Download AP Midterm Review

AP Midterm Review
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. What type of compound is NaOH?
A. Binary
B. Molecular
C. Acid
D. Base
____
2. Name the compound CrO3.
A. chromium oxide
B. chromium(II) oxide
C. chromium(III) trioxide
D. chromium(VI) oxide
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3. Which of the following elements is chemically similar to magnesium?
A. sulfur
B. calcium
C. iron
D. nickel
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4. Which one of the following elements is most likely to form a 2+ ion?
A. calcium
B. carbon
C. fluorine
D. oxygen
____
5. Which one of the following elements is most likely to form a 2– ion?
A. scandium
B. selenium
C. silicon
D. strontium
____
6. A magnesium ion, Mg2+, has
A. 12 protons and 13 electrons.
B. 24 protons and 26 electrons.
C. 12 protons and 10 electrons.
D. 24 protons and 22 electrons.
____
7. An oxide ion, O2–, has:
A. 8 protons and 10 electrons
B. 10 protons and 8 electrons
C. 8 protons and 9 electrons
D. 8 protons and 7 electrons
____
8. What are the two different ions present in the compound Na2S?
A. Na2+, S2B. Na+, S2C. Na2+, S2D. Na+, S-
____
9. Which of the following is an example of an empirical formula?
A. C9H12
B. C9H18Cl2
C. C6H6
D. N2O4
____ 10. What is the empirical formula for C10H22O2?
A. C10H22O2
B. C5H11O
C. C20H44O4
D. C2H11O
____ 11. What is the formula for the ionic compound containing calcium ions and nitrate ions?
A. Ca3N2
B. Ca(NO3)2
C. Ca2NO3
D. Ca2NO2
____ 12. Which is the correct formula for iron(II) phosphate?
A. Fe2PO4
B. Fe3(PO4)2
C. Fe2PO3
D. Fe(PO4)2
____ 13. Which of the following is the formula for hydroiodic acid?
A. HIO4
B. HIO3
C. HIO2
D. HI
____ 14. The formula for magnesium sulfate is
A. MnS
B. MgS
C. MnSO3
D. MgSO4
____ 15. The formula for sodium sulfide is
A. NaS.
B. K2S.
C. NaS2.
D. Na2S.
____ 16. The name for KHCO3 is
A. calcium bicarbonate.
B. potassium hydrogen carbonate .
C. potassium carbonate.
D. calcium hydrogen carbon trioxide.
____ 17. Name the compound Al2O3
A. Aluminum oxide
B. Aluminum (II) oxide
C. Dialuminum trioxide
D. Aluminum trioxide
____ 18. Which is the formula for lead(IV) chloride?
A. Pb4Cl
B. PbCl2
C. PbCl3
D. PbCl4
____ 19. What type of compound is NH4NO3
A. Ionic
B. Molecular
C. Acid
D. Base
____ 20. What type of compound is IF5?
A. Ionic
B. Molecular
C. Acid
D. Base
____ 21. What type of compound is H2SO3?
A. Ionic
B. Binary
C. Acid
D. Base
____ 22. Name the acid H3PO4 (dissolved in water).
A. Phosphoric acid
B. Phosphorous acid
C. Hydrogen phosphate acid
D. Hydrophosphate acid
____ 23. Name the acid H2SO3 (dissolved in water).
A. Sulfuric acid
B. Sulfurous acid
C. Hydrosulfuric acid
D. Persulfuric acid
____ 24. What is the molecular mass of Br2 ?
A. 79.90 amu
B. 79.90 g
C. 159.8 amu
D. 159.8 g
____ 25. What is the mass of 3.50  1024 Ti atoms?
A. 47.9 amu
B. 47.9 g
C. 5.81 g
D. 278 g
____ 26. If 0.274 moles of a substance weighs 62.5 g, what is the molar mass of the substance, in units of
g/mol?
A. 2.28  102 g/mol
B. 1.71  101 g/mol
C. 4.38  10–3 g/mol
D. 2.17  102 g/mol
____ 27. How many C atoms are in 5.50 g of C?
A. 5.01  1022 C atoms
B. 3.31  1024 C atoms
C. 6.02  1023 C atoms
D. 2.76  1023 C atoms
____ 28. How many moles of CF4 are there in 171 g of CF4?
A. 0.51 mol
B. 1.94 mol
C. 4.07 mol
D. 88.0 mol
____ 29. Calculate the number of moles of cesium in 50.0 g of cesium.
A. 0.376 mol
B. 0.357 mol
C. 2.66 mol
D. 2.80 mol
____ 30. Calculate the molar mass of Ba(NO3)2.
A. 199.3 g/mol
B. 323.3 g/mol
C. 247.3 g/mol
D. 261.3 g/mol
____ 31. How many moles of O are in 2.45 moles of H2CO3?
A. 2.45 moles O
B. 39.2 moles O
C. 118 moles O
D. 7.35 moles O
____ 32. Calculate the mass of N in 2.34 g of N2H4?
A. 4.68 g N
B. 65.6 g N
C. 28.02 g N
D. 2.05 g N
____ 33. A mass spectrometer works by ionizing atoms or molecules, and then accelerating them through
oppositely charged plates. The mass is obtained by
A. measuring the force of impact on a detecting screen, and then calculating the mass
using force = mass  acceleration.
B. suspending the ions in an applied electric field, and then calculating mass by the
setting the downward gravitational force equal to the upward electrostatic force.
C. measuring the magnitude of deflection as the ions pass through a magnetic field to
obtain the charge-to-mass ratio, and then calculating the mass from that ratio.
D. measuring the time it takes for the ions to hit the detector at a known distance to
calculate the acceleration, and then calculating mass from force = mass 
acceleration.
____ 34. An unknown compound with a molar mass of 223.94 g/mol consists of 32.18% C, 4.50% H, and
63.32% Cl. Find the molecular formula for the compound.
A. CHCl
B. C6H10Cl4
C. C3H5Cl2
D. C9H15Cl6
____ 35. The empirical formula of a compound of uranium and fluorine that is composed of 67.6% uranium
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and 32.4% fluorine is
A. U2F
B. U3F4
C. UF4
D. UF6
Which one of the following is an example of a balanced chemical reaction?
A. C3H6O + 4O2  3CO2 + 3H2O
B. 2C3H6O + 9O2  6CO2 + 6H2O
C. C3H6O + 3O2  3CO2 + 3H2O
D. 2C3H6O + 9O2  6CO2 + 3H2O
When balanced the coefficient of O2 in the following equation is
__ C2H4 + __ O2  __ CO2 + __ H2O
A. 1.
B. 2.
C. 3.
D. 4.
Ammonia reacts with hydrochloric acid to produce ammonium chloride. Identify the balanced
reaction that describes this process.
A. NH4+ + HCl  NH4Cl + H
B. NH3 + HCl  NH4Cl
C. NH3 + 2HCl  NH4Cl + H
D. NH4+ + 2HCl  NH4Cl2
When 22.0 g NaCl and 21.0 g H2SO4 are mixed and react according to the equation below, which is
the limiting reagent?
2NaCl + H2SO4  Na2SO4 + 2HCl
A. NaCl
B. H2SO4
C. Na2SO4
D. HCl.
Phosphorus pentachloride reacts with water to form hydrochloric acid and phosphoric acid. How
many total moles of acid are formed when starting with 4.5 g of PCl5 and excess H2O?
PCl5 + 4H2O  5HCl + H3PO4
A. 0.022 moles
B. 0.12 moles
C. 0.13 moles
D. 27 moles
Hydrogen chloride gas can be prepared by the following reaction:
2NaCl(s) + H2SO4(aq)  2HCl(g) + Na2SO4(s)
How many grams of HCl can be prepared from 2.00 mol H2SO4 and 2.56 mol NaCl?
A. 7.30 g
B. 93.3 g
C. 146 g
D. 150 g
____ 42. Calculate the mass of excess reagent remaining at the end of the reaction in which 90.0 g of SO2 are
mixed with 100.0 g of O2.
2SO2 + O2  2SO3
A. 11.5 g
B. 22.5 g
C. 67.5 g
D. 77.5 g
____ 43. What is the theoretical yield of H2O that can be obtained from the reaction of 4.5 g H2 and excess
O2?
2H2(g) + O2(g)  2H2O(g)
A. 4.5 g
B. 9.0 g
C. 40. g
D. 80. g
____ 44. The reaction of 44.1 g of Cr2O3 with 35.0 g of Al produced 25.6 g of Cr. What is the percent yield
for this reaction?
2Al + Cr2O3  Al2O3 + 2Cr
A. 37.9 %
B. 58.0 %
C. 73.1 %
D. 84.9%
____ 45. Based on the solubility rules, which one of the following compounds should be insoluble in water?
A. NaCl
B. MgBr2
C. FeCl2
D. AgBr
____ 46. Based on the solubility rules, which of the following compounds should be insoluble in water?
A. Na2SO4
B. BaSO4
C. CuSO4
D. MgSO4
____ 47. Which of the following will occur when a solution of Pb(NO3)2(aq) is mixed with a solution of
KI(aq) ?
A. A precipitate of KNO3 will form; Pb2+ and I– are spectator ions.
B. No precipitate will form.
C. A precipitate of Pb(NO3)2 will form; K+ and I– are spectator ions.
D. A precipitate of PbI2 will form; K+ and NO3– are spectator ions.
____ 48. Which of the following will occur when solutions of CuSO4(aq) and BaCl2(aq) are mixed?
A. A precipitate of CuCl2 will form; Ba2+ and SO42– are spectator ions.
B. A precipitate of CuSO4 will form; Ba2+ and Cl– are spectator ions.
C. A precipitate of BaSO4 will form; Cu2+ and Cl– are spectator ions.
D. A precipitate of BaCl2 will form; Cu2+ and SO42– are spectator ions.
____ 49. Identify the precipitate(s) formed when solutions of Ca(ClO4)2(aq), K2CO3(aq), and NaNO3(aq) are
mixed.
A. CaCO3
B. Na2CO3
C. Ca(NO3)2 and NaClO4
D. CaCO3 and Na2CO3
____ 50. Identify the correct net ionic equation for the reaction that occurs when solutions of Pb(NO3)2 and
NH4Cl are mixed.
A. Pb(NO3)2(aq) + 2NH4Cl(aq)  NH4NO3(aq) + PbCl2(s)
B. Pb2+(aq) + 2Cl–(aq)  PbCl2(s)
C. Pb2+(aq) + 2NO3– (aq) + 2NH (aq) + 2Cl–(aq)  2NH (aq) + 2NO3– (aq) +
PbCl2(s)
D. NH4+(aq)+ NO3– (aq)  2NH4NO3(s)
____ 51. Which of the following compounds is a strong acid?
A. HF
B. HI
C. HClO2
D. H2SO3
____ 52. Which of the following compounds is a weak base?
A. KOH
B. Sc(OH)3
C. NH3
D. NH4+
____ 53. Identify the correct net ionic equation for the reaction that occurs when solutions of HNO3 and KOH
are mixed?
A. HNO3(aq) + KOH(aq)  H2O(l) + KNO3(aq)
B. K+(aq) + NO3-(aq)  KNO3(aq)
C. HNO3(aq) + KOH(aq)  2(l) + KNO3(s)
D. H+(aq) + OH-(aq)  H2O(l)
____ 54. The oxidation number of Fe in K3Fe(CN)6 is
A. +3
B. +2
C. +1
D. –3
____ 55. Determine the correct oxidation numbers for all three elements in Rb2SO3 in the order that the
elements are shown in the formula.
A. –2, +6, –2
B. –1, +4, –3
C. +2, +4, –2
D. +1, +4, –2
____ 56. Using the redox reaction below determine which element is oxidized and which is reduced.
4NH3 + 3Ca(ClO)2  2N2 + 6H2O + 3CaCl2
A. H is oxidized and N is reduced
B. N is oxidized and Cl is reduced
C. N is oxidized and O is reduced
D. Cl is oxidized and O is reduced
____ 57. Which of the following represents a precipitation reaction?
A. 2H2(g) + O2(g)  2H2O(l)
B. CaBr2(aq) + H2SO4(aq)  CaSO4(s) + 2HBr(g)
C. 2KNO3(s)  2KNO2(s) + O2(g)
D. 2KBr(aq) + Cl2(g)  2KCl(aq) + Br2(l)
____ 58. Which of the following represents an acid-base neutralization reaction?
A. 2Al(s) + 3H2SO4(aq)  Al2(SO4)3(aq) + 3H2(g)
B. SO2(g) + H2O(l)  H2SO3(g)
C. LiOH(aq) + HNO3(aq)  LiNO3(aq) + H2O(l)
D. 2KBr(aq) + Cl2(g)  2KCl(aq) + Br2(l)
____ 59. Which of the following represents a combustion reaction?
A. 2C2H6(g) + 7O2(g)  4CO2(g) + 6H2O(l)
B. LiOH(aq) + HNO3(aq)  LiNO3(aq) + H2O(l)
C. N2(g) + 3H2(g)  2NH3(g)
D. 2Na(s) + 2H2O(l)  2NaOH(aq) + H2(g)
____ 60. What mass of C6H12O6 (glucose) is needed to prepare 450. mL of a 0.650 M solution of glucose in
water?
A. 0.293 g
B. 293 g
C. 0.692 g
D. 52.7 g
____ 61. A 50.0 mL sample of 0.436 M NH4NO3 is diluted with water to a total volume of 250.0 mL. What is
the ammonium nitrate concentration in the resulting solution?
A. 21.8 M
B. 0.459 M
C. 2.18  10–2 M
D. 8.72  10–2 M
____ 62. A 350. mL solution of 0.150 M HNO3(aq) is mixed with a solution of 230. mL of 0.240 M HCl(aq).
How many moles of H+(aq) are present in the final solution?
A. 0.0525 moles H+
B. 0.108 moles H+
C. 0.186 moles H+
D. 0.0539 moles H+
____ 63. What volume (mL) of a 0.3428 M HCl(aq) solution is required to completely neutralize 23.55 mL of
a 0.2350 M Ba(OH)2(aq) solution?
A. 55.34 mL
B. 11.07 mL
C. 16.14 mL
D. 32.29 mL
____ 64. What will happen to the height (h) of the column of mercury in the manometer shown below if the
stopcock is opened?
A.
B.
C.
D.
h will decrease
h will not change
h will increase
not enough information given to answer the question
____ 65. A sample of oxygen gas has a volume of 545 mL at 35°C. The gas is heated to 151°C at constant
pressure in a container that can contract or expand. What is the final volume of the oxygen gas?
A. 750. mL
B. 396 mL
C. 417 mL
D. 267 mL
____ 66. A small bubble rises from the bottom of a lake, where the temperature and pressure are 4°C and 3.0
____ 67.
____ 68.
____ 69.
____ 70.
____ 71.
____ 72.
atm, to the water's surface, where the temperature is 25°C and the pressure is 0.95 atm. Calculate the
final volume of the bubble if its initial volume was 2.1 mL.
A. 0.72 mL
B. 6.2 mL
C. 7.1 mL mL
D. 22.4 mL
The temperature of a sample of argon gas in a 365 mL container at 740. mmHg and 25°C is lowered
to 12°C. Assuming the volume of the container and the amount of gas is unchanged, calculate the
new pressure of the argon.
A. 0.468 atm
B. 0.931 atm
C. 1.02 atm
D. 1.54 atm
0.820 mole of hydrogen gas has a volume of 2.00 L at a certain temperature and pressure. What is
the volume of 0.125 mol of this gas at the same temperature and pressure?
A. 0.0512 L
B. 0.250 L
C. 0.305 L
D. 4.01 L
Calculate the volume occupied by 35.2 g of methane gas (CH4) at 25°C and 1.0 atm. R = 0.08206
Latm/Kmol.
A. 0.0186 L
B. 4.5 L
C. 53.7 L
D. 49.2 L
Calculate the mass, in grams, of 2.74 L of CO gas measured at 33°C and 945 mmHg.
A. 0.263 g
B. 2.46 g
C. 3.80 g
D. 35.2 g
A 1.07 g sample of a Noble gas occupies a volume of 363 mL at 35°C and 678 mmHg. Identify the
Noble gas in this sample? (R = 0.08206 Latm/Kmol)
A. He
B. Ne
C. Ar
D. Kr
A mixture of three gases has a total pressure of 1,380 mmHg at 298 K. The mixture is analyzed and
is found to contain 1.27 mol CO2, 3.04 mol CO, and 1.50 mol Ar. What is the partial pressure of
Ar?
A. 0.258 atm
B. 301 mmHg
C. 356 mmHg
D. 5,345 mmHg
____ 73. How many liters of chlorine gas at 25°C and 0.950 atm can be produced by the reaction of 12.0 g of
____ 74.
____ 75.
____ 76.
____ 77.
____ 78.
____ 79.
____ 80.
MnO2 with excess HCl(aq) according to the following chemical equation?
MnO2(s) + 4HCl(aq)  MnCl2(aq) + 2H2O(l) + Cl2(g)
-3
A. 5.36  10 L
B. 3.55 L
C. 0.282 L
D. 3.09 L
Calculate the volume of H2(g) at 273 K and 2.00 atm that will be formed when 275 mL of 0.725 M
HCl solution reacts with excess Mg to give hydrogen gas and aqueous magnesium chloride.
A. 0.56 L
B. 1.12 L
C. 2.23 L
D. 3.54 L
What mass of KClO3 must be decomposed to produce 126 L of oxygen gas at 133°C and 0.880 atm?
(The other reaction product is solid KCl.)
A. 24.6 g
B. 70.8 g
C. 272 g
D. 408 g
The molecules of different samples of an ideal gas have the same average kinetic energies, at the
same
A. pressure.
B. temperature.
C. volume.
D. density.
Which gas has molecules with the greatest average molecular speed at 25°C?
A. CH4
B. Kr
C. N2
D. CO2
Which of these gas molecules have the highest average kinetic energy at 25°C?
A. H2
B. O2
C. N2
D. All the gases have the same average kinetic energy.
Deviations from the ideal gas law are greater at
A. low temperatures and low pressures.
B. low temperatures and high pressures.
C. high temperatures and high pressures.
D. high temperatures and low pressures.
Samples of the following volatile liquids are opened simultaneously at one end of a room. If you are
standing at the opposite end of this room, which species would you smell first? (Assume that your
nose is equally sensitive to all these species.)
A. ethyl acetate (CH3COOC2H5)
B. camphor (C10H16O)
C. naphthalene (C10H8)
D. diethyl ether (C2H5OC2H5)
AP Midterm Review
Answer Section
MULTIPLE CHOICE
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REF: Section: 2.7
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DIF: Difficult
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52. ANS:
OBJ:
53. ANS:
OBJ:
54. ANS:
OBJ:
55. ANS:
OBJ:
56. ANS:
OBJ:
57. ANS:
OBJ:
58. ANS:
OBJ:
59. ANS:
OBJ:
60. ANS:
OBJ:
61. ANS:
OBJ:
62. ANS:
OBJ:
63. ANS:
OBJ:
64. ANS:
OBJ:
65. ANS:
OBJ:
66. ANS:
OBJ:
67. ANS:
OBJ:
68. ANS:
OBJ:
69. ANS:
OBJ:
70. ANS:
OBJ:
D
EK.3.C.1
C
EK.3.C.1
A
EK.3.C.1
B
EK.3.A.1
B
EK.3.B.2
C
EK.3.B.2
D
EK.3.A.1
A
EK.3.B.3
D
EK.3.B.3
B
EK.3.B.3
B
EK.3.C.1
C
EK.3.B.2
A
EK.3.B.1
D
EK.2.A.3
D
EK.2.A.3
B
EK.2.A.3
D
EK.2.A.3
A
EK.2.A.2
A
EK.1.E.1
C
EK.2.A.2
B
EK.1.E.1
C
EK.1.E.1
C
EK.2.A.2
C
EK.2.A.2
PTS: 1
DIF: Medium
REF: Section: 4.2
PTS: 1
DIF: Medium
REF: Section: 4.2
PTS: 1
DIF: Medium
REF: Section: 4.2
PTS: 1
DIF: Medium
REF: Section: 4.2
PTS: 1
DIF: Easy
REF: Section: 4.3
PTS: 1
DIF: Easy
REF: Section: 4.3
PTS: 1
DIF: Medium
REF: Section: 4.3
PTS: 1
DIF: Medium
REF: Section: 4.4
PTS: 1
DIF: Medium
REF: Section: 4.4
PTS: 1
DIF: Medium
REF: Section: 4.4
PTS: 1
DIF: Easy
REF: Section: 4.2
PTS: 1
DIF: Easy
REF: Section: 4.3
PTS: 1
DIF: Easy
REF: Section: 4.4
PTS: 1
DIF: Medium
REF: Section: 4.5
PTS: 1
DIF: Easy
REF: Section: 4.5
PTS: 1
DIF: Difficult
REF: Section: 4.5
PTS: 1
DIF: Medium
REF: Section: 4.7
PTS: 1
DIF: Medium
REF: Section: 5.2
PTS: 1
DIF: Medium
REF: Section: 5.3
PTS: 1
DIF: Medium
REF: Section: 5.4
PTS: 1
DIF: Medium
REF: Section: 5.3
PTS: 1
DIF: Medium
REF: Section: 5.3
PTS: 1
DIF: Medium
REF: Section: 5.4
PTS: 1
DIF: Medium
REF: Section: 5.4
71. ANS:
OBJ:
72. ANS:
OBJ:
73. ANS:
OBJ:
74. ANS:
OBJ:
75. ANS:
OBJ:
76. ANS:
OBJ:
77. ANS:
OBJ:
78. ANS:
OBJ:
79. ANS:
OBJ:
80. ANS:
OBJ:
D
EK.2.A.2
C
EK.2.A.2
B
EK.1.E.2
B
EK.1.E.2
C
EK.1.E.2
B
EK.2.A.2
A
EK.2.A.2
D
EK.2.A.2
B
EK.2.A.2
D
EK.2.A.2
PTS: 1
DIF: Medium
REF: Section: 5.4
PTS: 1
DIF: Medium
REF: Section: 5.6
PTS: 1
DIF: Medium
REF: Section: 5.5
PTS: 1
DIF: Difficult
REF: Section: 5.5
PTS: 1
DIF: Difficult
REF: Section: 5.5
PTS: 1
DIF: Easy
REF: Section: 5.7
PTS: 1
DIF: Easy
REF: Section: 5.7
PTS: 1
DIF: Easy
REF: Section: 5.7
PTS: 1
DIF: Medium
REF: Section: 5.8
PTS: 1
DIF: Medium
REF: Section: 5.7