
electrolysis, the anode and
the cathode must be which
of the following?
Kim Duncan
Upper School Science Teacher
Flint Hill School
(A)
(B)
(C)
(D)
(E)
Anode
Pure copper
Pure zinc
Pure copper
Impure copper sample
Impure copper sample
Cathode
Pure zinc
Pure copper
Impure copper sample
Pure copper
Pure zinc
1
9
8
4
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Electro
1
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Electro
1
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8
4
17
Electro
1
9
8
4
17
Electro
1
9
8
9
17
Electro
[email protected]
703-584-2204
D
C
B
B
AP MULTIPLE CHOICE PROBLEMS
60. The standard reduction
Fe2+ + 2e¯ ---> Fe(s)
E° = - 0.44 volt
potentials for two half reactions are Ni2+ + 2e¯ ---> Ni(s)
E° = - 0.23 volt
given above. The Nernst equation
for a galvanic cell at 25° C in which Fe(s) reduces Ni2+ is the following.
E = E° - 0.059/2 log [Fe2+] / [Ni2+]
What is the equilibrium constant for the reaction below?
Fe(s) + Ni2+ ---> Fe2+ + Ni(s)
(A) 1.9 x 10¯23
(B) 7.6 x 10¯8
(C) 3.6 x 10+3
(D) 1.3 x 10+7
(E) 5.2 x 10+22
36. Zn(s) + Cu2+ ---> Zn2+ + Cu(s)
An electrolytic cell based on the reaction represented above was constructed from
zinc and copper half-cells. The observed voltage was found to be 1.00 volt instead
of the standard cell potential, E°, of 1.10 volts. Which of the following could
correctly account for this observation?
(A) The copper electrode was larger than the zinc electrode.
(B) The Zn2+ electrolyte was Zn(NO3)2, while the Cu2+ electrolyte was CuSO4.
(C) The Zn2+ solution was more concentrated than the Cu2+ solution.
(D) The solutions in the half-cells had different volumes.
(E) The salt bridge contained KCl as the electrolyte.
63R. Which of the following expressions is correct for the maxirnum mass of copper,
in grams, that cou1d be plated out by electrolyzing aqueous CuCl2 for 16 hours at a
constant current of 3.0 amperes? (1 faraday = 96,500 coulombs)
(A) [(16)(3,600)(3.0)(63.55)(2)] / (96,500)
(B) [(16)(3,600)(3.0)(63.55)] / [(96,500)(2)]
(C) [(16)(3,600)(3.0)(63.55)] / (96,500)
(D) [(16)(60)(3.0)(96,500)(2)] / (63.55)
(E) [(16)(60)(3.0)(96,500)] / [(63.55)(2)]
75. A direct-current power supply of low voltage (less than 10 volts) has lost the
markings that indicate which output terminal is positive and which is negative. A
chemist suggests that the power supply terminals be connected to a pair of platinum
electrodes that dip into 0.1-molar KI solution. Which of the following correctly
identifies the polarities of the power supply terminals?
(A) A gas will be evolved only at the positive electrode.
(B) A gas will be evolved only at the negative electrode.
(C) A brown color will appear in the solution near the negative electrode.
(D) A metal will be deposited on the positive electrode.
(E) None of the methods above will identify the polarities of the power supply
terminals.
Kim Duncan
Upper School Science Teacher
Flint Hill School
1
9
8
9
17
Electro
1
9
9
4
17
Electro
1
9
9
4
17
Electro
1
9
9
4
17
Electro
[email protected]
703-584-2204
AP MULTIPLE CHOICE PROBLEMS
34. Questions 34-35 refer to an electrolytic cell that involves the following halfreaction.
AlF63¯ + 3 e¯ ---> Al + 6F¯
A 34. Which of the following occurs in the reaction?
(A) AlF 63¯ is reduced at the cathode.
(B) Al is oxidized at the anode.
(C) Aluminum is converted from the -3 oxidation state
to the 0 oxidation state.
(D) F¯ acts as a reducing agent.
(E) F¯ is reduced at the cathode.
C
35. As steady current of 10 amperes in passed though
an aluminum-production cell for 15 minutes. Which of
the following is the correct expressions for calculating
the number of grams of aluminum produced? (1
faraday = 96,500 coulombs)
57. According to the information above, what is the standard reduction potential for
the half-reaction M3+(aq) + 3 e¯ --> M(s)?
A) -1.66 V
M(s) + 3 Ag+(aq) --> 3 Ag(s) + 3+(aq) E = +2.46 V
A B) -0.06 V
C) 0.06 V
Ag+(aq) + e¯ --> Ag(s)
E = +0.80 V
D) 1.66 V
E) 3.26 V
C 30. When 84-Po-214 decays, the emission consists consecutively of an alpha
particle, then two beta particles, and finally another alpha particle. The resulting
stable nucleus is
(A) 83-Bi-206
(B) 83-Bi-210
(C) 82-Pb-206
(D) 82-Pb-208
(E) 81-Tl-210
A 38. The radioactive decay of 6-C-14 to 7-N-14 occurs by the process of
(A) beta particle emission
(B) alpha particle emission
(C) positron emission
(D) electron capture
(E) neutron capture
B 18. For the types of radiation given, which of the following is the correct order of
increasing ability to penetrate a piece of lead?
(A) Alpha particles < gamma rays < beta particles
(B) Alpha particles < beta particles < gamma rays
(C) Beta particles < alpha particles < gamma rays
(D) Beta particles < gamma rays < alpha particles
(E) Gamma rays < alpha particles < beta particles
D 38. 98-Cf-251 ---> 2n + 54-Xe-131 + __
What is the missing product in the nuclear reaction represented above?
(A) 42-Mo-118
(B) 44-Ru-118
(C) 42-Mo-120
(D) 44-Ru-120
(E) 46-Pd-122
Kim Duncan
Upper School Science Teacher
Flint Hill School
1
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Electro
1
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Electro
1
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Nuke
1
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Nuke
1
9
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9
18
Nuke
1
9
18
8
9
Nuke
[email protected]
703-584-2204
E
D
E
B
D
AP MULTIPLE CHOICE PROBLEMS
68. The specific rate constant k for radioactive element X is 0.023 min -1. What
weight of X wsa originally present in a sample if 40. grams is left after 60. minutes?
(A) 10. grams
(B) 20. grams
(C) 80. grams
(D) 120 grams
(E) 160 grams
21. Correct statements about alpha particles include which of the following?
I. They have a mass number of 4 and a charge of +2.
II. They are more penetrating than beta particles.
III. They are helium nuclei.
(A) I only
(B) III only
(C) I and II
(D) I and III
(E) II and III
72. The nuclide 245Cm is radioactive and decays by the loss of one beta ([beta]¯)
particle. The product nuclide is
(A) 245Pu
(B) 95Am
(C) 248Cm
(D) 250Cm
(E) 97Bk
48. If 87.5 percent of a sample of pure 131I decays in 24 days, what is the half-life
of 131I?
(A) 6 days
(B) 8 days
(C) 12 days
(D) 14 days
(E) 21 days
77. Which of the following compounds exhibits optical isomerism?
1
9
18
8
9
Nuke
1
9
18
9
4
Nuke
1
9
9
4
18
Nuke
1
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Nuke
1
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22
Org.
1
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22
Org.
1
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22
Org.
A 43. Which of the following pairs of compounds are isomers?
(A)
(B)
(C)
(D)
(E)
E 29. The organic compound represented above
is an example of
(A) an organic acid
(B) an alcohol
(C) an ether
(D) an aldehyde
(E) a ketone
Kim Duncan
Upper School Science Teacher
Flint Hill School
[email protected]
703-584-2204
A
E
D
D
B
AP MULTIPLE CHOICE PROBLEMS
40. The geometry of the SO3 molecule is best described as
(A) trigonal planar
(B) trigonal pyramidal
(C) square pyramidal
(D) bent
(E) tetrahedral
31. A 0.1-molar solution of which of the following ions is orange?
(A) Fe(H2O)42+
(B) Cu(NH3)42+
(C) Zn(OH)42¯
(D) Zn(NH3)42+
(E) Cr2O72¯
35. The addition of an oxidizing agent such as chlorine water to a clear solution of
an unknown compound results in the appearance of a brown color. When this solution
is shaken with the organic solvent, methylene dichloride, the organic solvent layer
turns purple. The unknown compound probably contains
(A) K+
(B) Br¯
(C) NO3¯
(D) I¯
(E) Co2+
62. A student pipetted five 25.00-milliliter samples of hydrochloric acid and
transferred each sample to an Erlenmeyer flask, diluted it with distilled water, and
added a few drops of phenolphthalein to each. Each sample was then titrated with a
sodium hydroxide solution to the appearance of the first permanent faint pink color.
The following results were obtained.
Volumes of NaOH Solution
First Sample..................35.22 mL
Second Sample..............36.14 mL
Third Sample.................36.13 mL
Fourth Sample..............36.15 mL
Fifth Sample..................36.12 mL
Which of the following is the most probable explanation for the variation in the
student's results?
(A) The burette was not rinsed with NaOH solution.
(B) The student misread a 5 for a 6 on the burette when the first sample was titrated.
(C) A different amount of water was added to the first sample.
(D) The pipette was not rinsed with the HCI solution.
(E) The student added too little indicator to the first sample.
36. Appropriate laboratory procedures include which of the following?
I. Rinsing a buret with distilled water just before filling it with the titrant for the first
titration
II. Lubricating glass tubing before inserting it into a stopper
III. For accurate results, waiting until warm or hot objects have reached room
temperature before weighing them
(A) II only
(B) I and II only
(C) I and III only
(D) II and III only
(E) I, II, and III
Kim Duncan
Upper School Science Teacher
Flint Hill School
1
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10
Bonds
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Lab
Lab
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Lab
Lab
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Lab
Lab
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AP MULTIPLE CHOICE PROBLEMS
73. Adding water to some chemicals can be dangerous because large amounts of
heat are liberated. Which of the following does NOT liberate heat when water is
added to it?
(A) KNO3
(B) NaOH
(C) CaO
(D) H2SO4
(E) Na
38. Concentrations of colored substances are commonly measured by means of a
spectrophotometer. Which of the following would ensure that correct values are
obtained for the measured absorbance?
I. There must be enough sample in the tube to cover the entire light path.
II. The instrument must be periodically reset using a standard.
III. The solution must be saturated.
(A) I only
(B) II only
(C) I and II only
(D) II and III only
(E) I, II, and III
41. A strip of metallic scandium, Sc, is placed in a beaker containing concentrated
nitric acid. A brown gas rapidly forms, the scandium disappears, and the resulting
liquid is brown-yellow but becomes colorless when warmed. These observations best
support which of the following statements?
(A) Nitric acid is a strong acid.
(B) In solution scandium nitrate is yellow and scandium chloride is color less.
(C) Nitric acid reacts with metals to form hydrogen.
(D) Scandium reacts with nitric acid to form a brown gas.
(E) Scandium and nitric acid react in mole proportions of 1 to 3.
46. Which of the following solids dissolves in water to form a colorless solution?
(A) CrCl3
(B) FeCl3
(C) CoCl2
(D) CuCl2
(E) ZnCl2
52. When dilute nitric acid was added to a solution of one of the following
chemicals, a gas was evolved, This gas turned a drop of limewater, Ca(OH)2, cloudy,
due to the formation of a white precipitate. The chemical was
(A) household ammonia, NH3
(B) baking soda, NaHCO3
(C) table salt, NaCl
(D) epsom salts, MgSO4 . 7H2O
(E) bleach, 5% NaOCl
67. Substances X and Y that were in a solution were separated in the laboratory
using the technique of fractional crystallization. This fractional crystallization is
possible because substances X and Y have different
(A) boiling points
(B) melting points
(C) densities
(D) crystal colors
(E) solubilities
Kim Duncan
Upper School Science Teacher
Flint Hill School
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AP MULTIPLE CHOICE PROBLEMS
69. Correct procedures for a titration include which of the following?
I. Draining a pipet by touching the tip to the side of the container used for the
titration
II. Rinsing the buret with distilled water just before filling it with the liquid to be
titrated
III. Swirling the solution frequently during the titration
(A) I only
(B) II only
(C) I and III only
(D) II and III only
(E) I, II, and III
70. To determine the molar mass of a solid monoprotic acid, a student titrated a
weighed sample of the acid with standardized aqueous NaOH. Which of the
following could explain why the student obtained a molar mass that was too large?
I. Failure to rinse all acid from the weighing paper into the titration vessel
II. Addition of more water than was needed to dissolve the acid
III. Addition of some base beyond the equivalence point
(A) I only
(B) III only
(C) I and II only
(D) II and III only
(E) I, II, and III
21. When a solution of sodium chloride is vaporized in a flame, the color of the
flame is
(A) blue
(B) yellow
(C) green
(D) violet
(E) White
24. The safest and most effective emergency procedure to treat an acid splash on
skin is to do which of the following immediately?
(A) Dry the affected area with paper towels
(B) Sprinkle the affected area with powdered Na2SO4(s)
(C) Flush the affected area with water and then with a dilute NaOH solution
(D) Flush the affected area with water and then with a dilute NaHCO3 solution
(E) Flush the affected area with water and then with a dilute vinegar solution
27. Appropriate uses of a visible-light spectrophtometer include which of the
following?
I. Determining the concentration of a solution of Cu(NO3)2
II. Measuring the conductivity of a solution of KMnO4
III. Determining which ions are present in a solution that may contain Na+, Mg2+, Al3+
(A) I only
(B) II only
(C) III only
(D) I and II only
(E) I and III only
Kim Duncan
Upper School Science Teacher
Flint Hill School
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AP MULTIPLE CHOICE PROBLEMS
46. Which of the following occurs when excess concentrated NH3(aq) is mixed
thoroughly with 0.1 M Cu(NO3)2(aq) ?
(A) A dark red precipitate forms and settles out.
(B) Separate layers of immiscible liquids form with a blue layer on top.
(C) The color of the solution turns from light blue to dark blue.
(D) Bubbles of ammonia gas form.
(E) The pH of the solution decreases.
72. After completing an experiment to determine gravimetrically the percentage of
water in a hydrate, a student reported a value of 38 percent. The correct value for
the percentage of water in the hydrate is 51 percent. Which of the following is the
most likely explanation for this difference?
A) Strong initial heating caused some of the hydrate sample to spatter out of the
crucible.
B) The dehydrated sample absorbed moisture after heating.
C) The amount of the hydrate sample used was too small.
D) The crucible was not heated to constant mass before use.
E) Excess heating caused the dehydrated sample to decompose.
20. .....Mg(s) + .....NO3¯(aq) +.....H+(aq) --->......Mg2+(aq) + ....NH4+(aq) +
....H2O(l)
When the skeleton equation above is balanced and all coefficients reduced to their
lowest whole-number terms. what is the coeficient for H+ ?
(A) 4
(B) 6
(C) 8
(D) 9
(E) 10
32. The net ionic equation for the reaction between silver carbonate and
hydrochloric acid is
(A) Ag2CO3(s) + 2 H+ + 2 Cl¯ ---> 2 AgCl(s) + H2O + CO(g)
(B) 2 Ag+ + CO32¯ + 2 H+ + 2 Cl¯ ---> 2 AgCl(s) + H2O + CO2(g)
(C) CO32¯ + 2 H+ ---> H2O + CO2(g)
(D) Ag+ + Cl¯ ---> AgCl(s)
(E) Ag2CO3(s) + 2 H+ ---> 2Ag+ + H2CO3
34. ...CrO2¯ + ...OH¯ ---> ... CrO42¯ + ... H2O + ... e¯ When the equation for the
half-reaction above is balanced, what is the ratio of the coefficients OH¯ / CrO2¯ ?
(A) 1:1
(B) 2:1
(C) 3:1
(D) 4:1
(E) 5:1
42. Metallic copper is heated strongly with concentrated sulfuric acid. The products
of this reaction are
(A) CuSO4(s) and H2(g) only
(B) Cu2+, SO2(g), and H2O
(C) Cu2+, H2(g), and H2O
(D) CuSO4(s), H2(g), and SO2(g)
(E) Cu2+, SO3(g), and H2O
Kim Duncan
Upper School Science Teacher
Flint Hill School
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A
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AP MULTIPLE CHOICE PROBLEMS
45. The alkenes are compounds of carbon and hydrogen with the Genl formula
CnH2n. If 0.561 gram of any alkene is burned in excess oxygen, what number of
moles of H2O is formed?
(A) 0.0400 mole
(B) 0.0600 mole
(C) 0.0800 mole
(D) 0.400 mole
(E) 0.800 mole
61. When a solution of potassium dichromate is added to an acidified solution of
iron(II) sulfate, the products of the reaction are
(A) FeCr2O7(s) and H2O
(B) FeCrO4(s) and H2O
(C) Fe3+, CrO42¯, and H2O
(D) Fe3+, Cr3+, and H2O
(E) Fe2(SO4)3(s), Cr3+ and H2O
65. Which of the following species CANNOT function as an oxidizing agent?
(A) Cr2O72¯
(B) MnO4¯
(C) NO3¯
(D) S
(E) I¯
79. 5 Fe2+ + MnO4¯ + 8 H+ <===> 5 Fe3+ + Mn2+ + 4 H2O
In a titration experiment based on the equation above, 25.0 milliliters of an acidified
Fe2+ solution requires 14.0 milliliters of standard 0.050-molar MnO4¯ solution to
reach the equivalence point. The concentration of Fe2+ in the original soluiton is
(A) 0.0010 M
(B) 0.0056 M
(C) 0.028 M
(D) 0.090 M
(E) 0.14 M
E 20. 6 I¯ + 2 MnO4¯ + 4 H2O(l) ---> 3 I2(s) + 2 MnO2(s) + OH¯
Which of the following statements regarding the reaction represented by the
equation above is correct?
(A) Iodide ion is oxidized by hydroxide ion.
(B) MnO4¯ is oxidized by iodide ion.
(C) The oxidation number of manganese changes from +7 to +2.
(D) The oxidation number of manganese remains the same.
(E) The oxidation number of iodine changes from -1 to 0.
D 22. __ Cr2O72¯ + __ e¯ + __ H+ ---> __ Cr3+ + __ H2O(l) When the equation for
the half reaction above is balanced with the lowest whole-number coefficients, the
coefficient for H2O is
(A) 2
(B) 4
(C) 6
(D) 7
(E) 14
Kim Duncan
Upper School Science Teacher
Flint Hill School
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B
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AP MULTIPLE CHOICE PROBLEMS
37. __ CH3CH2COOH(l) + __ O2(g) ---> __ CO2(g) + __ H2O(l)
How many moles of O2 are required to oxidize 1 mole of CH3CH2COOH according
to the reaction represented above?
(A) 2 moles
(B) 5/2 moles
(C) 3 moles
(D) 7/2 moles
(E) 9/2 moles
44. The metal calcium reacts with molecular hydrogen to form a compound. All of the
following statements concerning this compound are true EXCEPT:
(A) Its formula is CaH2.
(B) It is ionic.
(C) It is solid at room temperatur(E)
(D) When added to water, it reacts to produce H2 gas.
(E) When added to water, it forms an acidic solution.
61. When acidified K2Cr2O7 solution is added to Na2S solution, green Cr3+ ions and
free S are formed. When acidified K2Cr2O7 solution is added to NaCl, no change
occurs. Of the substances involved in these reactions, which is the best reducing
agent?
(A) K2Cr2O7
(B) Na2S
(C) Cr3+
(D) S
(E) NaCl
67. BrO3¯ + 5 Br¯ + 6 H+ <===> 3 Br2 + 3 H2O
If 25.0 milliliters of 0.200-molar BrO3¯ is mixed with 30.0 milliliters of 0.450-molar
Br¯ solution that contains a large excess of H+, the amount of Br2 formed, according
to the equation above, is
(A) 5.00 x 10¯3 mole
(B) 8.10 x 10¯3 mole
(C) 1.35 x 10¯2 mole
(D) 1.50 x 10¯2 mole
(E) 1.62 x 10¯2 mole
18. 2 H2O + 4 MnO4¯ + 3 ClO2¯ ---> 4 MnO2 + 3 ClO4¯ + 4 OH¯
Which species acts as an oxidizing agent in the reaction represented above?
(A) H2O
(B) ClO4¯
(C) ClO2¯
(D) MnO2
(E) MnO4¯
20. . . . Ag+ + . . . AsH3(g) + . . . OH¯ ---> . . . Ag(s) + . . . H3AsO3(aq) + . . . H2O
When the equation above is balanced with lowest whole-number coefficients, the
coefficient for OH¯ is
(A) 2
(B) 4
(C) 5
(D) 6
(E) 7
Kim Duncan
Upper School Science Teacher
Flint Hill School
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04/05
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Rxns
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AP MULTIPLE CHOICE PROBLEMS
29. When an aqueous solution of NaOH is added to an aqueous solution of
potassium dichromate, K2Cr2O7 the dichromate ion is converted to
(A) CrO42¯
(B) CrO2
(C) Cr3+
(D) Cr2O3(s)
(E) Cr(OH)3(s)
55. What volume of 0.150-molar HCl is required to neutralize 25.0 milliliters of
0.120-molar Ba(OH)2?
(A) 20.0 mL
(B) 30 0 mL
(C) 40.0 mL
(D) 60.0 mL
(E) 80.0 mL
56. It is suggested that SO2 (molar mass 64 grams), which contributes to acid rain,
could be removed from a stream of waste Gas by bubbling the Gas through 0.25molar KOH, thereby producing K2SO3. What is the maximum mass of SO2 that could
be removed by 1,000. liters of the KOH solution?
(A) 4.0 kg
(B) 8.0 kg
(C) 16 kg
(D) 20. kg
(E) 40. kg
59. R. When a 1.25-gram sample of limestone was dissolved in acid, 0.44 gram of
CO2 was generated. If the rock contained no carbonate other than CaCO3, what
was the percent of CaCO3 by mass in the limestone?
(A) 35%
(B) 44%
(C) 67%
(D) 80%
(E) 100%
71 ... Fe(OH)2 + ... O2 + ... H2O ---> ... Fe(OH)3
If 1 mole of O2 oxidizes Fe(OH)2 according to the reaction represented above, how
many moles of Fe(OH)3 can be formed?
(A) 2
(B) 3
(C) 4
(D) 5
(E) 6
17. Question 17-18 refer to the following elements.
(A) Lithium
(B) Nickel
(C) Bromine
(D) Uranium
(E) Fluorine
17. Is a gas in its standard state at 298 K
18. Reacts with water to form a strong base
Kim Duncan
Upper School Science Teacher
Flint Hill School
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AP MULTIPLE CHOICE PROBLEMS
20. What mass of Au is produced when 0.0500 mol of Au2S3 is reduced completely
with excess H2?
(A) 9.85 g
(B) 19.7 g
(C) 24.5 g
(D) 39.4 g
(E) 48.9 g
26. . . .C10H12O4S(s) + . . O2(g) ---> . . . CO2(g) + . . . SO2(g) + . . . H2O(g)
When the equation above is balanced and all coefficients are reduced to their
lowest whole-number terms, the coefficient for O2(g) is?
(A) 6
(B) 7
(C) 12
(D) 14
(E) 28
42. . . . Li3N(s) + . . . H2O(l) ---> . . . Li+ (aq) + . . . OH¯(aq) + . . . NH3(g) When
the equation above is balanced and all coefficients reduced to lowest whole number
terms, the coefficient for OH¯(aq) is
(A) 1
(B) 2
(C) 3
(D) 4
(E) 6
55. 10 HI + 2 KMnO4 + 3 H2SO4 --> 5 I2 + 2 MnSO4 + K2SO4 + 8 H2O
According to the balanced equation above, how many moles of HI would be
necessary to produce 2.5 mol of I2, starting with 4.0 mol of KMnO4 and 3.0 mol of
H2SO4?
A) 20
B) 10
C) 8.0
D) 5.0
E) 2.5
Kim Duncan
Upper School Science Teacher
Flint Hill School
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