Download LaBrake, Fundamentals Diagnostic Questions

LaBrake, Fundamentals Diagnostic Questions
1. Assuming the following numbers are measurements and using the rules for significant
figures, determine the answer for the following calculation.
(2 x 2.4) + (361 /1.7) + (3.5  102) =
a)
b)
c)
d)
e)
567.1529
567.2
567
5.7  102 (correct)
600
2. Assuming the following numbers are measurements and using the rules for significant
figures, determine the answer for the following calculation.
(15.5/42)  219.5 =
a)
b)
c)
d)
e)
81.0059
81.006
81.01
81.0
81 (correct)
3. Assuming the following numbers are measurements and using the rules for significant
figures, determine the answer for the following equation.
10054.67 + 454.2 + 64.78 + 2891 =
a) 10862.75
b) 10862.8
c) 10863 (correct)
d) 10860
e) 10900
4. How many significant figures are in the following measurements?
1  102 cm, 1.01  102 cm, 1.001  102 cm, 1.0010  102 cm, 1.00  102 cm, 1.00010 
102 cm
a) 3, 3, 4, 4, 3, 5
b) 3, 3, 2, 4, 3, 5
c) 3, 3, 4, 5, 3, 6
d) 1, 3, 4, 5, 3, 6 (correct)
e) 1, 3, 4, 4, 3, 5
5. The length of 5 meters is the same as (1 in = 2.54 cm)
a) 5 feet
b) 5 yards
c) 5 liters
d) 5  103 mm (correct)
e) 5  10-3 mm
6. How many grams of potatoes are equivalent to 31.2 pounds of potatoes? (1 lb = 453.6
g)
a) 14152 g
b) 10,000 g
c) 1.42  104 g (correct)
d) 0.06878 g
e) 6.88  10-2 g
7. What is the density of a pear that occupies 32 cubic centimeters and has a mass of 42
grams?
a) 2.0 g ∙ cm-3
b) .7619 g ∙ cm-3
c) .76 g ∙ cm-3
d) 1.3125 g ∙ cm-3
e) 1.3 g ∙ cm-3 (correct)
8. A small leak in a water tower drips at a rate of 72 gallons per day. Express this rate
in units of milliliters per minute. (1 gal = 3.785 L)
a) 27.4 mL ∙ min-1
b) 28 mL ∙ min-1
c) 190 mL ∙ min-1 (correct)
d) 1900 mL ∙ min-1
e) 3.2 mL ∙ min-1
9. A small leak in a water tower drips at a rate of 72 gallons per day. The water tower
holds 25 000 gallons of water. How many days will it take to empty the tower at the
given rate?
a) about one month
b) about 1 year (correct)
c) about 5 years
d) about 10 years
e) about 20 years
10. A liquid has a density of 1.8 grams per milliliter. How many grams of the liquid are
in 62 milliliters of the sample?
a) 110 g (correct)
b) 220 g
c) 34 g
d) 0.029 g
e) 0.03 g
11. Density can be measured as
a) lb ∙ ft-3 (correct)
b) lb ∙ ft-1
c) lb ∙ ft-2
d) ft2 ∙ lb-1
e) ft3 ∙ lb-1
12. A liquid has a density of 1.45 grams per milliliter. How many milliters are there in a
45.0 gram sample?
a) 65.3 mL
b) 31.0 mL (correct)
c) 3.22  10-2 mL
d) 70.0 mL
e) 29.0 mL
13. Express 14.3 square centimeters in units of square millimeters.
a) 143 mm2
b) 0.143 mm2
c) 1.43 mm2
d) 1 430 mm2 (correct)
3) 14 300 mm2
14. A star athlete threw a baseball at a velocity of 97 miles per hour. Express this
velocity in units of meters per second. (1 mi = 5280 ft; 1 in = 2.54 cm)
a) 142 m ∙ s-1
b) 361 m ∙ s-1
c) 2600 m ∙ s-1
d) 86 m ∙ s-1
e) 43 m ∙ s-1 (correct)
15. Table sugar, sucrose, is an example of
a) a heterogeneous mixture
b) a homogeneous mixture
c) a mineral
d) an element
e) a compound (correct)
16. Iced tea with lemon, ice, and sugar is an example of
a) a heterogeneous mixture (correct)
b) a homogenous mixture
c) a mineral
d) an element
e) a compound
17. All of the following are considered subatomic particles, except:
a) gamma rays (correct)
b) electrons
c) protons
d) neutrons
e) positrons
18. All of the following are statements from Dalton’s atomic hypothesis, except:
a) All the atoms of a given element are identical.
b) The atoms of different elements have different masses.
c) All atoms are composed of electrons, protons, and neutrons. (correct)
d) A compound is a specific combination of atoms of more than one element.
e) In a chemical reaction, atoms are neither created nor destroyed; they exchange
partners to produce new substances.
19. All of the following statements are true regarding the nuclear model of the atom,
except:
a) The positive charge is densely found in the center of the atom, while the negatively
charged electrons exist in a diffuse cloud outside the nucleus.
b) Most of the space of an atom is empty space.
c) The nuclear model in which the positive charge is held densely in the center of the
atom is no longer accepted, because it was proposed over 100 years ago. (correct)
d) In a neutral atom, the number of protons in the nucleus is equal to the number of
electrons outside the nucleus.
e) One of the most important experiments conducted to reveal the nuclear model of the
atom was to bombard a thin metal sheet with alpha particles and show that some alpha
particles were deflected directly back to the source by the positively charged, dense
nucleus.
21
20. The 10
Ne isotope has:
a) 10 protons, 21 electrons, 11 neutrons
b) 10 protons, 11 electrons, 21 neutrons
c) 10 protons, 10 electrons, 11 neutrons (correct)
d) 21 protons, 11 electrons, 10 neutrons
e) 21 protons, 10 electrons, 11 neutrons
21. The 126 C isotope has:
a) 6 protons, 12 electrons, 6 neutrons
b) 6 protons, 8 electrons, 12 neutrons
c) 6 protons, 6 electrons, 6 neutrons (correct)
d) 12 protons, 12 electrons, 6 neutrons
e) 12 protons, 6 electrons, 6 neutrons
22. Which element is in the same period as carbon?
a) fluorine (correct)
b) silicon
c) lead
d) phosphorus
e) hydrogen
23. Which element is in the same group as calcium?
a) cadmium
b) cesium
c) barium (correct)
d) scandium
e) potassium
24. Which of the following is a halogen?
a) lithium
b) hydrogen
c) helium
d) fluorine (correct)
e) lithium
25. Which of the following is a nonmetal?
a) bromine (correct)
b) lithium
c) antimony
d) vanadium
e) beryllium
26. Identify the symbols for the elements sodium, silicon, boron, calcium, and sulfur,
respectively.
a) S, Si, Bo, Ca, Su
b) S, Si, Bo, Ca, Su
c) Na, S, Bo, C, Su
d) Na, Si, B, C, S
e) Na, Si, B, Ca, S (correct)
27. Which of the following would be considered a binary ionic compound?
a) HCl
b) CO2
c) CO
d) H2S
e) KCl (correct)
28. Which would be considered a binary molecular compound?
a) NaCl
b) CaCl2
c) FeCl3
d) BrCl (correct)
e) BaCl2
29. All of the following monatomic ions have the correct charge, except:
a) Sr2+
b) S2c) S2+ (correct)
d) Mg2+
e) O230. The proper formula unit for the binary compound formed from calcium and fluorine
is:
a) CaF
b) Ca2F
c) CaF2 (correct)
d) Ca2F2
e) Ca3F2
31. All of the following names and formulas are properly matched, except:
a) rubidium chloride, RbCl
b) potassium sulfide, KS (correct)
c) magnesium hydroxide, Mg(OH)2
d) iron (III) chloride, FeCl3
e) lithium nitrate, LiNO3
32. The correct formula for bromine pentachloride is:
a) Br5Cl
b) BrCl5 (correct)
c) BrCl
d) Br4Cl
e) BrCl4
33. The correct name for NH4NO2 is:
a) ammonia hydronitrogen oxide
b) ammonia nitrogen oxide
c) ammonium nitrate
d) ammonium nitrite (correct)
e) ammonium nitrous acid
34. The correct name for SO3 is:
a) sulfur oxide
b) sulfur trioxide (correct)
c) sulfurous acid
d) sulfuric acid
e) trisulfur oxide
35. The correct name for Na2O is:
a) disodium monoxide
b) disodium oxide
c) sodium oxide (correct)
d) sodium dioxide
e) disodium oxyacid
36. The correct name for KClO4 is:
a) krypton chlorine tetroxide
b) krypton oxychlorine
c) potassium chlorine tetroxide
d) potassium perchlorate (correct)
e) potassium perchlorine
37. All of the following hydrocarbons are named correctly with the common names,
except:
a) CH4, carbon tetrahydride (correct)
b) C2H6, ethane
c) C4H10, butane
d) C5H12, pentane
e) C10H22, decane
38. Which of the following is NOT correctly matched?
a) silicon, Si
b) sodium, Na
c) sulfur, S
d) tin, Ti (correct)
e) antimony, Sb
39. Which of the following is NOT correctly matched?
a) boron, B
b) mercury, M (correct)
c) iodine, I
d) oxygen, O
e) potassium, K
40. Which of the following common names is not correctly matched with the formula?
a) NH3, ammonia
b) H2O, water
c) C2H2, dicarbon dihyrdide (correct)
d) C2H4, ethylene
e) N2O, nitrous oxide
41. Which has more molecules: a mole of H2O or a mole of O2?
a) a mole of H2O
b) a mole of O2
c) insufficient information to answer
d) They both have the same number of molecules. (correct)
e) The answer depends on the volume of the container.
42. How many moles of hydrogen are in 3 moles of ammonia, NH3?
a) 3 moles
b) 6 moles
c) 9 moles (correct)
d) 6.0221  1023 moles
e) 1.80663  1023 moles
43. How many atoms of hydrogen are in 3 moles of ammonia, NH3?
a) 3 atoms
b) 9 atoms
c) 6.0221  1023 atoms
d) 1.8066  1023 atoms
e) 5.4199  1024 atoms (correct)
44. How many moles of sodium ions are there in 2.5 moles of sodium chloride, NaCl?
a) 6.0221  1023 moles
b) 1.5055  102 moles
c) 1.0 mole
d) 2.5 moles (correct)
e) 5.0 moles
45. How many moles of glucose are there in 2.4088  1024 molecules of glucose?
a) 4 moles (correct)
b) 2 moles
c) 6.0221  1023 moles
d) 1.4506  1048 moles
e) insufficient information to answer
46. Calculate the molar mass of copper (II) nitrate, Cu(NO3)2.
a) 187.57 g∙mol-1 (correct)
b) 93.56 g∙mol-1
c) 125.56 g∙mol-1
d) 251.12 g∙mol-1
e) 198.45 g∙mol-1
47. Calculate the molar mass of ammonium sulfide, (NH4)2S.
a) 47.08 g∙mol-1
b) 61.09 g∙mol-1
c) 68.14 g∙mol-1 (correct)
d) 62.10 g∙mol-1
e) 75.10 g∙mol-1
48. Calculate the molar mass of glucose, C6H12O6.
a) 29.02 g∙mol-1
b) 116.08 g∙mol-1
c) 156.21 g∙mol-1
d) 174.12 g∙mol-1
e) 180.16 g∙mol-1 (correct)
49. Calculate the number of moles of glucose, C6H12O6, in a 512 gram sample of
glucose.
a) 1.42 moles
b) 2.84 moles (correct)
c) 0.352 moles
d) 9.22  104 moles
e) 1.71  1024 moles
50. Calculate the number of molecules of glucose, C6H12O6, in a 512 gram sample of
glucose.
a) 1.71  1024 molecules (correct)
b) 8.55  1023 molecules
c) 6.0221  1023 molecules
d) 2.84 molecules
e) 9.224  104 molecules
51. How many grams of glucose are in 5.9 moles of glucose?
a) 31 g
b) 3.3  10-2 g
c) 1.1  103 g (correct)
d) 2.0  1022 g
e) 3.3  102 g
52. How many formula units of sodium fluoride, NaF, are in 496 g of sodium fluoride?
a) 11.8 formula units
b) 2.08  104 formula units
c) 1.25  1028 formula units
d) 7.11  1024 formula units (correct)
e) 1.96  10-23 formula units
53. What is the mass percent of oxygen in water?
a) 88.81% (correct)
b) 66.67%
c) 33.33%
d) 11.19%
e) insufficient information to answer
54. A compound containing only nitrogen and oxygen was found to contain 2.1 grams of
nitrogen and 1.2 grams of nitrogen. What is the mass percent composition of oxygen and
nitrogen in this compound?
a) 2.1% N, 1.2% O
b) 75% N, 25% O
c) 25% N, 75% O
d) 64% N, 36% O (correct)
e) 36% N, 64% O
55. Calculate the mass percent composition of sodium nitrate, NaNO3.
a) 27.05% Na, 16.48% N, 56.47% O (correct)
b) 43.38% Na, 26.43% N, 30.19% O
c) 27.05% Na, 16.48% N, 30.10% O
d) 20% Na, 20% N, 60% O
e) 10% Na, 10% N, 30% O
56. The mass percent composition of a particular compound was found to be 65.45%
carbon, 5.492% hydrogen, and 29.06 % oxygen. Determine the empirical formula of this
compound.
a) C7H5O3
b) CHO
c) C3H3O (correct)
d) C6H12O6
e) insufficient information to answer
57. The mass percent composition of a particular compound was found to be 26.95%
sulfur, 14.43% oxygen, and 59.61% chlorine. The molar mass of the compound was
determined to be 118.96 g∙mol-1. Determine the molecular formula for this compound.
a) SOCl
b) S2OCl6
c) SOCl2 (correct)
d) S2O2Cl4
e) S2O2Cl2
58. Determine the empirical formula for a pure sample of a compound that contains 6.3
grams of nitrogen and 3.6 grams of oxygen.
a) N2O6
b) N3O6
c) N6O3
d) N2O (correct)
e) NO2
59. What is the molecular formula of a compound that has an empirical formula of CH
and a molecular mass of 78.53 grams per mole?
a) CH
b) C3H3
c) C6H6 (correct)
d) CH4
e) C6H14
60. Identify the empirical formula of C6H4Cl2.
a) C6H4Cl2
b) C6Cl2H4
c) C12H8Cl4
d) CHCl
e) C3H2Cl (correct)
61. Which of the following is NOT true?
a) A homogeneous mixture can also be referred to as a solution.
b) Within a solution, the component in the least amount is called the solute.
c) Within a solution, the component in the least amount is called the solvent. (correct)
d) A solution in which the solute is water is called an aqueous solution.
e) Solutions can exist in the liquid phase or in the gas phase.
62. All of the following are physical techniques used to separate mixtures, except:
a) filtration
b) chromatography
c) decanting
d) combustion train (correct)
e) distillation
63. What is the molarity of a solution prepared by dissolving 238 grams of potassium
bromide, KBr, in water to make a total of 5.00  102 milliliters of aqueous solution?
a) 4.76  10-1 molar
b) 4.76  101 molar
c) 4.00 molar (correct)
d) 4.00  10-3 molar
e) 5.66  101 molar
64. What is the molarity of a solution prepared by dissolving 457 grams of sodium
nitrate, NaNO3, in water to make a total of 2.00 liters of aqueous solution?
a) 2.69 molar (correct)
b) 9.30  10-2 molar
c) 1.08  102 molar
d) 2.69  10-3 molar
e) 5.38 molar
65. What mass of glucose, C6H12O6, is necessary to prepare 2.50  102 milliliters of a
1.00 molar aqueous solution?
a) 7.20  102 g
b) 4.50  101 g (correct)
c) 2.50  10-1 g
d) 1.00  101 g
e) 2.50  101 g
66. What total volume of a 2.25 molar sodium chloride aqueous solution contains 4.5 
10-1 moles of sodium chloride formula units?
a) 1.0 mole
b) 2.3 mole
c) 2.0  10-1 mole (correct)
d) 2.0  10-2 mole
e) 4.5  10-2 mole
67. How many grams of sodium carbonate, Na2CO3, must be dissolved in 3.75 L of
aqueous solution to yield a molar concentration of 1.75 molar?
a) 2.02  10-2 g
b) 202 g
c) 2.92  10-1 g
d) 696 g (correct)
e) 6.96 g
68. What is the volume of a 1.28 molar aqueous sodium chloride, NaCl, solution that
contains 32 grams of sodium chloride?
a) 7.0  10-1 L (correct)
b) 7.0  102 L
c) 6.8  10-4 L
d) 1.2  104 L
e) 1.4  10-1 L
69. What is the final molar concentration of a sodium hydroxide (NaOH) solution if 25
milliliters of a 0.350 molar NaOH solution is diluted to 1.00 liter?
a) 7.1  10-2 molar
b) 14 molar
c) 1.4 molar
d) 8.75 molar
e) 8.75  10-3 molar (correct)
70. How many milliliters of a 0.100 molar sulfuric acid, H2SO4, solution is needed to
make 25.0 milliliters of a 5.00  10-3 molar solution?
a) 1.25 mL (correct)
b) 800 mL
c) 8.00 mL
d) 125 mL
e) .125 mL
71. When the following chemical reaction is properly balanced the coefficients are:
C3H8 + O2  CO2 + H2O
a) 0, 5, 3, 4
b) 1, 5, 3, 4 (correct)
c) 2, 11, 6, 8
d) 2, 12, 6, 16
e) 3, 13, 9, 12
72. Write the following word equation as a balanced chemical equation: Aluminum
bromide reacts with chlorine to yield aluminum chloride and bromine.
a) AlBr + Cl  AlCl + Br
b) 2AlBr + Cl2  2AlCl + Br2
c) AlBr2 + Cl2  AlCl2 + Br2
d) 2AlBr3 + 2Cl3  2AlCl3 + 6Br
d) 2AlBr3 + 3Cl2  2AlCl3 + 3 Br2 (correct)
73. Write the following word equation as a balanced chemical equation: Copper reacts
with sulfuric acid to yield copper(II)sulfate, water, and sulfur dioxide.
a) Cu + 2 H2SO4  CuSO4 + 2 H2O + SO2 (correct)
b) 2 Cu + 3 H2S  Cu2S + 3 H2O + S2O
c) Cu + H2SO4  Cu2SO4 + H2O + SO2
d) 2 Cu + 2 H2SO4  2 CuSO4 + 4 H2O + S2O
e) Cu + H2S + 3O2  CuSO4 + H2O + SO2
74. Write the following word equation as a balanced chemical equation: Hydrogen gas
reacts with nitric oxide to yield water and nitrogen gas.
a) 2 H + NO  H2O + N
b) H2 + NO  H2O + N
c) 2 H2 + 2NO  2 H2O + N2 (correct)
d) 4 H + 2NO  2 H2O + N2
e) 4 H + 2NO  2 H2O + 2 N
75. When the following chemical equation is balanced, with all whole numbers, the
coefficient for CO2 is:
C8H18 + O2  CO2 + H2O
a) 16 (correct)
b) 12
c) 10
d) 9
e) 8
76. When the following chemical reaction is balanced, with all whole numbers, the
coefficient for oxygen is:
S8 + O2  SO3
a) 1
b) 3
c) 4
d) 6
e) 12 (correct)
77. When the following chemical reaction is balanced, with all whole numbers, the
coefficients are:
FeCl3 + NaOH  Fe(OH)3 + NaCl
a) 1, 3, 1, 3 (correct)
b) 3, 1, 3, 1
c) 3, 2, 3, 2
d) 2, 3, 2, 3
e) 3, 1, 1, 3
78. When the following chemical reaction is balanced, with all whole numbers, the
coefficients are:
Ca(OH)2 + H3PO4  Ca3(PO4)2 + H2O
a) 1, 2, 1, 6
b) 3, 2, 1, 6 (correct)
c) 2, 3, 2, 3
d) 3, 2, 4, 6
e) 3, 2, 3, 2
79. When the following chemical reaction is balanced, with all whole numbers, the
coefficients are:
KClO3  KCl + O2
a) 1, 1, 2
b) 1, 1, 3
c) 2, 1, 3
d) 2, 2, 3 (correct)
e) 2, 2, 2
80. When the following chemical reaction is balanced, with all whole numbers, the
coefficients are:
CO2 + H2O  C6H12O6 + O2
a) 6, 6, 1, 6 (correct)
b) 3, 3, 1, 3
c) 6, 3, 3, 6
d) 12, 3, 2, 6
e) 12, 3, 2, 12
81. Which of the following substances would be considered a weak electrolyte?
a) a strong acid
b) a soluble salt
c) a weak acid (correct)
d) a soluble base
e) an inert gas
82. Which of the following would NOT be classified as a strong acid?
a) HClO3
b) HI
c) HBr
d) HClO4
e) HClO2 (correct)
83. When acetic acid, H3CCOOH, is dissolved in water, all of the following should be
present in the solution, EXCEPT:
a) H3CCOOH
b) H2O
c) H3O+
d) H3C+ (correct)
e) H3CCOO84. What type of reaction is the following?
AgNO3(aq) + NH4Cl(aq)  NH4NO3(aq) + AgCl(s)
a) redox
b) single displacement
c) precipitation (correct)
d) decomposition
e) combustion
85. Which of the following state symbols is not properly defined?
a) (s), solid
b) (l), liquid
c) (g), gas
d) (aq), aqueous
e) They are all correct. (correct)
86. Write the correct balanced precipitation reaction when aqueous lead(II)chloride is
mixed with aqueous lithium sulfate to yield the precipitate lead(II)sulfate.
a) PbCl2(aq) + Li2SO4(aq)  PbSO4(s)
b) PbCl2(aq) + Li2SO4(aq)  PbSO4(s) + 2 LiCl(aq) (correct)
c) PbCl2(aq) + Li2SO4(aq)  PbSO4(s) + 2 LiCl(s)
d) PbCl2(aq) + Li2SO4(aq)  PbSO4(s) + LiCl(aq)
e) Pb2Cl2(aq) + Li2SO4(aq)  Pb2SO4(s) + 2 LiCl(s)
87. The total ionic equation for the following reaction is:
AgNO3(aq) + NaCl(aq)  NaNO3(aq) + AgCl(s)
+
a) Ag (aq) + NO3-(aq) + Na+(aq) + Cl-(aq)  Na+(aq) + NO3-(aq)
b) Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq)  Na+(aq) + NO3-(aq) + AgCl(s) (correct)
c) NO3-(aq) + Na+(aq)  Na+(aq) + NO3-(aq)
d) Ag+(aq) + Cl-(aq)  AgCl(s)
e) Ag+(s) + NO3-(aq) + Na+(aq) + Cl-(s)  Na+(aq) + NO3-(aq) + AgCl(s)
88. The total ionic equation for the following reaction is:
Fe2(SO4)3(aq) + 6NaOH(aq)  2Fe(OH)3(s) + 3Na2SO4(aq)
3+
a) 2Fe (aq) + 3SO42-(aq) + 6Na+(aq) + 6OH-(aq)  2Fe(OH)3(s) + 6Na+(aq)
+ 3SO42-(aq) (correct)
b) 2Fe3+(aq) + 3SO42-(aq) + 6Na+(aq) + 6OH-(aq)  6Na+(aq) + 3SO42-(aq)
c) 3SO42-(aq) + 6Na+(aq)  6Na+(aq) + 3SO42-(aq)
d) 2Fe3+(s) + 3SO42-(aq) + 6Na+(aq) + 6OH-(s)  2Fe(OH)3(s) + 6Na+(aq) + 3SO42-(aq)
e) 2Fe3+(aq) + 6OH-(aq)  2Fe(OH)3(s)
89. The net ionic equation for the following reaction:
AgNO3(aq) + NaCl(aq)  NaNO3(aq) + AgCl(s)
+
a) Ag (aq) + NO3-(aq) + Na+(aq) + Cl-(aq)  Na+(aq) + NO3-(aq)
b) Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq)  Na+(aq) + NO3-(aq) + AgCl(s)
c) NO3-(aq) + Na+(aq)  Na+(aq) + NO3-(aq)
d) Ag+(aq) + Cl- (aq)  AgCl(s) (correct)
e) Ag+(s) + NO3-(aq) + Na+(aq) + Cl-(s)  Na+(aq) + NO3-(aq) + AgCl(s)
90. The net ionic equation for the following reaction is:
HBr (aq) + KOH(aq)  KBr(aq) + H2O(l)
a) H+(aq) + Br-(aq) + K+(aq) + OH-(aq)  K+(aq) + Br-(aq) + H+(aq) + OH-(aq)
b) H+(aq) + Br-(aq) + K+(aq) + OH-(aq)  K+(aq) + Br-(aq) + H2O (l)
c) H+(aq) + Br-(aq) + K+(aq) + OH-(aq)  K+(aq) + Br-(aq) + H+(l) + OH-(l)
d) Br-(aq) + K+(aq)  K+(aq) + Br-(aq)
e) H+(aq) + OH-(aq)  H2O(l) (correct)
91. All of the following are strong bases, EXCEPT:
a) NaOH
b) KOH
c) Ca(OH)2
d) Mg(OH)2 (correct)
e) Ba(OH)2
92. All of the following are strong bases, EXCEPT:
a) NaOH
b) KOH
c) Na2O
d) NH3 (correct)
e) Ba(OH)2
93. Which of the following is a strong acid?
a) HF
b) CH3COOH
c) NH3
d) CH3NH2
e) HI (correct)
94. Of the following, the compound that is classified as a salt is:
a) HF
b) HI
c) NaI (correct)
d) Na2O
e) NaOH
95. When ammonia is combined with hydrochloric acid, the products are:
a) NH4Cl + H2O (correct)
b) NH4Cl + OH- + H2
c) NH3Cl + H2O
d) NH3Cl + H2
e) NH4Cl + OH96. When barium hydroxide is combined with sulfuric acid, the products are:
a) Ba(OH)2 + H2SO4
b) BaSO4 + H2O (correct)
c) BaSO4
d) H2O
e) BaSO4 + H3O+
97. Of the following, the compound that is classified as a salt is:
a) KI (correct)
b) KOH
c) H2O
d) HI
e) H3O+
98. The net ionic equation for the following chemical reaction is:
HF(aq) + KOH(aq)  KF(aq) + H2O(l)
a) HF(aq) + K+(aq) + OH-(aq)  K+(aq) + F-(aq) + H+(l) + OH-(l)
b) HF(aq) + K+(aq) +  K+(aq) + F-(aq) + H+(l)
c) HF(aq) + K+(aq) + OH-(aq)  K+(aq) + F-(aq) + H2O(l)
d) HF(aq) + OH-(aq)  F-(aq) + H2O(l) (correct)
e) HF(aq) + K+(aq)  K+(aq) + H2O(l)
99. The net ionic equation for the following chemical reaction is:
2 CH3COOH(aq) + Ba(OH)2(aq)  Ba(CH3COO)2(aq) + 2H2O(l)
a) 2CH3COO-(aq) + H+(aq) + Ba2+(aq) + 2OH-(aq)  Ba2+(aq) + 2CH3COO-(aq)
+ 2H2O(l)
b) 2H+(aq)+ + 2OH-(aq)  2H2O(l)
c) 2CH3COOH(aq) + 2OH-(aq)  2CH3COO-(aq) + 2H2O(l) (correct)
d) Ba2+(aq) + 2OH-(aq)  Ba2+(aq) + 2H2O(l)
e) 2CH3COO-(aq) + H+(aq) + 2OH-(aq)  2CH3COO-(aq) + 2H2O(l)
100. The total ionic equation for the following reaction is:
2CH3COOH(aq) + Ba(OH)2(aq)  Ba(CH3COO)2(aq) + 2H2O(l)
a) 2CH3COO-(aq) + H+(aq) + Ba2+(aq) + 2OH-(aq)  Ba2+(aq) + 2CH3COO-(aq) +
2H2O(l)
b) 2H+(aq)+ + 2OH-(aq)  2H2O(l)
c) 2CH3COOH(aq) + Ba2+(aq) + 2OH-(aq)  2CH3COO-(aq) + Ba2+(aq) + 2H2O(l)
(correct)
d) Ba2+(aq) +2OH-(aq)  Ba2+(aq) + 2H2O(l)
e) 2CH3COO-(aq) + H+(aq) + 2OH-(aq)  2CH3COO-(aq) + 2H2O(l)
101. Determine the oxidation number on sulfur in SO42-.
a) +4
b) -4
c) +6 (correct)
d) -6
e) -2
102. Determine the oxidation number on phosphorus in P2O5.
a) +1
b) -1
c) +5 (correct)
d) -5
e) +10
103. Determine the oxidation number on chromium in Cr2O72-.
a) +2
b) +3
c) +4
d) +5
e) +6 (correct)
104. Determine the oxidation number on nitrogen in NaNO3.
a) -2
b) -5
c) +2
d) +5 (correct)
e) +6
105. Considering the following reaction, what is undergoing reduction?
2Na + Cl2  2NaCl
a) insufficient information to determine
b) Na and Cl2
c) Na
d) Cl2 (correct)
e) NaCl
106. Considering the following reaction, what is undergoing reduction?
2H2 + O2  2H2O
a) insufficient information
b) H2 and O2
c) H2
d) O2 (correct)
e) H2O
107. Considering the following reaction, what is undergoing oxidation?
Fe + ZnCl2  FeCl2 + Zn
a) Fe and Cl2
b) Fe and Zn
c) Fe (correct)
d) Zn
e) Cl2
108. Considering the following reaction, what is undergoing oxidation?
Cl2 + 2NaBr  Br2 + 2NaCl
a) Na
b) Na and Br2
c) Br- (correct)
d) Cl2
e) Na+
109. Balance the following net ionic redox reaction:
Fe + Ag+  Fe2+ + Ag
a) Fe + Ag+  Fe2+ + Ag
b) 2Fe + Ag+  Fe2+ + 2Ag
c) Fe + 2Ag+  Fe2+ + 2Ag (correct)
d) 2Fe + Ag+  2Fe2+ + Ag
e) Fe + 2Ag+  Fe2+ + Ag
110. Balance the following net ionic redox reaction:
Ca + Sb3+  Ca2+ + Sb
a) Ca + Sb3+  Ca2+ + Sb
b) 2Ca + Sb3+  Ca2+ + 3Sb
c) Ca + 2Sb3+  3Ca2+ + Sb
d) 3Ca + 2Sb3+  3Ca2+ + 2Sb (correct)
e) 2Ca + 3Sb3+  2Ca2+ + 3Sb
111. How many moles of calcium carbonate are produced when 2 moles of calcium
cyanide react with excess water, according to the following balanced equation:
Ca(CN)2 + 3 H2O  CaCO3 + 2NH3
a) 1 mole
b) 2 moles (correct)
c) 3 moles
d) 4 moles
e) insufficient information
112. How many moles of hydrochloric acid are necessary to react completely with 4
moles of aluminum according to the following chemical reaction?
2Al + 6HCl  2AlCl3 + 3H2
a) 1 mole
b) 2 moles
c) 4 moles
d) 8 moles
e) 12 moles (correct)
113. How many moles of hydrogen are necessary to completely react with 10 moles of
carbon monoxide in the following chemical reaction?
CO + 2H2  CH3OH
a) 1 mole
b) 2 moles
c) 5 moles
d) 10 moles
e) 20 moles (correct)
114. Given 4 moles of iron and 6 moles of chlorine, how many moles of iron(III)chloride
can be formed according to the following chemical reaction?
2Fe + 3Cl2  2FeCl3
a) 1 mole
b) 2 moles
c) 3 moles
d) 4 moles (correct)
e) 6 moles
115. Given 8 moles of methane and 12 moles of chlorine, how many moles of carbon
tetrachloride will be formed according to the following chemical reaction?
CH4 + 4Cl2  CCl4 + 4HCl
a) 1 mole
b) 2 moles
c) 3 moles (correct)
d) 8 moles
e) 12 moles
116. Given 8 moles of aluminum in the following chemical reaction, how many moles of
copper(II)sulfate must be supplied to react away all the aluminum?
2Al + 3 CuSO4  Al2(SO4)3 + 3 Cu
a) 2 moles
b) 3 moles
c) 6 moles
d) 8 moles
e) 12 moles (correct)
117. What mass of potassium chloride would be produced upon the decomposition of 15
grams of potassium chlorate, according to the following balanced decomposition
reaction?
2KClO3  2KCl + 3O2
a) 4.5 g
b) 9.1 g (correct)
c) 15 g
d) 18 g
e) 30 g
118. How many grams of oxygen must be supplied to completely burn 26 grams of
acetylene according to the following balanced combustion reaction?
2C2H2 + 5O2  4CO2 + 2H2O
a) 8.5 g
b) 32 g
c) 65 g
d) 80 g (correct)
e) 160 g
119. How many grams of carbon dioxide will be formed by the decomposition of 68
grams of calcium carbonate according to the following balanced decomposition reaction?
CaCO3  CaO + CO2
a) 30 g (correct)
b) 60 g
c) 68 g
d) 130 g
e) 260 g
120. How many grams of water can be produced in the complete combustion (excess
oxygen) of 216 grams of octane according to the following balanced combustion
reaction?
2 C8H18 + 25 O2  16 CO2 + 18 H2O
a) 0.222 g
b) 162 g
c) 254 g
d) 324 g (correct)
e) 1.17  102 g
121. How many grams of water can be produced when 12 grams of zinc oxide react with
12 grams of hydrochloric acid according to the following balanced chemical equation?
ZnO + 2HCl  ZnCl2 + H2O
a) 2.7 g (correct)
b) 6.0 g
c) 12 g
d) 24 g
e) 36 g
122. How many grams of sodium chloride can be formed when 25 grams of
iron(II)chloride react with 50 grams of sodium phosphate according to the following
balance chemical equation?
3FeCl2 + 2Na3PO4  Fe3(PO4)2 + 6NaCl
a) 13 g
b) 23 g (correct)
c) 33 g
d) 50 g
e) 75 g
123. How many grams of water are produced when 45 grams of benzene burn in 15
grams of oxygen according to the following balanced chemical equation?
2C6H6 + 15O2  12CO2 + 6H2O
a) 0.19 g
b) 1.7 g
c) 3.4 g (correct)
d) 31 g
e) 50 g
124. How many grams of nitric oxide are produced when 26 grams of ammonia burn in
26 grams of oxygen according to the following balanced chemical equation?
4NH3 + 5O2  4NO + 6H2O
a) 13 g
b) 20 g (correct)
c) 26 g
d) 46 g
e) 52 g
125. When 26 grams of ammonia burn in 26 grams of oxygen, according to the
following balanced equation, what is the limiting reagent?
4NH3 + 5O2  4NO + 6H2O
a) NH3
b) O2 (correct)
c) NO
d) H2O
e) NH3 and O2
126. When 12 grams of zinc oxide react with 12 grams of hydrochloric acid according to
the following balanced chemical equation, what is the limiting reagent?
ZnO + 2HCl  ZnCl2 + H2O
a) ZnO (correct)
b) HCl
c) ZnCl2
d) H2O
e) ZnO and HCl
127. How many milliliters of a 0.50 molar solution of calcium hydroxide are necessary
to completely neutralize 40 milliliters of a 0.25 molar nitric acid solution according to the
following balanced neutralization reaction?
2HNO3(aq) + Ca(OH)2(aq)  Ca(NO3)2(aq) + H2O(l)
a) 40 mL
b) 20 mL
c) 10 mL (correct)
d) 5 mL
e) 1 mL
128. How many milliliters of a 0.40 molar solution of hydrochloric acid is necessary to
neutralize 25 milliliters of a 0.20 molar sodium hydroxide solution?
a) 50 mL
b) 25 mL
c) 20 mL
d) 12.5 mL (correct)
e) 10.5 mL
129. How many milliliters of a 0.70 molar solution of barium hydroxide, Ba(OH)2, is
necessary to neutralize 55 milliliters of a 1.4 molar solution of sulfuric acid, H2SO4?
a) 220 mL
b) 110 mL (correct)
c) 55 mL
d) 22 mL
e) 11 mL
130. For a particular chemical reaction the theoretical yield was 12 grams of product, but
the actual yield was 3 grams. What is the percent yield of this reaction?
a) 100%
b) 75%
c) 50%
d) 25% (correct)
e) insufficient information
131. For a particular chemical reaction the theoretical yield was 3 grams of product, but
the actual yield was 12 grams. What is the percent yield of this reaction?
a) 100%
b) 75%
c) 50%
d) 25%
e) impossible occurrence (correct)