Chemistry And Chemical Reactivity International Edition 8th Edition By John C. Kotz – Test Bank

Description

Chemistry And Chemical Reactivity International Edition 8th Edition By John C. Kotz – Test Bank

 Sample Questions

Instant Download With Answers

Chapter 2—Atoms, Molecules, and Ions

 

MULTIPLE CHOICE

 

1. Which of the following statements concerning atomic structure is/are correct?

	1.	Neutrons and electrons are found in space as a cloud around the nucleus.
	2.	The nucleus contains all the positive charge of an atom.
	3.	Electrons surround the nucleus and account for the majority of an atom’s volume.

 

a.	1 only
b.	2 only
c.	3 only
d.	2 and 3
e.	1, 2, and 3

 

 

ANS:  D

 

2. Rank the subatomic particles from least to greatest mass.

a.	electron mass = proton mass = neutron mass
b.	electron mass = neutron mass < proton mass
c.	electron mass = proton mass < neutron mass
d.	electron mass < proton mass < neutron mass
e.	electron mass < proton mass = neutron mass

 

 

ANS:  D

 

3. Atomic number is the________ in the nucleus of an atom.

a.	number of electrons
b.	number of protons
c.	number of protons minus the number of neutrons
d.	sum of the number of electrons and neutrons
e.	sum of the number of neutrons and protons

 

 

ANS:  B

 

4. The atomic number of fluorine is ____.

a.	7A
b.	9
c.	10
d.	19
e.	0

 

 

ANS:  B

 

 

 

5. Which of the following statements is/are CORRECT?

	1.	A hydrogen atom with 1 proton and zero neutrons is assigned a mass of exactly 1 atoms mass unit.
	2.	1 atomic mass unit is equivalent to 9.11 ´ 10–28 g.
	3.	A carbon atom with 6 protons and 6 neutrons is assigned a mass of exactly 12 atomic mass units.

 

a.	1 only
b.	2 only
c.	3 only
d.	1 and 2
e.	1, 2, and 3

 

 

ANS:  C

 

6. What is the mass number of an argon atom with 22 neutrons?

a.	2
b.	18
c.	22
d.	40
e.	39.95

 

 

ANS:  D

 

7. How many protons, neutrons, and electrons are in a silver atom with a mass number of 108?

a.	47 protons, 47 neutrons, 61 electrons
b.	47 protons, 61 neutrons, 47 electrons
c.	61 protons, 47 neutrons, 47 electrons
d.	47 protons, 108 neutrons, 47 electrons
e.	61 protons, 108 neutrons, 61 electrons

 

 

ANS:  B

 

8. How many protons, neutrons, and electrons are in a nitrogen-15 atom?

a.	15 protons, 15 neutrons, 15 electrons
b.	15 protons, 7 neutrons, 15 electrons
c.	8 protons, 7 neutrons, 7 electrons
d.	7 protons, 8 neutrons, 7 electrons
e.	8 protons, 7 neutrons, 8 electrons

 

 

ANS:  D

 

9. What is the mass of chlorine-35 relative to carbon-12?

a.	0.657
b.	0.522
c.	1.52
d.	2.92
e.	23

 

 

ANS:  D

 

 

 

10. Which of the following atoms contains the fewest protons?

a.	232Th
b.	231Pa
c.	245Pu
d.	238U
e.	232Pa

 

 

ANS:  A

 

11. Which of the following atoms contains the largest number of protons?

a.	231Pa
b.	238U
c.	232Th
d.	244Pu
e.	244Am

 

 

ANS:  E

 

12. What is the atomic symbol for an element with 39 protons and 50 neutrons?

a.
b.
c.
d.
e.

 

 

ANS:  C

 

13. What is the identity of ?

a.	Ni
b.	Zn
c.	Rn
d.	Ce
e.	Pd

 

 

ANS:  A

 

14. What is the atomic symbol for an element that has 30 neutrons and a mass number of 55?

a.	At
b.	Zn
c.	Co
d.	Mn
e.	Cs

 

 

ANS:  D

 

15. How many neutrons are in an atom of gallium-71?

a.	71
b.	40
c.	111
d.	31
e.	102

 

 

ANS:  B

 

16. Which of the following atoms contains the largest number of neutrons?

a.
b.
c.
d.
e.

 

 

ANS:  E

 

17. Which two of the atoms below have the same number of neutrons?

 

a.	and
b.	and
c.	and
d.	and
e.	and

 

 

ANS:  B

 

18. Two isotopes of a given element will have the same number of ____, but a different number of ____ in their nucleus.

a.	protons, electrons
b.	electrons, protons
c.	protons, neutrons
d.	neutrons, protons
e.	electrons, neutrons

 

 

ANS:  C

 

19. Which of the following are a pair of isotopes?

a.	and
b.	and
c.	and
d.	and
e.	and

 

 

ANS:  E

 

20. The masses of isotopes and their abundances are determined experimentally using

a.	a mass spectrometer.
b.	an analytical balance.
c.	a centrifuge.
d.	filtration followed by distillation.
e.	electrolysis.

 

 

ANS:  A

 

21. Rubidium has two naturally occurring isotopes. The average mass of Rb is 85.4678 u. If 72.15% of Rb is found as Rb-85 (84.9117 u), what is the mass of the other isotope?

a.	0.56 u
b.	85.68 u
c.	86.91 u
d.	86.02 u
e.	83.47 u

 

 

ANS:  C

 

22. An element consists of three isotopes. The abundance of one isotope is 92.21% and its atomic mass is 27.97693 u. The abundance of the second isotope is 4.70% and its atomic mass is 28.97649 u. The atomic mass of the third isotope is 29.97376 u. What is the average atomic mass of the element?

a.	28.09 u
b.	28.98 u
c.	28.96 u
d.	29.87 u
e.	29.07 u

 

 

ANS:  A

 

23. Copper has an average atomic mass of 63.55 u. If 69.17% of Cu exists as Cu-63 (62.93960 u), what is the identity and the atomic mass of the other isotope?

a.	Cu-64; 63.82 u
b.	Cu-64; 64.16 u
c.	Cu-65; 64.16 u
d.	Cu-65; 64.92 u
e.	Cu-66; 65.91 u

 

 

ANS:  D

 

24. Silver has two stable isotopes with masses of 106.90509 u and 108.9047 u. The average molar mass of silver is 107.868 u. What is the percent abundance of each isotope?

a.	50.0% Ag-107 and 50.0% Ag-109
b.	51.8% Ag-107 and 48.2% Ag-109
c.	55.4% Ag-107 and 44.6% Ag-109
d.	48.2% Ag-107 and 51.8% Ag-109
e.	44.6% Ag-107 and 55.4% Ag-109

 

 

ANS:  B

 

25. Group 1A elements are also known as

a.	alkaline earth metals.
b.	alkali metals.
c.	chalcogens.
d.	halogens.
e.	noble gases.

 

 

ANS:  B

 

 

 

26. Which of the following statements is/are CORRECT?

	1.	The group 3A elements are also known as the chalcogens.
	2.	The noble gases are sometimes called the rare gases because of their low abundances.
	3.	The halogens, or group 7A elements, all exist as diatomic molecules.

 

a.	1 only
b.	2 only
c.	3 only
d.	2 and 3
e.	1, 2, and 3

 

 

ANS:  D

 

27. What element is in the fourth period in Group 3A?

a.	Sb
b.	Ga
c.	In
d.	Si
e.	Tl

 

 

ANS:  B

 

28. What halogen is in the third period?

a.	S
b.	Cl2
c.	I2
d.	H2
e.	Ar

 

 

ANS:  B

 

29. Which three elements are likely to have similar chemical and physical properties?

a.	boron, silicon, and germanium
b.	sodium, magnesium, and aluminum
c.	sodium, potassium, and rubidium
d.	oxygen, sulfur, and chlorine
e.	carbon, nitrogen, and oxygen

 

 

ANS:  C

 

30. In which group of the following groups of the periodic table are all the elements nonmetals?

a.	2A
b.	3A
c.	5A
d.	6A
e.	7A

 

 

ANS:  E

 

 

 

31. Which of the following elements is not a metalloid?

a.	boron
b.	selenium
c.	germanium
d.	arsenic
e.	silicon

 

 

ANS:  B

 

32. The formula of acetic acid, CH₃CO₂H, is an example of a(n)

a.	condensed formula.
b.	empirical formula.
c.	structural formula.
d.	ionic compound formula.
e.	mass spectrum.

 

 

ANS:  A

 

33. C₂H₂F₄ is the formula for two possible molecules. C₂H₂F₄ is an example of a(n)

a.	structural formula.
b.	empirical formula.
c.	condensed formula.
d.	space-filling model.
e.	molecular formula.

 

 

ANS:  E

 

34. Which element is most likely to form a 2– ion?

a.	K
b.	Mg
c.	P
d.	Br
e.	S

 

 

ANS:  E

 

35. Which atom is most likely to form a 2+ ion?

a.	scandium
b.	calcium
c.	aluminum
d.	oxygen
e.	fluorine

 

 

ANS:  B

 

36. Identify the ions present in Na₂SO₄.

a.	Na+, S2–, and O2–
b.	Na+, S2+, and O2–
c.	Na+ and SO42–
d.	Na+, S2–, and O2+
e.	Na+ and SO4–

 

 

ANS:  C

 

 

37. Identify the ions in CaHPO₄.

a.	Ca2+ and PO43–
b.	Ca2+ and HPO42–
c.	Ca+ and HPO4–
d.	Ca3+ and HPO43–
e.	Ca2+, H+, P3–, and O2–

 

 

ANS:  B

 

38. What charge is likely on a monatomic silver cation?

a.	2–
b.	1–
c.	1+
d.	2+
e.	3+

 

 

ANS:  C

 

39. For a nonmetal in Group 6A of the periodic table, the most common monatomic ion will have a charge of ____.

a.	3–
b.	2–
c.	1–
d.	1+
e.	2+

 

 

ANS:  B

 

40. What is the correct formula for an ionic compound that contains magnesium ions and phosphide ions?

a.	MgP
b.	MgP2
c.	Mg3P2
d.	Mg3(PO4)2
e.	Mg2P3

 

 

ANS:  C

 

41. Which of the following formulas is not correct?

a.	AlPO4
b.	KClO4
c.	CaS
d.	Na(NO3)2
e.	Na2HPO4

 

 

ANS:  D

 

42. What is the correct formula for an ionic compound that contains barium ions and carbonate ions?

a.	BaCO3
b.	Ba(HCO3)2
c.	Ba2CO3
d.	Ba2C
e.	Ba(CO3)2

 

 

ANS:  A

 

43. Sodium sulfate has the chemical formula Na₂SO₄. Based on this information, the formula for chromium(III) sulfate is ____.

a.	CrSO4
b.	Cr(SO4)3
c.	Cr2(SO4)3
d.	Cr2SO4
e.	Cr3(SO4)2

 

 

ANS:  C

 

44. What is the charge on the copper ion in Cu₃P?

a.	3–
b.	1–
c.	0
d.	1+
e.	3+

 

 

ANS:  D

 

45. What is the correct formula for calcium nitrate?

a.	CaN
b.	Ca3N2
c.	CaNO2
d.	Ca3(NO3)2
e.	Ca(NO3)2

 

 

ANS:  E

 

46. What is the correct formula for potassium dihydrogen phosphate?

a.	KH2PO4
b.	K2HPO4
c.	K2H2PO4
d.	K3H2PO4
e.	KH2P

 

 

ANS:  A

 

47. What is the correct formula for ammonium bromide?

a.	NH4Br
b.	(NH4)2Br
c.	NH3Br
d.	NH4Br2
e.	NH2Br

 

 

ANS:  A

 

48. What is the correct formula for cobalt(III) bromide?

a.	CoBr
b.	CoBr3
c.	Co2Br3
d.	Co3Br2
e.	Co3Br

 

 

ANS:  B

 

 

49. What is the correct formula for iron(II) nitrate?

a.	Fe2(NO3)2
b.	Fe2NO3
c.	Fe(NO3)2
d.	Fe3N2
e.	FeNO3

 

 

ANS:  C

 

50. What is the correct name for NH₄NO₃?

a.	ammonia hydrogen nitrate
b.	ammonia hydrogen nitride
c.	ammonium nitric acid
d.	ammonium nitrate
e.	ammonium nitride

 

 

ANS:  D

 

51. What is the correct name for SrCl₂?

a.	strontium dichloride
b.	strontium dichlorine
c.	strontium(II) dichloride
d.	strontium chloride
e.	iodine strontide

 

 

ANS:  D

 

52. What is the correct name for MnS?

a.	manganese sulfide
b.	dimanganese sulfate
c.	dimanganese sulfide
d.	manganese(II) sulfate
e.	manganese(II) sulfide

 

 

ANS:  E

 

53. What is the correct name for Ca(CH₃CO₂)₂?

a.	calcium(II) carbonate
b.	calcium carbonate
c.	calcium acetate
d.	acetic calcide
e.	calcium carbonide

 

 

ANS:  C

 

 

54. Which of the following statements concerning ionic compounds is/are correct?

	1.	As ion charges increase, the attraction between oppositely charged ions increases.
	2.	Although not electrically conductive like metals, ionic compounds are malleable.
	3.	Positive and negative ions are attracted to each other by electrostatic forces.

 

a.	1 only
b.	2 only
c.	3 only
d.	1 and 3
e.	1, 2, and 3

 

 

ANS:  D

 

55. Predict which ionic compound has the highest melting point.

a.	KBr
b.	MgO
c.	RbI
d.	CaBr2
e.	CsCl

 

 

ANS:  B

 

56. What is the correct name for N₂O₄?

a.	nitrogen oxide
b.	dinitrogen tetraoxide
c.	nitrogen(II) oxide
d.	nitrogen tetraoxide
e.	dinitrogen tetraoxygen

 

 

ANS:  B

 

57. What is the correct name for CCl₄?

a.	carbon chlorine
b.	tetracarbon chloride
c.	carbon tetrachloride
d.	carbon(IV) chloride
e.	tetrachlorocarbide

 

 

ANS:  C

 

58. What is the common name for PH₃?

a.	laughing gas
b.	hydrazine
c.	nitroglycerin
d.	ammonia
e.	phosphine

 

 

ANS:  E

 

 

59. You have 2.50 g of each of the following elements: Ca, Cu, Cs, C, and Cr. Which sample contains the largest number of atoms?

a.	Ca
b.	Cu
c.	Cs
d.	C
e.	Cr

 

 

ANS:  D

 

60. Calculate the number of moles in 0.48 g Cu.

a.	0.033 mol
b.	0.48 mol
c.	31 mol
d.	7.6 ´ 10–3 mol
e.	1.3 ´ 102 mol

 

 

ANS:  D

 

61. What is the mass of 0.71 mol Na?

a.	1.2 ´ 10–24 g
b.	12 g
c.	16 g
d.	0.031 g
e.	32 g

 

 

ANS:  C

 

62. A 0.0050 g sample of boron contains ____ B atoms.

a.	4.6 ´ 10–4
b.	7.7 ´ 10–28
c.	2.8 ´ 1020
d.	3.1 ´ 1021
e.	3.3 ´ 1022

 

 

ANS:  C

 

63. The molar mass of platinum is 195.08 g/mol. What is the mass of 1.00 ´ 10² Pt atoms?

a.	8.51 ´ 10–25 g
b.	3.24 ´ 10–24 g
c.	1.67 ´ 10–22 g
d.	3.24 ´ 10–22 g
e.	3.24 ´ 10–20 g

 

 

ANS:  E

 

64. What mass of Al contains the same number of atoms as 3.0 g Pb?

a.	23 g
b.	0.014 g
c.	3.0 g
d.	0.39 g
e.	0.11 g

 

 

ANS:  D

 

65. A nail is coated with a 0.053 cm thick layer of zinc. The surface area of the nail is 8.59 cm². The density of zinc is 7.13 g/cm³. How many zinc atoms are used in the coating?

a.	5.9 ´ 1020 atoms
b.	3.0 ´ 1022 atoms
c.	3.8 ´ 1022 atoms
d.	2.0 ´ 1024 atoms
e.	1.3 ´ 1026 atoms

 

 

ANS:  B

 

66. What is the molar mass of calcium chloride hexahydrate?

a.	75.53 g/mol
b.	111.0 g/mol
c.	117.0 g/mol
d.	183.6 g/mol
e.	219.1 g/mol

 

 

ANS:  E

 

67. What is the molar mass of sodium sulfate?

a.	55.06 g/mol
b.	119.1 g/mol
c.	78.05 g/mol
d.	142.0 g/mol
e.	110.0 g/mol

 

 

ANS:  D

 

68. Calculate the number of moles of aluminum oxide in 6.83 g Al₂O₃.

a.	6.70 ´ 10–2 mol
b.	6.96 ´ 102 mol
c.	0.253 mol
d.	0.127 mol
e.	1.56 ´ 10–3 mol

 

 

ANS:  A

 

69. What is the mass of 8.04 ´ 10^–3 mol O₂?

a.	2.51 ´ 10–4 g
b.	5.03 ´ 10–4 g
c.	0.129 g
d.	3.89 g
e.	0.257 g

 

 

ANS:  E

 

70. What is the mass of 0.50 mol chromium(III) sulfide?

a.	2.5 ´ 10–3 g
b.	5.9 ´ 10–3 g
c.	42 g
d.	1.0 ´ 102 g
e.	110 g

 

 

ANS:  D

 

71. How many hydrogen atoms are present in 1.0 g of NH₃?

a.	0.059 atoms
b.	0.18 atoms
c.	3.5 ´ 1022 atoms
d.	1.1 ´ 1023 atoms
e.	1.2 ´ 1022 atoms

 

 

ANS:  D

 

72. How many bromide ions are in 0.55 g of iron(III) bromide?

a.	1.1 ´ 1021 ions
b.	3.4 ´ 1021 ions
c.	3.3 ´ 1023 ions
d.	9.9 ´ 1023 ions
e.	2.9 ´ 1026 ions

 

 

ANS:  B

 

73. If 1.00 g of an unknown molecular compound contains 8.35 ´ 10²¹ molecules, what is its molar mass?

a.	44.0 g/mol
b.	66.4 g/mol
c.	72.1 g/mol
d.	98.1 g/mol
e.	132 g/mol

 

 

ANS:  C

 

74. What is the mass percent of chlorine in magnesium chloride?

a.	25.53%
b.	37.24%
c.	40.67%
d.	59.33%
e.	74.47%

 

 

ANS:  E

 

75. What is the mass percent of each element in sulfuric acid, H₂SO₄?

a.	2.055% H, 32.69% S, 65.25% O
b.	1.028% H, 32.69% S, 66.28% O
c.	28.57% H, 14.29% S, 57.17% O
d.	1.028% H, 33.72% S, 65.25% O
e.	2.016% H, 32.07% S, 65.91% O

 

 

ANS:  A

 

76. Nitrogen and oxygen form an extensive series of oxides with the general formula N_xO_y. What is the empirical formula for an oxide that contains 30.44% by mass nitrogen?

a.	N2O
b.	NO
c.	NO2
d.	N2O3
e.	N2O5

 

 

ANS:  C

 

77. A molecule is found to contain 47.35% by mass C, 10.60% by mass H, and 42.05% by mass O. What is the empirical formula for this molecule?

a.	C2H6O
b.	C3H4O
c.	C3H8O2
d.	C4H6O2
e.	C4H8O3

 

 

ANS:  C

 

78. An ionic compound has the formula MCl₂. The mass of 0.3011 mol of the compound is 62.69 grams. What is the identity of the metal?

a.	Ni
b.	Cu
c.	Sn
d.	Hg
e.	Ba

 

 

ANS:  E

 

79. A 3.592 g sample of hydrated magnesium bromide, MgBr₂×xH₂O, is dried in an oven. When the anhydrous salt is removed from the oven, its mass is 2.263 g. What is the value of x?

a.	1
b.	3
c.	6
d.	8
e.	12

 

 

ANS:  C

 

80. A 2.000 g sample of MgCl₂×xH₂O is dried in an oven. When the anhydrous salt is removed from the oven, its mass is 0.9366 g. What is the value of x?

a.	1
b.	3
c.	6
d.	8
e.	12

 

 

ANS:  C

 

SHORT ANSWER

 

81. Buckminsterfullerene is a molecule composed of sixty ________ atoms.

 

ANS:

carbon

 

82. Pure oxygen can exist as O₂ or O₃. Elements that exist in more than one distinct form are called ________.

 

ANS:

allotropes

 

 

83. Oxygen and ________ are the two most abundant elements in the Earth’s crust.

 

ANS:

silicon

 

 

84. What are the names of four metalloids?

 

ANS:

boron, silicon, germanium, arsenic, (antimony, and tellurium)

 

 

85. In reactions, metals generally lose electrons to become ________, and nonmetals gain electrons to become anions.

 

ANS:

cations

 

 

86. In which ionic compound, NaBr or KBr, is the force of attraction between anions and cations stronger?

 

ANS:

The force of attraction is stronger for NaBr. The electrostatic attraction between anions and cations decreases as the separation of the ions increases. The potassium ion will be farther from the bromide ion than the sodium ion due to its larger ionic radius.

 

 

87. The numerical quantity of a mole, 6.022 ´ 10²³, is defined as the number of atoms in a specific mass of an element. What is the mass and the identity of the element used to define one mole?

 

ANS:

A mole is equal to the number of atoms in 12.00 grams of carbon-12.

Chapter 4—Stoichiometry: Quantitative Information about Chemical Reactions

 

MULTIPLE CHOICE

 

1. Iron reacts with oxygen to produce iron(III) oxide.

4 Fe(s) + 3 O₂(g) ® 2 Fe₂O₃(s)

If 3.2 moles of Fe react with excess O₂, how many moles of Fe₂O₃ can be formed?

a.	1.6 mol
b.	2.4 mol
c.	3.2 mol
d.	4.3 mol
e.	6.4 mol

 

 

ANS:  A

 

 

2. Potassium reacts with chlorine gas to produce potassium chloride. How many moles of K will react with 0.40 moles of Cl₂?

a.	0.20 mol
b.	0.32 mol
c.	0.40 mol
d.	0.60 mol
e.	0.80 mol

 

 

ANS:  E

 

 

3. The complete combustion of 0.20 moles of propane, C₃H₈, will

a.	consume 0.20 mol O2 and produce 0.20 mol CO2.
b.	consume 0.20 mol O2 and produce 0.40 mol CO2.
c.	consume 1.0 mol O2 and produce 0.60 mol CO2.
d.	consume 1.0 mol O2 and produce 3.0 mol CO2.
e.	consume 1.0 mol O2 and produce 0.80 mol CO2.

 

 

ANS:  C

 

4. Aluminum reacts with hydrochloric acid to produce aluminum chloride and hydrogen gas.

2 Al(s) + 6 HCl(aq) ® 2 AlCl₃(aq) + 3 H₂(g)

What mass of H₂(g) is produced from the reaction of 0.75 g Al(s) with excess hydrochloric acid?

a.	0.056 g
b.	0.084 g
c.	0.17 g
d.	1.1 g
e.	2.3 g

 

 

ANS:  B

 

 

5. The reaction of coal and water at a high temperature produces a mixture of hydrogen and carbon monoxide gases. This mixture is known as synthesis gas (or syngas). What mass of water is required for the formation of 175 grams of carbon monoxide?

C(s) + H₂O(g) ® H₂(g) + CO(g)

a.	272 g
b.	315 g
c.	489 g
d.	113 g
e.	175 g

 

 

ANS:  D

 

6. When strongly heated, boric acid breaks down to boric oxide and water. What mass of boric oxide is formed from the decomposition of 15.0 g B(OH)₃?

2 B(OH)₃(s) ® B₂O₃(s) + 3 H₂O(g)

a.	7.50 g
b.	15.0 g
c.	8.44 g
d.	16.9 g
e.	33.8 g

 

 

ANS:  C

 

 

7. If the complete combustion of an unknown mass of ethylene produces 16.0 g CO₂, what mass of ethylene is combusted?

C₂H₄(g) + 3 O₂(g) ® 2 CO₂(g) + 2 H₂O(g)

a.	0.182 g
b.	0.364 g
c.	5.10 g
d.	8.00 g
e.	12.6 g

 

 

ANS:  C

 

8. Nitroglycerine decomposes violently according to the chemical equation below. What mass of carbon dioxide gas is produced from the decomposition of 5.00 g C₃H₅(NO₃)₃?

4 C₃H₅(NO₃)₃() ® 12 CO₂(g) + 6 N₂(g) +10 H₂O(g) + O₂(g)

a.	15.0 g
b.	0.969 g
c.	11.6 g
d.	2.91 g
e.	0.323 g

 

 

ANS:  D

 

 

 

9. The compound P₄S₃ is used in matches. It reacts with oxygen to produce P₄O₁₀ and SO₂. The unbalanced chemical equation is shown below.

P₄S₃(s) + O₂(g) ® P₄O₁₀(s) + SO₂(g)

What mass of SO₂ is produced from the combustion of 0.401 g P₄S₃?

a.	0.134 g
b.	1.20 g
c.	0.0389 g
d.	0.117 g
e.	0.350 g

 

 

ANS:  E

 

10. What mass of water is produced by the complete combustion of 2.68 grams of ethanol, C₂H₅OH?

a.	1.05 g
b.	1.17 g
c.	3.14 g
d.	0.439 g
e.	20.6 g

 

 

ANS:  C

 

 

11. Hydrogen peroxide decomposes into oxygen and water. What mass of oxygen is formed from the decomposition of 125 g of H₂O₂?

a.	58.8 g
b.	66.4 g
c.	107 g
d.	118 g
e.	125 g

 

 

ANS:  A

 

 

12. How many moles of sodium bromide can be produced from the reaction of 1.03 moles of sodium with 0.650 moles of bromine gas?

2 Na(s) + Br₂(g) ® 2 NaBr(s)

a.	0.650 mol
b.	1.03 mol
c.	1.30 mol
d.	2.06 mol
e.	0.515 mol

 

 

ANS:  B

 

13. How many moles of Mg₃P₂(s) can be produced from the reaction of 0.14 mol Mg(s) with 0.020 mol P₄(s)?

6 Mg(s) + P₄(s) ® 2 Mg₃P₂(s)

a.	0.047 mol
b.	0.14 mol
c.	0.42 mol
d.	0.020 mol
e.	0.040 mol

 

 

ANS:  E

 

 

14. Nitric oxide is made from the oxidation of ammonia. What mass of nitric oxide can be made from the reaction of 8.00 g NH₃ with 17.0 g O₂?

4 NH₃(g) + 5 O₂(g) ® 4 NO(g) + 6 H₂O(g)

a.	4.54 g
b.	12.8 g
c.	14.1 g
d.	15.9 g
e.	25.0 g

 

 

ANS:  B

 

15. If 5.00 g Br₂ and 1.10 g NH₃ react according to the equation below, what is the maximum mass of ammonium bromide produced?

3 Br₂() + 8 NH₃(g) ® 6 NH₄Br(s) + N₂(g)

a.	3.06 g
b.	6.13 g
c.	12.9 g
d.	4.74 g
e.	8.43 g

 

 

ANS:  D

 

16. What mass of iron can be produced from the reaction of 175 kg Fe₂O₃ with 385 kg CO?

Fe₂O₃(s) + 3 CO(g) ® 2 Fe(s) + 3 CO₂(g)

a.	2.19 kg
b.	30.6 kg
c.	61.2 kg
d.	122 kg
e.	512 kg

 

 

ANS:  D

 

17. Magnesium reacts with iodine gas at high temperatures to form magnesium iodide. What mass of MgI₂ can be produced from the reaction of 5.15 g Mg and 50.0 g I₂?

a.	29.5 g
b.	44.9 g
c.	54.8 g
d.	55.2 g
e.	58.9 g

 

 

ANS:  C

 

18. Aspirin (C₉H₈O₄) is produced by the reaction of salicylic acid (M = 138.1 g/mol) and acetic anhydride (M = 102.1 g/mol).

C₇H₆O₃(s) + C₄H₆O₃() ® C₉H₈O₄(s) + C₂H₄O₂()

If you react 2.00 g C₇H₆O₃ with 1.60 g C₄H₆O₃, what mass of aspirin (M = 180.2 g/mol) can theoretically be obtained?

a.	0.40 g
b.	2.61 g
c.	2.82 g
d.	1.53 g
e.	3.60 g

 

 

ANS:  B

 

19. Aspirin is produced by the reaction of salicylic acid (M = 138.1 g/mol) and acetic anhydride (M = 102.1 g/mol).

C₇H₆O₃(s) + C₄H₆O₃() ® C₉H₈O₄(s) + C₂H₄O₂()

If 2.04 g of C₉H₈O₄ (M = 180.2 g/mol) is produced from the reaction of 3.03 g C₇H₆O₃ and 4.01 g C₄H₆O₃, what is the percent yield?

a.	28.8%
b.	29.0%
c.	50.9%
d.	51.6%
e.	67.3%

 

 

ANS:  D

 

20. Under certain conditions the reaction of ammonia with excess oxygen will produce a 29.5% yield of NO. What mass of NH₃ must react with excess oxygen to yield 157 g NO?

4 NH₃(g) + 5 O₂(g) ® 4 NO(g) + 6 H₂O(g)

a.	89.1 g
b.	302 g
c.	263 g
d.	26.3 g
e.	938 g

 

 

ANS:  B

 

21. If 15.0 g N₂ and 2.00 g H₂ react to produce 1.38 g NH₃, what is the percent yield of the reaction?

N₂(g) + 3 H₂(g) ® 2 NH₃(g)

a.	7.57%
b.	12.2%
c.	8.12%
d.	15.1%
e.	8.17%

 

 

ANS:  B

 

22. Sulfur hexafluoride is produced by reacting elemental sulfur with fluorine gas.

S₈(s) + 24 F₂(g) ® 8 SF₆(g)

What is the percent yield if 18.3 g SF₆ is isolated from the reaction of 10.0 g S₈ and 30.0 g F₂?

a.	40.2%
b.	45.8%
c.	47.6%
d.	54.6%
e.	61.0%

 

 

ANS:  C

 

 

23. A mass of 4.561 g of a metal carbonate, MCO₃, is heated to drive off carbon dioxide. The remaining metal oxide has a mass of 3.544 g.

MCO₃(s) ® MO(s) + CO₂(g)

What is the identity of the metal?

a.	Ni
b.	Ba
c.	Ca
d.	Co
e.	Mg

 

 

ANS:  B

 

24. A mixture of MnSO₄ and MnSO₄×4H₂O has a mass of 2.005 g. After heating to drive off all the water the mass is 1.780 g. What is the mass percent of MnSO₄×4H₂O in the mixture?

a.	11.2%
b.	34.7%
c.	65.3%
d.	69.6%
e.	88.8%

 

 

ANS:  B

 

25. A 1.850 g mixture of SrCO₃ and SrO is heated. The SrCO₃ decomposes to SrO and CO₂. What was the mass percentage of SrCO₃ in the mixture if the mass after heating is 1.445 g?

a.	26.6%
b.	21.9%
c.	13.7%
d.	73.4%
e.	78.1%

 

 

ANS:  D

 

26. A 7.3648 g sample of an oxide of mercury, when heated in a stream of hydrogen, produces Hg() and 0.6126 g H₂O. What is formula for the compound?

a.	Hg2O
b.	HgO
c.	Hg2O3
d.	Hg2O5
e.	HgO2

 

 

ANS:  B

 

27. The reaction of 0.779 g K with O₂ forms 1.417 g potassium superoxide, a substance used in self-contained breathing devices. Determine the formula for potassium superoxide.

a.	KO2
b.	KO
c.	K2O3
d.	K2O
e.	KO4

 

 

ANS:  A

 

 

28. A 1.5991 g sample of a hydrocarbon is combusted to give 1.6918 g of H₂O and 5.1661 g of CO₂. What is the empirical formula of the compound?

a.	CH
b.	CH2
c.	C2H3
d.	C3H4
e.	C5H8

 

 

ANS:  E

 

29. The combustion of 0.0272 mole of a hydrocarbon produces 1.9609 g H₂O and 3.5927 g CO₂. What is the molar mass of the hydrocarbon?

a.	16.0 g/mol
b.	30.1 g/mol
c.	44.1 g/mol
d.	72.2 g/mol
e.	92.1 g/mol

 

 

ANS:  C

 

30. Polyethylene is a polymer consisting of only carbon and hydrogen. If 2.300 g of the polymer is burned in oxygen it produces 2.955 g H₂O and 7.217 g CO₂. What is the empirical formula of polyethylene?

a.	CH
b.	CH2
c.	C2H3
d.	C5H8
e.	C7H8

 

 

ANS:  B

 

31. Soft drink bottles are made of polyethylene terephthalate (PET), a polymer composed of carbon, hydrogen, and oxygen. If 1.9022 g PET is burned in oxygen it produces 0.6585 g H₂O and 4.0216 g CO₂. What is the empirical formula of PET?

a.	CHO
b.	CH7O5
c.	C5H7O
d.	C8H10O
e.	C10H8O5

 

 

ANS:  E

 

32. An unknown hydrocarbon contains carbon, hydrogen, and oxygen. Combustion of 1.5000 g of the hydrocarbon produces 1.1738 g H₂O and 2.1505 g CO₂. What is the empirical formula of the hydrocarbon?

a.	CHO
b.	C2H3O
c.	C3H4O
d.	C3H8O3
e.	C5H5O

 

 

ANS:  D

 

 

33. Naphthalene, a hydrocarbon, has an approximate molar mass of 128 g/mole. If the combustion of 0.6400 g naphthalene produces 0.3599 g H₂O and 2.1977 g CO₂, what is the molecular formula of this compound?

a.	C8H32
b.	C9H18
c.	C9H20
d.	C10H8
e.	C11H7

 

 

ANS:  D

 

34. If 4.49 g NaNO₃ is dissolved in enough water to make 250.0 mL of solution, what is the molarity of the sodium nitrate solution?

a.	1.80 ´ 10–2 M
b.	5.28 ´ 10–2 M
c.	2.11 ´ 10–1 M
d.	1.32 ´ 10–2 M
e.	18.0 M

 

 

ANS:  C

 

35. How many liters of 0.1107 M KCl(aq) contain 2.50 g of KCl?

a.	0.277 L
b.	0.303 L
c.	3.71 ´ 10–3 L
d.	3.30 L
e.	5.94 ´ 10–4 L

 

 

ANS:  B

 

 

36. If 5.15 g Fe(NO₃)₃ is dissolved in enough water to make exactly 150.0 mL of solution, what is the molar concentration of nitrate ion?

a.	0.00319 M
b.	0.0343 M
c.	0.142 M
d.	0.313 M
e.	0.426 M

 

 

ANS:  E

 

 

37. What is the mass of potassium iodide in 50.0 mL of 5.75 ´ 10^–2 M KI(aq)?

a.	2.88 ´ 10–2 g
b.	191 ´ 10–1 g
c.	6.92 ´ 10–3 g
d.	4.77 ´ 10–1 g
e.	191 ´ 102 g

 

 

ANS:  D

 

 

 

38. If 25.00 mL of 1.50 M HCl(aq) is diluted with water to a volume of 750.0 mL, what is the molarity of the diluted HCl(aq)?

a.	2.22 ´ 10–2 M
b.	5.00 ´ 10–2 M
c.	2.07 ´ 10–3 M
d.	4.50 ´ 101 M
e.	1.35 ´ 103 M

 

 

ANS:  B

 

 

39. What volume of 3.0 M HNO₃(aq) must be diluted to make 4.0 L of 0.20 M HNO₃(aq)?

a.	6.0 L
b.	0.15 L
c.	0.20 L
d.	0.27 L
e.	2.4 L

 

 

ANS:  D

 

 

40. What is the pH of 3.5 ´ 10^–3 M HCl(aq)?

a.	–1.01
b.	2.46
c.	3.50
d.	1.01
e.	5.65

 

 

ANS:  B

 

41. The pH of an aqueous NaOH solution is 12.83. What is the hydrogen ion concentration of this solution?

a.	1.5 ´ 10–13 M
b.	6.7 ´ 10–2 M
c.	1.2 M
d.	6.7 ´ 1012 M
e.	2.7 ´ 10–6 M

 

 

ANS:  A                    PTS

 

42. The pH of a vinegar solution is 4.15. What is the H₃O⁺ concentration of the solution?

a.	7.1 ´ 10–5 M
b.	1.6 ´ 10–2 M
c.	0.62 M
d.	1.4 M
e.	1.4 ´ 104 M

 

 

ANS:  A

 

 

43. An aqueous nitric acid solution has a pH of 2.15. What mass of HNO₃ is present in 20.0 L of this solution?

a.	0.11 g
b.	0.022 g
c.	3.7 g
d.	6.8 g
e.	8.9 g

 

 

ANS:  E

 

44. Zn reacts with hydrochloric acid.

Zn(s) + 2 HCl(aq) ® ZnCl₂(aq) + H₂(g)

What volume of 3.05 M HCl(aq) will react with 25.0 g Zn(s)?

a.	0.251 L
b.	4.01 L
c.	0.125 L
d.	0.0627 L
e.	2.33 L

 

 

ANS:  A

 

45. What volume of 0.250 M KCl(aq) will completely react with 50.0 mL of 0.115 M Pb(NO₃)₂(aq)?

2 KCl(aq) + Pb(NO₃)₂(aq) ® PbSO₄(s) + 2 KNO₃(aq)

a.	23.0 mL
b.	46.0 mL
c.	11.5 mL
d.	109 mL
e.	218 mL

 

 

ANS:  B

 

46. A mass of 0.4113 g of an unknown acid, HA, is titrated with NaOH. If the acid reacts with 28.10 mL of 0.1055 M NaOH(aq), what is the molar mass of the acid?

a.	2.965 ´ 10–3 g/mol
b.	9.128 g/mol
c.	138.7 g/mol
d.	337.3 g/mol
e.	820.7 g/mol

 

 

ANS:  C

 

47. A 25.00 mL sample of NaOH is titrated with 26.14 mL of 0.1750 M HCl(aq). What is the concentration of the NaOH solution?

a.	1.995 ´ 10–4 M
b.	0.09149 M
c.	0.1830 M
d.	0.1674 M
e.	0.08945 M

 

 

ANS:  C

 

 

48. If 0.1800 g of impure soda ash (Na₂CO₃) is titrated with 15.66 mL of 0.1082 M HCl, what is the percent purity of the soda ash?

Na₂CO₃(aq) + 2 HCl(aq) ® 2 NaCl(aq) + H₂O() + CO₂(g)

a.	17.96%
b.	49.89%
c.	50.11%
d.	94.13%
e.	99.77%

 

 

ANS:  B

 

49. Transmittance, T, is defined as the intensity of light transmitted through a sample divided by the intensity of light incident on the sample. The absorbance, A, is defined as

a.	A = –log T
b.	A = log (–T)
c.	A = 10T
d.	A = 10–T
e.	A = 10–1/T

 

 

ANS:  A

 

50. Which of the following statements is/are CORRECT?

	1.	Absorbance is directly proportional to the intensity of the incident light.
	2.	Absorbance is inversely proportional to the analyte concentration.
	3.	Absorbance is directly proportional to the path length of the light.

 

a.	1 only
b.	2 only
c.	3 only
d.	2 and 3
e.	1,2, and 3

 

 

ANS:  C

 

SHORT ANSWER

 

51. The numbers preceding the formulas in chemical equations are referred to as the ________ coefficients.

 

ANS:

stoichiometric

 

 

52. The percent yield of a chemical reaction is calculated by dividing the actual yield by the ________ yield and multiplying by 100%.

 

ANS:

theoretical

 

 

53. The pH of purified water (or of a neutral solution) is _____.

 

ANS:

7.00

 

 

54. The following equation: A = e ´  ´ C (where  is path length and C is concentration) is known as the _____-Lambert law.

 

ANS:

Beer

 

 

55. PCl₃ can be produced from the reaction of P₄ with Cl₂.

P₄(s) + 6 Cl₂(g) ® 4 PCl₃(g)

If 1.00 g P₄ reacts with 1.00 g Cl₂, which reactant is the limiting reactant? What mass of product may be produced?

 

ANS:

Chlorine is the limiting reactant and 1.29 g PCl₃ may be produced.

 

 

56. The reaction of 5.07 g N₂ with 0.722 g H₂ produces 1.27 g NH₃. The percent yield of this reaction is ________.

 

ANS:

31.2%

 

 

57. In combustion analysis, the gases produced by the combustion of a hydrocarbon are passed through a tube containing finely divided NaOH supported on asbestos. The purpose of the NaOH is to absorb ________ produced by the combustion reaction.

 

ANS:

CO₂ or carbon dioxide