Problem Bank R51 Problem Bank Appendix D Chapter 2 Are intensive or extensive properties most 1. helpful in identif ying a substance? Explain your choice. Classif y the following mixtures as homo- 2. geneous or heterogeneous. a toaster a. a calculator b. the air on a clear day c. a copper coin d. Identif y the following as a mixture or a sub - 3. stance. tomato juice a. a rusty, iron fence post b. a drop of mercury c. a milkshake d. Classif y the following as a physical change or a 4. chemical change. salad dressing separates into layers after a. standing spilled acid burns a hole in cotton jeans b. alcohol freezes c. ice sublimes d. Classif y the following properties of an alumi - 5. num bar as either physical or chemical. burns in pure oxygen a. melts at 660°C b. bends easily c. is nonmagnetic d. Chapter 3 How many significant figures are in each 6. measurement? 786.32 mg 786 32 a. e. 0.0500 s 00500 0.0004 s b. f. 66.066 mg 5.060 kg c. g. 4000 m 7006.0 g d. h. 40.0 10 3 m measurements in Problem 6 Write each of the m 7. n. in scientific notation ass of three gold bars that What is the total ma 8. 45 mg, and 697.4 mg? weigh 5543 mg, 23.4 igh temperature on the e normal daily hi 9. planet Zork is C. Express this temperature 85°C in kelvins. contributes to global Methane, a gas that 10. sity of 0.714 g/L. What is warming, has a den of 25.0 L of methane? the mass, in grams, is 9.394 g/cm e density of zinc i 11. 3 at 20°C. ( in cubic centimeters ) of a What is the volume l that has a mass of 15.6 g? sphere of zinc metal in kilograms of 964 mL of Calculate the mass i 12. y. e density of mercury is the element mercury 13.6 g/mL. conversions: Make the following 13. 55 mg to grams a. 5.76 dL to liters b. meters 0.96 m to microm c. s 5.26 ns to seconds d. ms 87 kg to milligram e. timoles 846 mmol to cent f. eters 3.4 nm to picome g. 6.66 h. 10 3 megagrams kg to m 2.34 i. 10 5 o microliters mL to unit of blood to the Red When you donate a 14. bout 0.55 L of blood. How Cross, you “give” ab eters (cm many cubic centime 3 ) of blood is this? daily amount (RDA) of e recommended d 15. vitamin B 6 ts is 0.2 cg. How many for adult min B micrograms of vitam 6 should be consumed each day? aundice (characterized by A person develops ja 16. n) when the concentration yellowing of the skin of bilirubin in his or her blood is 18 mg biliru of bilirubin in hisor - bin per liter of blood. Assuming a total blood volume of 5.2 L, what is the number of grams of bilirubin in the person’s blood? Problem Bank R51 PROBLEM BANK Appendix D Problem Bank Answers Chapter 2 1. Intensive properties: because they depend on the composition of the sample, not the amount of matter in the sample. 2. a. heterogeneous b. heterogeneous c. homogeneous d. homogeneous 3. a. mixture b. mixture c. substance d. mixture 4. a. physical change b. chemical change c. physical change d. physical change 5. a. chemical b. physical c. physical d. physical Chapter 3 6. a. 5 b. 1 c. 4 d. 5 e. 3 f. 5 g. 1 h. 3 7. a. 7.8632 × 10 2 b. 4 × 10 −4 c. 5.060 × 10 0 d. 7.0060 × 10 3 e. 5.00 × 10 −2 f. 6.6066 × 10 1 g. 4 × 10 3 h. 4.00 × 10 4 8. 6264 mg 9. 188 K 10. 17.9 g 11. 1.66 cm 3 12. 13.1 kg 13. a. 5.5 × 10 −2 g b. 5.76 × 10 −1 L c. 9.6 × 10 5 μm d. 5.26 × 10 −9 s e. 8.7 × 10 7 mg f. 8.46 × 10 1 cmol g. 3.4 × 10 3 pm h. 6.66 Mg i. 2.34 × 10 −2 μL 14. 5.5 × 10 2 cm 3 15. 2 × 10 3 μg 16. 9.4 × 10 −2 g
Transcript
Problem Bank R51
Problem BankAppendix D Chapter 2
Are intensive or extensive properties most1.helpful in identifying a substance? Explain your choice.
Classify the following mixtures as homo-2.geneous or heterogeneous.
a toastera.a calculatorb.the air on a clear dayc.a copper coind.
Identify the following as a mixture or a sub-3.stance.
tomato juicea.a rusty, iron fence postb.a drop of mercuryc.a milkshaked.
Classify the following as a physical change or a 4.chemical change.
salad dressing separates into layers aftera.standingspilled acid burns a hole in cotton jeansb.alcohol freezesc.ice sublimesd.
Classify the following properties of an alumi-5.num bar as either physical or chemical.
burns in pure oxygena.melts at 660°Cb.bends easilyc.is nonmagneticd.
Chapter 3
How many significant figures are in each 6.measurement?
786.32 mg786 32a. e. 0.0500 s0 05000.0004 sb. f. 66.066 mg5.060 kgc. g. 4000 m7006.0 gd. h. 40.0 103 m
measurements in Problem 6 Write each of the m7.n.in scientific notation
ass of three gold bars that What is the total ma8.45 mg, and 697.4 mg?weigh 5543 mg, 23.4
igh temperature on theThe normal daily hi9.planet Zork is C. Express this temperature 85°Cin kelvins.
contributes to globalMethane, a gas that 10.sity of 0.714 g/L. What iswarming, has a denof 25.0 L of methane?the mass, in grams,
is 9.394 g/cmThe density of zinc i11. 3 at 20°C.(in cubic centimeters) of a What is the volume
l that has a mass of 15.6 g?sphere of zinc metal
in kilograms of 964 mL of Calculate the mass i12.y. The density of mercury is the element mercury
13.6 g/mL.
conversions:Make the following 13.55 mg to gramsa.5.76 dL to litersb.
meters0.96 m to micromc.s5.26 ns to secondsd.ms87 kg to milligrame.timoles846 mmol to centf.eters3.4 nm to picomeg.
6.66 h. 103 megagramskg to m2.34 i. 10 5 o microliters mL to
unit of blood to the Red When you donate a 14.bout 0.55 L of blood. How Cross, you “give” abeters (cmmany cubic centime 3) of blood is this?
daily amount (RDA) of The recommended d15.vitamin B6 ts is 0.2 cg. How many for adult
min Bmicrograms of vitam 6 should be consumed each day?
aundice (characterized by A person develops ja16.n) when the concentration yellowing of the skin
of bilirubin in his or her blood is 18 mg biliruof bilirubin in his or -bin per liter of blood. Assuming a total bloodvolume of 5.2 L, what is the number of gramsof bilirubin in the person’s blood?
Problem Bank R51
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Appendix D Problem Bank
Answers
Chapter 2 1. Intensive properties: because they depend on
the composition of the sample, not the amount of matter in the sample.
2. a. heterogeneous b. heterogeneousc. homogeneous d. homogeneous
3. a. mixture b. mixturec. substance d. mixture
4. a. physical change b. chemical changec. physical change d. physical change
5. a. chemical b. physicalc. physical d. physical
Chapter 3
6. a. 5 b. 1 c. 4 d. 5 e. 3 f. 5 g. 1 h. 3
7. a. 7.8632 × 102 b. 4 × 10−4
c. 5.060 × 100 d. 7.0060 × 103
e. 5.00 × 10−2 f. 6.6066 × 101
g. 4 × 103 h. 4.00 × 104
8. 6264 mg
9. 188 K
10. 17.9 g
11. 1.66 cm3
12. 13.1 kg
13. a. 5.5 × 10−2 g b. 5.76 × 10−1 L c. 9.6 × 105 μm d. 5.26 × 10−9 s e. 8.7 × 107 mg f. 8.46 × 101 cmol g. 3.4 × 103 pm h. 6.66 Mg i. 2.34 × 10−2 μL
14. 5.5 × 102 cm3
15. 2 × 103 μg
16. 9.4 × 10−2 g
R52 Appendix D
Mites are small eight-legged “bugs” in the17.same family as spiders. A particularly small mite has a mass of 0.0043 dg. What is the mass of this mite expressed in micrograms?
In the United States, a typical can of soda 18.holds 355 mL. How many 2.00-L bottles could be filled from a 24-can case of soda?
You are going to carry out a chemical reaction19.in which you need 16 g of oxygen for every 7.0 g of nitrogen that will be used. If you have0.554 kg of oxygen, how many milligrams of nitrogen do you need?
If your heart beats at an average rate of 20.72 times per minute, how many times will your heart beat each year?
Four empty beakers weigh a total of 1.84 kg.21.Each beaker when full holds 0.75 kg of water.How much do two full beakers of water weigh?
How many days would it take you to count a22.million pennies if you could count one penny each second? Express the answer to 3 signifi-cant figures.
A soap bubble film is 8.0 23. 102 nm thick.Express this thickness in the following units:
centimetersa. c. decimetersmicrometersb. d. millimeters
The pitcher’s mound on a regulation baseball24.field is 60 feet 6 inches from home plate. How many seconds does it take a 96 mph fastball toreach home plate? (5280 ft 1 mile)
Gemstones such as diamonds are measured 25.in carats, where 1 carat 2.00 dg. How many kilograms of diamonds were produced if 12.5 million carats of diamonds were minedin a recent year?
How many meters does a car moving at 26.95 km/hour travel in 1.0 second?
A milliliter of water is equal to 20 drops of 27.water. If water is dripping from a faucet at therate of 7 drops per minute, how many dayswill it take to completely fill a 2.00-L sodabottle?
A prescription for a certain drug calls for a28.dose of 0.200 mg/kg of body weight, four timesa day. The drug is packaged in capsules of 5 mg. How many capsules per dose should begiven to a patient who weighs 75 kg?
A certain low-tar cigarette contains 11.0 mg of 29.tar per cigarette.
If all the tar gets into the lungs, how many a.packs of cigarettes (20 cigarettes per pack)would have to be smoked to produce 0.500 lbof tar? (454 g 1 lb)If a person smoked two packs per day, how b.many years would it take to accumulate0.500 lb of tar?
A chemist needs 25.0 mL of a liquid compound.30.What mass of the compound is necessary if a.the density is 0.718 g/cm3?If the compound costs $1.75/gram, what is b.the cost of this amount of the compound?
What volume of sodium has the same mass31.as 22.0 cm3 of silicon? The density of sodium is 0.97 g/cm3; the density of silicon is 2.33 g/cm3.
What is the mass, in kilograms, of a block of 32.platinum that measures 23.0 cm by 78.4 cm by 122 cm? The density of platinum is 22.5 g/cm3.
Sulfuric acid sold for laboratory use consists33.of 96.7% sulfuric acid, H2SO4, by mass. The density of the solution is 1.845 g/cm3. Computethe number of kilograms of H2SO4 in a 2.20-Lbottle of laboratory sulfuric acid.
How many kilograms of dry air are in a room 34.that measures 15.0 ft by 18.0 ft by 8.00 ft? Usean average density of air of 1.168 g/L. There are 30.48 cm in one foot.
Calculate the number of cubic centimeters in 35.each of the following:
1 ma. 3 c. 5 nm3
1 dmb. 3 d. 2 10 3 km3
Chapter 4
In which of these atom(s) is the number of pro-36.tons equal to the number of neutrons?
germanium-72a. c. silicon-28calcium-40b. d. hydrogen-1
Give the total number of subatomic particles37.(protons, electrons, and neutrons) in eachatom.
vanadium-51a. c. tin-120aluminum-27b. d. hafnium-178
R52 Appendix D
APPEN
DIX
D17. 4.3 × 102 μg
18. 4.26 bottles
19. 2.4 × 105 mg
20. 3.8 × 107 beats/year
21. 2.42 kg
22. 11.6 days
23. a. 8.0 × 10–5 cm b. 8.0 × 10–1 μmc. 8.0 × 10–6 dm d. 8.0 × 10–4 mm
24. 0.43 s
25. 2.50 × 103 kg
26. 26 m
27. 4 days
28. 3 capsules/dose
29. a. 1.03 × 103 packs b. 1.41 years
30. a. 18.0 g b. $31.50
31. 52.8 cm3 sodium
32. 4.95 × 103 kg
33. 3.93 kg
34. 71.5 kg of air
35. a. 1 × 106 cm3 b. 1 × 103 cm3
c. 5 × 10–21 cm3 d. 2 × 1012 cm3
Chapter 436. a. not equal b. equal
c. equal d. not equal
37. a. 23 protons, 23, electrons, 28 neutrons
b. 13 protons, 13 electrons, 14 neutrons
c. 50 protons, 50 electrons, 70 neutrons
d. 72 protons, 72 electrons, 106 neutrons
Problem Bank R53
Identify the element name and mass number of 38.an atom with the given composition.
Use the mass and percent abundance of the 39.four isotopes of strontium to calculate theatomic mass of strontium.
Isotope Mass (amu)
Abundance (%)
Strontium-84 83.193 0.560
Strontium-86 85.909 9.86
Strontium-87 86.908 7.00
Strontium-88 87.906 82.58
An atom of carbon and an atom of element 40.Z together weigh 6 amu less than double theweight of an atom of oxygen. If an atom of oxygen weighs 16 amu and an atom of carbon weighs 12 amu, what does an atom of element Z weigh?
Chapter 5
What is the maximum number of electrons in 41.each of the following?
the fourth energy levela.the 5b. p5 energy sublevela single 4c. f4 orbitalfthe first three energy levelsd.
Write the electron configuration of each atom.42.nickela.sulfurb.arsenicc.rubidiumd.
Identify the symbols of the elements with the 43.following electron configurations:
1a. s22s22p2 6 3s23p3 63d104s1
1b. s22s22p2 63s23p3 5
1c. s22s22p2 63s23p3 63d104s24p4 64d25s2
1d. s22s22p2 63s23p3 63d104s24p4 6
How many electrons are in the44.third energy level of an indium atom?a.second energy level of an oxygen atom?b.third energy level of a vanadium atom?c.first energy level of a barium atom?d.
Calculate the wavelength (in meters) of each of 45.these frequencies of electromagnetic radiation.
9.82 a. 1019/s2.24b. 1014/s5.31c. 107/s7.78 d. 1010/s
Order the wavelengths in Problem 45 from46.highest to lowest energy.
Chapter 6
Based on their relative positions on the 47.periodic table, which atom in each pair hasthe smaller atomic radius?
Na, Ka.Cl, Brb.K, Brc.Ne, Nad.
Based on their relative positions on the 48.periodic table, which atom in each pair hasthe greater electronegativity?
B, Ca.Na, Alb.Li, Csc.As, Fd.
Based on their relative positions on the 49.periodic table, which atom in each pair has thehighest first ionization energy?
F, Bra.Li, Fb.Ca, Bec.K, Ard.
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Problem Bank R53
38. a. molybdenum-98 b. helium-3c. osmium-189 d. gallium-71
39. 87.62 amu
40. 14 amu
Chapter 541. a. 32 electrons b. 6 electrons
c. 2 electrons d. 28 electrons
42 a. 1s22s22p63s23p63d84s2
b. 1s22s22p63s23p4
c. 1s22s22p63s23p63d104s24p3
d. 1s22s22p63s23p63d104s24p65s1
43. a. Cu b. Clc. Zr d. Kr
44. a. 18 electrons b. 6 electronsc. 11 electrons d. 2 electrons
45. a. 3.05 × 10–12 m b. 1.34 × 10–6 mc. 5.65 m d. 3.85 × 10–3 m
46. highest to lowest: a, b, d, c
Chapter 647. a. Na b. Cl
c. Br d. Ne
48. a. C b. Alc. Li d. F
49. a. F b. Fc. Be d. Ar
R54 Appendix D
Here are the first, second, and third ionization50.energies (kJ/mol) respectively for the represen-tative elements “X” and “Y.”
Element
Firstionizationenergy (kJ/mol)
Secondionizationenergy (kJ/mol)
Thirdionizationenergy (kJ/mol)
X 738 1450 7732
Y 496 4565 6912
In what group on the periodic table would these elements most likely be found?
Would the ion formed from each element be 51.larger or smaller than the atom from which itwas formed?
calciuma.aluminumb.brominec.nitrogend.
Chapter 7
In any group of representative elements on the 52.periodic table, how does the number of valence electrons vary as the elements within the groupincrease in mass?
How many valence electrons are lost by the 53.metallic element when forming each of theseionic compounds?
BaSa.Inb. 2Se3
GaPc.SrId. 2
Write the formulas for two cations of represen-54.tative elements that have the electron configu-ration 1s22s22p2 63s23p3 6.
If “X” is the formula for any halogen and “M”55.is the formula for any metal, which of these is a valid formula of an ionic compound formedbetween “M” and “X”? What is the electron dotstructure for “M” in each of the compoundsthat can be formed?
MXa. 2
Mb. 2X2
MXc. 3
Md. 2X3
How many electrons are in each ion?56.Pba. 4 c. Te2
Crb. 3 d. C4
Chapter 8
Draw an electron dot structure for each sub-57.stance.
Ha. 2TeAsHb. 3
SiBrc. 4rId. 2
How many electrons are in the electron dot 58.structure for each of these polyatomic ions?
cyanide, CNa.bromate ion, BrOb. 3
phosphite ion, POc. 33
nitrite, NOd. 2
Use VSEPR theory to predict the shape of each 59.molecule in Problem 57.
Classify each of the molecules in Problem 57 as60.polar or nonpolar.
Chapter 9
Classify each of these compounds as molecular 61.or ionic.
CFa. 4
PtOb. 2
SrIc. 2
NHd. 4BrKe. 2CO3
NIf. 3
Cg. 5H10O5
Ba(OH)h. 2
Name or write the formulas for these molecu-62.lar compounds.
SiCla. 4
phosphorus triiodideb.Brc. 2O7
iodine monofluorided.BrFe. 5
diarsenic trioxidef.NClg. 3
diphosphorus pentoxideh.
R54 Appendix D
APPEN
DIX
D50. Element X, group 2A; element Y, group 1A
51. a. smaller b. smallerc. larger d. larger
Chapter 752. The number of valence electrons remains
the same.
53. a. 2 b. 3c. 3 d. 2
54. K+ and Ca2+
55. MX2 (M with 2 dots) and MX3 (M with 3 dots) are valid formulas
56. a. 78 b. 21c. 54 d. 10
Chapter 8
57. a. TeH H
b. AsH
H H
c.
SiBr
BrBr Br
d. II
58. a. 10 b. 26c. 26 d. 18
59. a. bent b. pyramidalc. tetrahedral d. linear
60. a. polar b. polarc. nonpolar d. nonpolar
Chapter 961. a. molecular b. ionic
c. ionic d. ionice. ionic f. molecularg. molecular h. ionic
62. a. silicon tetrachloride b. PI3c. dibromine heptoxide d. IFe. bromine pentafluoride f. As2O3
g. nitrogen trichloride h. P2O5
Problem Bank R55
Write the formulas for these ionic compounds.63.barium iodidea.iron(III) acetateb.potassium dichromatec.ammonium bromided.cesium nitridee.cobalt(III) nitratef.aluminum oxalateg.mercurous chlorideh.
Name these ionic compounds.64.Rba. 2S e. HgCl2
LiIb. f. CuClO3
Pb(Cc. 2H3O2)2 g. NaCNMgd. 3N2 h. Cr(ClO4)3
Name these compounds.65.Csa. 2O e. H2CrO4
SnSb. 2 f. CaC2O4
Nc. 4S4 g. (NH4)3PO4
Bd. 2O3 h. As4O10
Write the formulas for these compounds.66.calcium oxidea.sulfurous acidb.diboron tetrachloridec.calcium hydrogen phosphated.tin(II) chromatee.ferric hydroxidef.manganese(II) chloriteg.iodine monochlorideh.
Explain why it is not fair to be asked to write a 67.formula for each named “compound.”
iron bromidea.sulfur oxideb.lead hypochloritec.phosphorus chlorided.
Iron forms two compounds with oxygen. One 68.compound consists of 1.396 g of iron and0.400 grams of oxygen. The other has 0.582 giron and 0.250 g oxygen. Show by calculationwhether this pair of compounds obeys the law of multiple proportions.
Chapter 10
How many of each kind of atom are in a69.formula unit of each compound?
(NHa. 4)2SO3
AlPOb. 4
Ca(Cc. 2H3O2)2
Fed. 2(SO4)3
How many of each kind of atom are in a70.molecule of each compound?
Ca. 3H7O2
Cb. 3H5(OH)3
Cc. 2H4(COOH)2
Cd. 7H5(NO3)3
Calculate the molar mass of each of these bi-71.nary ionic compounds.
MgOa. c. Hg2I2
AlClb. 3 d. Sr3N2
Calculate the molar mass of each of these ionic 72.compounds.
(NHa. 4)2C2O4
Ca(OH)b. 2
Nac. 2HPO4
Mg(HSOd. 4)2
Calculate the molar mass of each of these 73.molecular compounds.
Na. 2O5
Cb. 3H7OHSOc. 3
XeFd. 6
Calculate the molar mass of each of these 74.compounds.
DEET, Ca. 12H17ON, an insect repellentaspartame, Cb. 14H18N2O5, a sugar substitutecodeine, Cc. 18H21NO3, an analgesic (painkiller)sodium benzoate, NaCd. 7H5O2, a food preservative
What is the mass, in grams, of each of the 75.following?
5.000 mol Ara.1.64 mol NaNOb. 2
0.886 mol (NHc. 4)2SO4
18.3 mol SiFd. 4
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Problem Bank R55
63. a. BaI2 b. Fe(C 2 H 3 O 2 )3
c. K2Cr2O7 d. NH4Bre. Cs3N f. Co(NO3)3
g. Al2(C2O4)3 h. Hg2Cl2
64. a. rubidium sulfide b. lithium iodidec. lead(II) acetate d. magnesium nitridee. mercury(II) chloride f. copper(I) chlorateg. sodium cyanide h. chromium(III)
perchlorate
65. a. cesium oxide b. tin(II) sulfidec. tetranitrogen tetrasulfide d. diboron trioxidee. chromic acid f. calcium oxalateg. ammonium phosphate h. tetraarsenic
decoxide
66. a. CaO b. H2SO3
c. B2Cl4 d. CaHPO4
e. SnCrO4 f. Fe(OH)3
g. Mn(ClO2)2 h. ICl
67. a. The ionic charge of iron must be given by a Roman numeral.
b. Prefixes must be used in the name of a molecular compound.
c. The ionic charge of lead must be given by a Roman numeral.
d. Prefixes must be used in the name of a molecular compound.
68. The ratio of masses of iron per gram of oxygen is 3:2, so these compounds obey the law of multiple proportions.
Chapter 10
69. a. N, 2; H, 8; S, 1; O, 3 b. Al, 1; P, 1; O, 4c. Ca, 1; C, 4; H, 6; O, 4 d. Fe, 2; S, 3; O, 12
70. a. C, 3; H, 7; O, 2 b. C, 3; H, 8; O, 3c. C, 4; H, 6; O, 4 d. C, 7; H, 5; N, 3; O, 9
71. a. 40.3 g b. 133.5 gc. 655.0 g d. 217.2 g
72. a. 124.0 g b. 74.1 gc. 142.0 g d. 218.5
73. a. 108.0 g b. 60.0 gc. 80.1 g d. 245.3 g
74. a. 191.0 g b. 294.0 gc. 299.0 g d. 144.0 g
75. a. 199.5 g b. 113 gc. 117 g d. 1.91 × 103 g
R56 Appendix D
How many moles is each of the following?76. 579 g Pta. 0.0426 g NOb. 2
56.8 g Hc. 2SO3
6.78 d. 103 g CsH2PO4
Find the number of representative particles in 77. each of the following:
4.40 mol Pda. 0.284 mol NaIb. 1.62 mol NHc. 3
12.8 mol Fe(Cd. 2H3O2)2
How many moles is each of the following?78. 7.26 a. 1022 atoms Zr1.48 b. 1024 molecules C2H6O4.00 c. 1023 formula units KClO3
9.02 d. 1024 molecules OF2
Calculate the volume, in liters, of each of these 79. gases at STP.
3.64 mol Ha. 2
0.0648 mol Cb. 2H6
8.44 mol SOc. 3
1.26 mol Xed.
How many moles is each of the following at 80. STP?
56.4 L Hea. 7.64 L Nb. 2
0.888 L COc. 126 L SOd. 2
Calculate the number of representative par-81. ticles in each mass.
14.6 g COa. 2
68.3 g Osb. 0.847 g KClc. 174 g Aud. 2O3
Calculate the mass of each of the following 82. samples.
7.00 a. 109 molecules Br2
9.22 b. 1022 formula units NaF4.8 c. 1024 atoms Li2.66 d. 1020 molecules H2CO
Find the mass of each of the gases at STP.83. 2.44 L Oa. 2 c. 78.0 L SO3
777 L CHb. 4 d. 0.0642 L H2
Calculate the volume of each of these gases at 84. STP.
0.469 g Cla. 2
44.8 g NOb. 2.76 g Nc. 2O3
93.2 g Fd. 2
Calculate the number of representative par-85. ticles in each volume.
64.0 L Ha. 2S3.36 L Cb. 3H8
4.78 c. 104 L HF6.88 d. 10 2 L Kr
Find the volume at STP of the following:86. 3.66 a. 1021 molecules F2
6.11 b. 1022 molecules PH3
1.16 c. 1025 atoms Ne4.48 d. 1024 molecules C2H2
Calculate the number of oxygen atoms in each 87. of the following:
7 molecules of the explosive nitroglycerine, a. C3H5(NO3)3
3.00 mol of the antiseptic hydrogen peroxide, b. H2O2
a balloon filled with 2.00 L Oc. 2
8.04 g of the fertilizer, NHd. 4NO3
Calculate the number of grams of hydrogen in 88. each of the following.
a balloon filled with 7.06 a. 1024 hydrogen moleculesa balloon filled with 14.0 L of methane, CHb. 4, at STPa 2.00-L bottle of water (density of Hc. 2O 1.00 g/mL)a 69.5-g ice cube (density of ice d. 0.917 g/cm3)
Calculate the percent composition of each 89. compound.
PbOa. 2
(CHb. 3)2COKIOc. 3
Nad. 2S2O3
IFe. 5
HBrOf. 4
Pg. 4O6
Ch. 3H7COOH
R56 Appendix D
APPEN
DIX
D76. a. 2.97 mol b. 9.26 × 10–4 mol
c. 0.692 mol d. 29.5 mol
77. a. 2.65 × 1024 molecules b. 1.71 × 1023 formula units c. 9.75 × 1023 molecules d. 7.71 × 1024 formula units
78. a. 0.121 mol b. 2.46 mol c. 0.664 mol d. 15.0 mol
79. a. 81.5 L b. 1.45 Lc. 189 L d. 28.2 L
80. a. 2.52 mol b. 0.341 molc. 3.96 × 10–2
mol d. 5.63 mol
81. a. 2.00 × 1023 molecules b. 2.16 × 1023 atoms c. 6.84 × 1021 formula units d. 2.37 × 1023 formula units
82. a. 1.86 × 10–12 g b. 6.43 gc. 55 g d. 1.33 × 10–2 g
83. a. 3.49 g b. 555 gc. 279 g d. 5.7 × 10–3 g
84. a. 0.148 L b. 33.5 Lc. 0.813 L d. 54.9 L
85. a. 1.72 × 1024 molecules b. 9.03 × 1022 molecules
c. 1.28 × 1027 molecules d. 1.85 × 1021 atoms
86. a. 0.136 L b. 2.27 Lc. 432 L d. 167 L
87. a. 63 oxygen atoms b. 3.61 × 1024 oxygen atoms c. 1.08 × 1023 oxygen atoms d. 1.82 × 1023 oxygen atoms
88. a. 23 g b. 2.50 gc. 222 g d. 7.72 g
89. a. 86.6% Pb, 13.4% O b. 62.1% C, 10.3% H, 27.6% O c. 18.3% K, 59.3% I, 22.4% O d. 29.1% Na, 40.6% S, 30.3% O e. 57.2% I, 42.8% F f. 0.69% H, 55.1% Br, 44.2% O g. 56.4% P, 43.6% O h. 54.5%C, 9.1% H, 36.4 % C
Problem Bank R57
Use the answers from Problem 89 to calculate90.the number of grams of the indicated elementin the compound.
lead in 63.8 g PbOa. 2
carbon in 1.664 g (CHb. 3)2COoxygen in 36.8 g KIOc. 3
sulfur in 6.26 g Nad. 2S2O3
fluorine in 594 g IFe. 5
bromine in 82.7 g HBrOf. 4
phosphorus in 2.66 g Pg. 4O6
carbon in 55.0 g Ch. 3H7COOH
Which of these are empirical formulas?91.Ala. 2(SO4)3
Cb. 6H4Cl2
Cc. 2H4(OH)2
Kd. 2Cr2O7
What is the empirical formula of92.Ca. 6H16N2, a compound used to make nylon?Cb. 6H8N2, a component of chocolate?Cc. 8H8, used to make polystyrene foam plastics?Cd. 3H7OH, rubbing alcohol?
Determine the empirical formula for each 93.compound from the percent composition data.
Find the molecular formula from the given 94.empirical formula and molar mass.
A compound with a molar mass of 95.312.2 g/mol contains 69.23% C, 3.85% H, and26.92% N. What is the molecular formula of this compound?
The molar mass of caffeine, the stimulant96.found in coffee, is 194.0 g/mol. The percentcomposition of caffeine is 49.48% C, 5.19% H, 28.85% N, and 16.48% O. What is the molecu-lar formula of caffeine?
Linoleic acid, which has a molar mass of 97.280.0 g/mol, is found in many vegetable oils.The percent composition of this compound is77.1% carbon, 11.4% hydrogen, and 11.4% oxy-gen. Find the empirical formula and molecular formula of this compound.
A 2.716-g sample of a compound of C, H, N, 98.and O was found to contain 0.7580 g C, 0.0633 g H, and 0.8843 g N. The molar massof the compound is 129 g/mol. Calculate thecompound’s empirical and molecular formula.
Chapter 11
What is the function of the element platinum99.in this reaction?
2H2 O2 2H2O
Balance the following equations:100.Hg(NOa. 3)2 NH4SCN
Classify each of the equations in Problem 100101.by type.
Write balanced equations for each of these102.reactions. Indicate states of matter in yourequations.
Potassium metal reacts with water to form a.hydrogen gas and aqueous potassiumhydroxide.Nitrogen monoxide gas reacts with gaseous b.carbon monoxide to form carbon dioxide gasand nitrogen gas.
Empirical formula
Molar mass (g/mol)
Molecular formula
C2H3 54.0 a.
C2H2Cl 123.0 b.
C3H4O3 176.0 c.
C5H7N 162.0 d.
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Problem Bank R57
90. a. 55.3 g Pb b. 1.03 g Cc. 8.24 g O d. 2.54 g Se. 254 g F f. 45.6 g Brg. 1.50 g P h. 30.0 g C
c. Ca + Cl2 → CaCl2d. 2Na3PO4 + 3CoCl2 → Co3(PO4)2 + 6NaCl
e. Fe + 2AgNO3 → Fe(NO3)2 + 2Ag
f. 3N2H4 → 4NH3 + N2
g. 2C12H26 + 37O2 → 24CO2 + 26H2O
h. 2CuCl + Mg → 2Cu + MgCl2
101. a. double-replacement b. combustionc. combination d. double-replacemente. single-replacement f. decompositiong. combustion h. single replacement
102. a. 2K(s) + 2H2O(l) → H2(g) + 2KOH(aq)
b. 2NO(g) + 2CO(g) → 2CO2(g) + N2(g)
R58 Appendix D
Hydrochloric acid reacts with oxygen gas to c.form liquid water and chlorine gas.Aqueous calcium hydroxide reacts with ace-d.tic acid to form water and aqueous calciumacetate.Oxygen gas reacts with solid lead(II) sulfidee.to form sulfur dioxide gas and lead(II) oxide.Solid lithium oxide reacts with water to formf.aqueous lithium hydroxide.Solid manganese dioxide reacts with oxalic g.acid to form solid manganese(II) oxide, water, and gaseous carbon dioxide.Gaseous diboron hexahydride reacts withh.oxygen gas to form liquid water and solid diboron trioxide.
Complete and then balance each of these103.equations.
Use Table 11.3 to predict whether a precipitate 105.will form when aqueous solutions of these pairs of salts are mixed. If a precipitate forms,write its formula.
ammonium sulfate and barium bromidea.chromium(II) chloride and lithium carbon-b.atepotassium nitrate and sodium chloridec.sodium sulfide and mercury(II) nitrated.
Write a balanced complete ionic equation for106.each of these double-replacement reactions. Allthe reactants are in aqueous solution.
nickel(II) chloride a. potassium phosphateacetic acid b. calcium hydroxidecalcium iodide c. sodium sulfatesodium hydroxided. lead(II) nitrate
Identify the spectator ions in each of the reac-107.tions in Problem 106.
Write net ionic equations for each of the reac-108.tions in Problem 106.
Chapter 12
Interpret each equation in terms of interacting 109.particles.
Ha. 2 F2 2HF2Kb. 3PO4 3CoCl2 Co3(PO4)2 6KCl2PbS c. 3O2 2PbO 2SO2
Fed. S FeS
Write all possible mole ratios for these equa-110.tions.
2NOa. Cl2 2NOCl2KClOb. 3 2KCl 3O2
3Nc. 2H4 4NH3 N2
2Na d. O2 Na2O2
Show by calculation that the following equa-111.tions obey the law of conservation of mass:
3NOa. 2 H2O 2HNO3 NO4HClb. O2 2H2O 2Cl2
2Li c. S Li2S2CHd. 4O 3O2 2CO2 4H2O
Nitric acid, HNO112. 3, is produced by a process that allows nitrogen dioxide to react with water.3NO2(g) gg H2O(l) 2HNO3(aq) NO(g)gg
How many moles of nitrogen dioxide, NOa. 2, are required to produce 3.56 mol of nitricacid?How many moles of water react with 0.946 b.mol of nitrogen dioxide?
electricity
R58 Appendix D
APPEN
DIX
D c. 4HCl(aq) + O2(g) → 2H2O(l) + 2Cl2(g)
d. Ca(OH)2(aq) + 2HC2H3O2(aq) → 2H2O(l) + Ca(C2H3O2)2(aq)
e. 3O2(g) + 2PbS(s) → 2SO2(g) + 2PbO(s)
f. Li2O(s) + H2O(l) → 2LiOH(aq)
g. MnO2(s) + H2C2O4(aq) → MnO(s) + H2O(l) + 2CO2(g)
h. B2H6(g) + 3O2(g) → 3H2O(l) + B2O3(s)
103. a. 2HCl(ag) H2(g) + Cl2(g)
b. 3Br2(l) + 2AlI3(aq) → 2AlBr3(aq) + 3I2(aq)
c. 2Na(s) + S(s) → Na2S(s)
d. Ba(OH)2(aq) + 2HNO3(aq) → 2H2O(l) + Ba(NO3)2(aq)
e. 2C7H14O2(l) + 19O2(g) → 14H2O(l) + 14CO2(g)
f. Ni(NO3)2(aq) + Na2CO3(aq) → NiCO3(s) + 2NaNO3(aq)
104. a. MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O
b. PCl5 + 4H2O → H3PO4 + 5HCl
c. Ca3P2 + 6H2O → 2PH3 + 3Ca(OH)2
d. Li3N + 3H2O → 3LiOH + NH3
e. 2H2O2 + N2H4 → N2 + 4H2O
f. SiCl4 + 2Mg → 2MgCl2 + Si
g. V2O5 + 2H2 → V2O3 + 2H2O
h. HBr + KHSO3 → KBr + H2O + SO2
105. a. BaSO4 b. CrCO3
c. no precipitate formed d. HgS
106. a. 3Ni2+(aq) + 6Cl–(aq)+ 6K+(aq) + 2PO43–(aq) →
Ni3(PO4)2(s) + 6Cl–(aq)+ 6K+(aq)
b. 2H+(aq) + 2C2H3O2–(aq) + Ca2+(aq) + 2OH–(aq)
→ 2H2O(l) + Ca2+(aq) + 2C2H3O2–(aq)
c. Ca2+(aq) + 2I–(aq) + 2Na+(aq) + SO42–(aq) →
CaSO4(s) + 2I–(aq) + 2Na+(aq)
d. 2Na+(aq) + 2OH–(aq) + Pb2+(aq) + 2NO3–(aq)
→ Pb(OH)2(s) + 2Na+(aq) + 2NO3–(aq)
107. a. Cl–(aq) + K+(aq) b. Ca2+(aq) + C2H3O2–(aq)
c. I–(aq) + Na+(aq) d. Na+(aq) + NO3–(aq)
108. a. 3Ni2+(aq) + 2PO43–(aq)→ Ni3(PO4)2(s)
b. 2H+(aq) + 2OH–(aq) → 2H2O(l)
c. Ca2+(aq) + SO42–(aq) → CaSO4(s)
d. Pb2+(aq) + 2OH–(aq) → Pb(OH)2(s)
electricity
Problem Bank R59
Calcium hydroxide reacts with nitric acid113.to produce an aqueous solution of calcium nitrate.Ca(OH)2(aq) 2HNO3(aq)
2H2O(l) Ca(NO3)2(aq)How many moles of calcium hydroxide area.needed to react with 5.88 mol of nitric acid?How many moles of calcium nitrate are b.produced when 2.30 mol of water are made in this reaction?
Chromium combines with oxygen to form114.chromium(III) oxide.
4Cr(s) 3O2(g)gg 2Cr2O3(s)
How many moles of chromium are needed toa.react with 45.6 g of oxygen?How many moles of chromium(III) oxide are b.produced when 2.86 g of chromium react?
Sodium hydroxide is formed when sodium115.oxide reacts with water.
Na2O(s) H2O(l) 2NaOH(aq)
Calculate the grams of sodium hydroxide a.formed when 2.24 moles of sodium oxide react with water.What mass of water (in centigrams) is neededb.to react with 0.126 mol of sodium oxide?
The reaction of nitrogen monoxide with car-116.bon monoxide produces carbon dioxide and nitrogen.
2NO(g) gg 2CO(g)gg 2CO2(g)gg N2(g)gg
How many liters of nitrogen monoxide at a.STP are needed to produce 3.40 mol of nitro-gen gas?When 2.18 moles of nitrogen are made in this b.reaction, how many liters of carbon dioxide at STP are produced?
Hydrogen fluoride gas is produced directly 117.from its component elements.
H2(g) gg F2(g)gg 2HF(g)gg
When 40.0 L of fluorine at STP reacts witha.an excess of hydrogen, how many moles of hydrogen fluoride are made?How many moles of fluorine are needed to b.make 8.04 L of hydrogen fluoride at STP?
Rust (iron(III) oxide) is formed by the reaction 118.of oxygen with iron.
4Fe(s) 3O2(g) gg 2Fe2O3(s)
Calculate the mass of oxygen required toa.react with 10.0 g of iron.How many grams of rust form when 2.48 g of b.iron reacts with an excess of oxygen?
Silver chloride precipitates when aqueous solu-119.tions of calcium chloride and silver nitrate are mixed.CaCl2(aq) 2AgNO3(aq)
2AgCl(s) Ca(NO3)2(aq)How many grams of calcium nitrate are a.formed when 0.500 g of calcium chloridereacts with an excess of silver nitrate?How many grams of calcium chloride areb.required to react completely with 34.8 g of silver nitrate?
The complete combustion of octane, a com-120.ponent of gasoline, forms carbon dioxide andwater.2C8H18(l) 25O2(g) gg
16CO2(g) gg 18H2O(l)How many grams of Ca. 8H18 must be reactedto give 5.00 g of CO2?How many liters of oxygen gas at STP areb.required to burn 2.20 g C8H18?
A precipitate of nickel(II) carbonate forms 121.when aqueous solutions of sodium carbonateand nickel(II) nitrate are mixed.Ni(NO3)2(aq) Na2CO3(aq)
NiCO3(s) 2NaNO3(aq)How many grams of each reactant must be a.used to form 67.2 g of the precipitate?When 1.88 g of nickel(II) carbonate areb.formed, how many grams of sodium nitrate are produced?
One way to make ethanol is to react ethene122.with water at high pressure.
C2H4(g)gg H2O(g)gg C2H6O(l)
How many grams of each reactant are needed a.to produce 8.84 g of ethanol?How many liters of ethanol are producedb.when 1.00 kg of ethene is reacted with an excess of water? The density of ethanol is 0.789 g/mL.
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Problem Bank R59
Chapter 12
109. a. One molecule of hydrogen reacts with one molecule of fluorine to form two molecules of hydrogen fluoride.
b. Two formula units of potassium phosphate react with three formula units of cobalt(II) chloride to form one formula unit of cobalt(II) phosphate and six formula units of potassium chloride.
c. Two formula units of lead(II) sulfide react with three molecules of oxygen to form two formula units of lead(II) oxide and two molecules of sulfur dioxide.
d. One atom of iron reacts with one atom of sulfur to form one formula unit of iron(II) sulfide.
111. a. 138.0 g + 18.0 g = 126.0 g + 30.0 g 156.0 g = 156.0 g
b. 146.0 g + 32.0 g = 36.0 g + 142.0 g 178.0 g = 178.0 g
c. 13.8 g + 32.1 g = 45.9 g 45.9 g = 45.9 g
d. 64.0 g + 96.0 g = 88.0 g + 72.0 g 160.0 g = 160.0 g
112. a. 5.34 mol NO2 b. 0.315 mol H2O
113. a. 2.94 mol Ca(OH)2 b. 1.15 mol Ca(NO3)2
114. a. 1.90 mol Cr b. 0.0275 mol Cr2O3
115. a. 179 g NaOH b. 227 cg H2O
116. a. 152 L NO b. 97.7 L CO2
117. a. 3.57 mol HF b. 0.179 mol F2
118. a. 4.30 g O2 b. 3.55 g Fe2O3
119. a. 0.739 g Ca(NO3)2 b. 11.4 g CaCl2
120. a. 1.62 g C8H18 b. 5.40 L O2
121. a. 103 g Ni(NO3)2 and 60.0 g Na2CO3
b. 2.69 g NaNO3
122. a. 5.38 g C2H4, 3.46 g H2O
b. 2.08 L C 2 H6O
R60 Appendix D
Chapter 12 (continued)
Balance the equation for the formation of 123.aluminum hydroxide, a common ingredient insome antacid tablets.Al2(SO4)3(aq) NaOH(aq)
Al(OH)3(s) Na2SO4(aq)How many grams of sodium hydroxide area.required to react completely with 6.22 g of aluminum sulfate?When 32.0 grams of sodium hydroxide reactsb.with an excess of aluminum sulfate, how many grams of aluminum hydroxide areformed?
One source of elemental oxygen in the labora-124.tory is the decomposition of hydrogen perox-ide.
2H2O2(l) 2H2O(l) O2(g)gg
How many grams of hydrogen peroxide are a.needed to produce 5.00 g of oxygen?When 16.8 g of hydrogen peroxide are b.decomposed, how many liters (at STP) of oxygen are produced?
One source of acid rain is the production of 125.nitric acid from nitrogen dioxide and water inthe atmosphere.3NO2(g) gg H2O(l) NO(g) gg 2HNO3(aq)
How many kilograms of nitric acid area.produced when 5.60 kg of nitrogen dioxidereacts with an excess of water?Calculate the mass in grams of nitrogenb.monoxide produced when 0.648 kg of nitric acid is formed by this reaction.
Steel rails for trains are welded together 126.with the liquid (molten) iron formed by theimmense heat generated by this reaction.
2Al(s) Fe2O3(s) Al2O3(s) 2Fe(l)
How many grams of aluminum are needed a.to react completely with 0.500 kg of iron(III) oxide?How many milliliters of molten iron are b.produced when 80.0 g of iron(III) oxide arereacted with an excess of aluminum? The density of iron is 7.87 g/cm3. Assume thedensities of molten iron and solid iron are the same.
Chlorine gas is made by reacting oxygen with 127.hydrochloric acid.
4HCl(aq) O2(g) gg 2Cl2(g)gg 2H2O(l)
How many grams of each of the reactants are a.required to produce 44.0 g of chlorine?At STP, how many liters of oxygen are needed b.to react completely with 125 g of hydrochlo-ric acid?
Hydrogen fluoride is made by reacting sulfuric128.acid with calcium fluoride.H2SO4(l) CaF2(s) 2HF(g) gg CaSO4(s)
How many grams of hydrogen fluoride anda.calcium sulfate are produced when 2.86 g of calcium fluoride reacts with an excess of sulfuric acid?Calculate the number of kilograms of cal-b.cium fluoride that must react with an excess of sulfuric acid to produce 1.00 kg of hydro-gen fluoride.
When solid dinitrogen pentoxide is heated, it 129.produces oxygen and nitrogen dioxide.
Write the balanced equation for this reaction.a.How many grams of each product are formedb.when 4.00 g of dinitrogen pentoxide is com-pletely decomposed?
Laundry bleach (NaClO) is made by reacting 130.chlorine with sodium hydroxide.Cl2(g)gg 2NaOH(aq)
NaClO(aq) NaCl(aq) H2O(l)How many grams of chlorine must react with a.an excess of sodium hydroxide to produce 2.50 kg of sodium hypochlorite?At room temperature, chlorine gas has ab.density of 2.95 g/L. How many dL of chlorine gas are needed to react completely with 66.8 gof sodium hydroxide?
Bubbling oxygen gas through liquid acetalde-131.hyde (C2H4O) forms a single product, acetic acid.
Write a balanced equation for this reaction.a.How many grams of oxygen are needed to b.react completely with 542 g of acetaldehyde?
R60 Appendix D
APPEN
DIX
D123. Al2(SO4)3(aq) + 6NaOH(aq) → 2Al(OH)3(s) +
3Na2SO4( aq)
a. 4.36 g NaOH b. 20.8 g Al(OH)3
124. a. 10.6 g H2O2 b. 5.53 L O2
125. a. 5.11 kg HNO3 b. 154 g NO
126. a. 169 g Al b. 7.11 mL Fe(l)
127. a. 45.2 g HCl, 9.92 g O2
b. 19.2 L O2
128. a. 1.46 g HF, 4.99 g CaSO4
b. 1.95 kg CaF2
129. a. 2N2O5 → O2 + 4NO2
b. 0.593 g O2, 3.41 g NO2
130. a. 2.38 × 103 g Cl2 b. 201 dL Cl2
131. a. 2C2H4O + O2 → 2C2H4O2
b. 197 g O2
Problem Bank R61
Water is decomposed into its elements by an 132.electric current.
Write a balanced equation for the reaction.a.What is the total volume (in liters at STP)b.of gases produced when 222 g of water aredecomposed?
Oxygen is generated in a rebreathing gas mask 133.by a reaction of water vapor with potassium superoxide, KO2.
4KO2(s) 2H2O(l) 3O2(g) gg 4KOH(s)
How many liters of oxygen gas at STP area.produced when 56.0 g of potassium superox-ide react completely with water vapor?How many grams of potassium hydroxideb.are produced when the 56.0 g of KO2 reactwith an excess of water?
Find the limiting reagent for each set of reac-134.tants. Then calculate the number of moles of each reactant remaining and the amount of each product formed after the reaction.
4NH3(g) gg 3O2(g)gg 2N2(g)gg 6H2O(l)
4.00 mol NHa. 3 4.00 mol O2
2.00 mol NHb. 3 1.00 mol O2
7.00 mol NHc. 3 5.00 mol O2
3.25 mol NHd. 3 2.75 mol O2
Diboron trioxide is formed by reacting 14.0 g135.of diboron hexahydride with 68.0 g of oxygen.
B2H6(g) gg 3O2(g)gg 3H2O(l) B2O3(s)
Identify the limiting reagent.a.Calculate the mass of diboron trioxide pro-b.duced.
When hydrochloric acid is added to calcium136.carbonate, bubbles of carbon dioxide gas are produced.CaCO3(s) 2HCl(aq)
CaCl2(aq) H2O(l) CO2(g)ggWhat is the limiting reagent when 1.68 g of a.HCl is added to 4.82 g CaCO3?In the reaction, how many milliliters of water b.are produced? (density 1.00 g/cm3)What is the volume, in liters, of carbon diox-c.ide produced? Assume STP.
The elements phosphorus and chlorine react to 137.form phosphorus trichloride.
P4(s) 6Cl2(g) gg 4PCl3(l)
What is the limiting reagent when 100.0 g of a.phosphorus reacts with 200.0 g of chlorine?How many grams of phosphorus trichlorideb.are formed?
Hydrogen gas is one of the products of the 138.reaction of aluminum with hydrochloric acid.
2Al(s) 6HCl(aq) AlCl3(aq) 3H2(g)gg
How many grams of H2 are produced when20.0 g of Al reacts with 60.0 g of HCl?
When copper(I) oxide, Cu139. 2O, is heated in oxy-gen, copper(II) oxide is formed.
2Cu2O(s) O2(g)gg 4CuO(s)
When 4.00 mol of copper(I) oxide reactswith 2.00 mol of oxygen, 7.44 mol of CuO is obtained. What is the percent yield of this reaction?
When 7.00 mol C reacts with 5.00 mol SO140. 2,1.80 mol CS2 is formed.
3C(s) 2SO2(g)gg CS2(l) 2CO2(g)gg
What is the percent yield of this reaction?
An excess of water is reacted with 25.0 g of 141.calcium carbide. A mass of 7.20 g of C2H2 isobtained. CaC2(s) 2H2O(l)
C2H2(g)gg Ca(OH)2(aq)What is the percent yield of C2H2?
An excess of sulfur dioxide was reacted with 142.0.150 g of oxygen gas. A mass of 0.725 g of sulfur trioxide was recovered.
2SO2(g) gg O2(g) gg 2SO3(g)gg
What is the percent yield of sulfur trioxide?
When 30.0 g CH143. 4 reacts with 90.0 g O2 and30.0 g NH3, 94.4 g H2O is formed.2CH4(g) gg 3O2(g) gg 2NH3(g) gg
2HCN(g)gg 6H2O(l)What is the percent yield of this reaction?
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Problem Bank R61
132. a. 2H2O → 2H2 + O2
b. 829 L
133. a. 13.2 L b. 44.2 g KOH
134. a. limiting reagent is NH3; after reaction: 0.0 mol NH3, 1.00 mol O2, 2.00 mol N2, and 6 mol H2O
b. limiting reagent is O2; after reaction: 0.67 mol NH3, 0.0 mol O2, 0.67 mol N2, 2.00 mol H2O
c. limiting reagent is O2; after reaction: 0.33 mol NH3, 0.0 mol O2, 3.33 mol N2, 10.00 mol H2O
d. limiting reagent is NH3; after reaction: 0.0 mol NH3, 0.31 mol O2, 1.63 mol N2, and 4.88 mol H2O
135. a. B2H6 is limiting b. 35.3 g B2O3
136. a. HCl is limiting b. 0.414 mL H2O
c. 0.516 L CO2
137. a. chlorine is limiting b. 258 g PCl3
138. 1.64 g H2
139. 93.0%
140. 77.3%
141. 71.3%
142. 96.5%
143. 99.1%
R62 Appendix D
Chapter 13
Make the following pressure conversions:144.364 kPa to atma.815 mm Hg to kPab.0.260 atm to mm Hgc.1555 mm Hg to atmd.85.8 kPa to mm Hge.0.440 atm to kPaf.
Water evaporates much more slowly at room145.temperature than acetone. How does the rela-tive strength of intermolecular forces compare in these two compounds?
In the same location, equal quantities of water146.are poured into a drinking glass and a glass pie pan. In which container will the water evapo-rate first? Explain your choice.
Equal masses of liquid and solid wax are 147.placed in an oven maintained at a temperature exactly at the melting point of the wax. How would the relative amounts of liquid and solid wax change over time?
Chapter 14
A sample of gas at a pressure of 124 kPa has a148.volume of 3.00 L. If the gas is compressed to avolume of 1.26 L, what is its new pressure?(Assume constant temperature.)
A scuba tank has a volume of 11.0 L. What149.volume of gas in liters at 0.950 atm is requiredto completely fill the tank to a pressure of 45.0 atm, assuming no change in the tempera-ture of the gas?
A syringe contains 2.60 mL of gas at 20.0°C.150.What is the volume of gas after the tempera-ture is increased to 68.0°C?
A contained gas has a volume of 120.0 mL at151.183°C. What volume does this gas occupy at
47.0°C?
To what temperature must a contained gas at152.a pressure of 464 mm Hg and a temperature of 40.0°C be raised to increase the pressure to 994 mm Hg?
The pressure of a gas in a cylinder at 27.0°C is 153.846 kPa. What is the pressure in the cylinderwhen the temperature is increased to 54.0°C?
Calculate the final pressure of a gas initially at154.122 kPa pressure that is expanded from 4.50 Lat 56°C to 18.0 L at 124°C.
A weather balloon has a volume of 3.5 kL at 155.1.01 atm and 18°C. What is the balloon’s vol-ume at a pressure of 0.420 atm and 18°C?
A cylinder contains 4.50 L of nitrogen at 35°C156.and a pressure of 644 kPa. How many moles of N2 are in the cylinder?
A balloon containing 1.46 mol of neon gas has157.a volume of 36.2 L.
Under the same conditions, what is the vol-a.ume of the balloon if an additional 0.34 mol of Ne is added to the balloon?Would the answer change if 0.34 mol of Heb.were added instead of neon?
What is the pressure (in kPa) in a 5.00-L tank 158.containing 0.240 mol of oxygen gas at a tem-perature of 17°C?
Calculate the volume of 0.880 mol of fluorine 159.gas at 26°C and 88.8 kPa.
A metal cylinder contains 0.440 mol of nitro-160.gen gas at a pressure of 34.0 kPa. What is the pressure in the container after 0.128 mol of nitrogen are removed?
All the neon gas from a 10.0-L container at a 161.pressure of 202 kPa is added to a 20.0-L con-tainer of argon at a pressure of 505 kPa. After the transfer, what are the partial pressures of neon and argon?
A child buys a balloon filled with 3.50 L of 162.helium on a very hot day when it’s 39.0°C out-side. Assuming a constant pressure, what is thevolume of the balloon when the child bringsthe balloon home to an air-conditioned house at 20.0°C?
Suppose you have a 0.500-L cylinder that con-163.tains 0.150 mol of oxygen gas, O2, at 25°C.
What is the pressure inside the cylinder?a.How would the pressure inside the cylinderb.change if you substituted 0.150 mol of sulfurdioxide gas, SO2 , for the 0.150 mol of oxygen gas?How would the pressure inside the cylin-c.der change if you added 0.150 mol of sulfur dioxide gas, SO2, to the oxygen already in thecylinder?
R62 Appendix D
APPEN
DIX
DChapter 13
144. a. 3.59 atm b. 109 kPa
c. 198 mm Hg d. 2.05 atm
e. 644 mm Hg f. 44.6 kPa
145. The intermolecular forces are greater in water.
146. The water will evaporate faster in the pie pan because of its greater surface area.
147. The relative amount of liquid and solid would remain unchanged.
Chapter 14
148. 295 k pa
149. 521 L
150. 3.03 mL
151. 427 mL
152. 398ºC
153. 922 kPa
154. 36.8 kPa
155. 7.4 kL
156. 1.13 mol N2
157. a. 44.6 L Ne b. no
158. 116 kPa
159. 24.6 L F2
160. 24.1 kPa
161. PNe = 101 kPa; PAr = 505 kPa
162. 3.29 L
163. a. 743 kPa
b. The pressure would not change.
c. The pressure would double to 1.49 × 103 kPa
Problem Bank R63
In a typical automobile engine, the gas mixture 164.in a cylinder is compressed and the pres-sure increases from 1.00 atm to 9.50 atm. If the uncompressed volume of the cylinder is 755 mL, what is the volume when fully com-pressed? (Assume constant temperature.)
What is the new pressure when an aerosol can 165.with an initial pressure of 4.50 atm at 25°C is heated in a fire to 650°C?
How many moles of air are in the lungs of an 166.average person with a total lung capacity of 3.8 L? Assume that the person is at sea level (1.00 atm) and has a normal body temperatureof 37°C.
Two containers of equal size are filled with167.4.0 g of He and 32.0 g of O2, respectively. Assuming a constant temperature, would you expect the pressures of these two gases to be identical? Explain your answer.
Lithium nitride is formed from its elements.168.6Li(s) N2(g) gg 2Li3N(s)
How many milliliters of nitrogen gas at STP are needed to react with 0.246 g of lithium?
Nitrogen and hydrogen react to form ammo-169.nia.
3H2(g)gg N2(g)gg 2NH3(g)gg
How many liters of hydrogen gas measuredat 86.4 kPa pressure and 245°C are needed toreact completely with 6.44 g N2?
Auto air bags are inflated by nitrogen gas 170.formed through this decomposition reaction:
2NaN3(s) 2Na(s) 3N2(g)gg
How many grams of NaN3 are needed toinflate an air bag to a volume of 10.6 L, assum-ing STP?
Chapter 15
Which of these molecules can form hydrogen171.bonds with water?
Ha. 2 c. HClCHb. 3OH d. C2H6
Classify each substance as an electrolyte or a 172.nonelectrolyte.
NHa. 4NO3 c. NaBr2
Cb. 2H6O d. Cl2
Calculate the percent by mass of water in 173.lithium perchlorate trihydrate.
An experiment requires making a solution that 174.contains 34.6 g of CaCl2. Your only source is the hydrate, CaCl2 2H2O. How many gramsof the hydrate do you need to use to obtain therequired mass of CaCl2?
A 19.97-g sample of a hydrate contains 5.08 g175.Cu, 2.57 g S, 5.12 g O, and 7.20 g H2O. What isthe empirical formula of this hydrate?
Chapter 16
The solubility of carbon dioxide gas at 50°C 176.and 1.00 atm pressure is 7.6 10 2 g/100 g H2O. Assuming constant temperature, calcu-late the solubility of CO2 when the pressure isincreased to 2.50 atm.
Calculate the molarity of each of these solu-177.tions.
4.24 mol NaCl in 2.00 L of solutiona.0.164 mol of Cb. 5H10O5 in 125 mL of solution0.0056 mol CsBr in 50.0 mL of solutionc.2.84 mol Cd. 2H6O in 0.650 L of solution
What is the molarity of each of these solutions?178.3.34 g CuNOa. 2 in 0.150 L of solution0.0688 g CoFb. 2 in 20.0 mL of solution88.8 g KOH in 0.755 L of solutionc.1.66 g LiNOd. 3 in 455 mL of solution
Find the moles of solute in the following179.solutions:
650 mL of 0.28a. M NaNOM 3
1.4 L of 0.35b. M KIM0.340 L of 2.22c. M CaCl2
148 mL of 0.0068d. M LiFM
Calculate the mass of solute in each of these180.solutions.
2.00 L of 0.440a. M MgF2
6.80 dL of 1.88b. M CHM 4O65.0 mL of 0.0360c. M NaNOM 3
5.00 mL of 1.48d. M HClM
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Problem Bank R63
164. 79.5 mL
165. 13.9 atm
166. 0.15 mol
167. Yes, because the masses are 1.00 mol of each gas, and equal moles of gases at the same temperature have the same volume.
168. 133 mL N2
169. 34.4 L H2
170. 20.5 g NaN3
Chapter 15
171. a. cannot b. canc. can d. cannot
172. a. electrolyte b. nonelectrolytec. electrolyte d. nonelectrolyte
173. 33.7%
174. 45.8 g CaCl2 ⋅ 2H2O
175. CuSO4 ⋅ 5H2O
Chapter 16
176. 0.19 g/100 g H2O
177. a. 2.12M b. 1.31M c. 0.11M d. 4.37M
178. a. 0.203M b. 3.55 × 10-2Mc. 2.10M d. 5.29 × 10-2M
179. a. 0.18 mol NaNO3 b. 0.49 mol KIc. 0.755 mol Ca(OH)2 d. 1.01× 10-3 mol LiF
180. a. 54.8 g MgF2 b. 40.9 g CH3OHc. 0.199 g NaNO3 d. 0.270 g HCl
R64 Appendix D
How many milliliters of a stock solution of 181. 2.50M SrCl2 solution are required to make each diluted solution?
50.0 mL of 1.00a. M SrCl2
1.0 L of 0.40b. M SrCl2
750 mL of 0.25c. M SrCl2
65.0 dL of 0.146d. M SrCl2
An aqueous solution is 65% (v/v) rubbing 182. alcohol. How many milliliters of alcohol are in a 97-mL sample of this solution?
Calculate the percent by mass of each of these 183. solutions.
6.50 g CsI in 266 g Ha. 2O246 g NaOH in 1.40 kg Hb. 2O0.428 g Kc. 2CO3 in 8.58 g H2O1.20 kg NaNOd. 3 in 2.00 kg H2O
Calculate the mole fraction of each component 184. of the following solutions:
2.40 mol CHa. 4O and 5.36 mol C2H6O1.25 mol Hb. 2O and 87.6 g HCl24.0 g Cc. 2H6O and 10.0 g H2O0.464 g Cd. 2H6O and 2.36 g CH4O
Potassium bromide is dissolved in water. 185. Which statements are true when comparing the solution to pure water?
The boiling point of the solution is higher.a. The vapor pressure of the solution is higher.b. The freezing point of the solution is higher.c.
Calculate the molality of these solutions.186. 0.246 mol KCl in 1.66 kg solventa. 0.116 mol LiNOb. 3 in 844 g solvent56.6 mmol CsI in 1.06 kg solventc. 6.66 mol MgBrd. 2 in 2.50 kg solvent
Calculate the freezing and boiling points of 187. each of these aqueous solutions.
2.34a. m NH4Br1.17b. m CaCl2
24.4 g LiCl in 0.400 kg Hc. 2O44.8 g MgCld. 2 in 1.20 kg H2O
When aqueous solutions of sodium carbon-188. ate and nickel(II) nitrate are mixed, nickel(II) carbonate precipitates.Ni(NO3)2(aq) Na2CO3(aq) NiCO3(s) 2NaNO3(aq)
What volume of 0.366a. M Ni(NO3)2 is required to completely react with 55.8 mL of 0.500M Na2CO3?How many grams of nickel(II) carbonate b. precipitate in this reaction?
Aluminum hydroxide precipitates when aque-189. ous solutions of aluminum sulfate and sodium hydroxide are mixed.Al2(SO4)3(aq) 6NaOH(aq) 2Al(OH)3(s) 3Na2SO4( aq)
What volume of 0.136a. M Al2(SO4)3 is needed to completely react with 26.0 mL of 1.20M NaOH?What mass of aluminum hydroxide precipi-b. tates in this reaction?
A conductivity meter quantitatively measures 190. the ability of an aqueous solution to conduct electrical current. The magnitude of the con-ductivity value is proportional to the number of ions in the solution. Data from an experi-ment are given in the table.
Solutions (0.2M)
Conductivity ( S/cm)
KCl 2050
AlCl3 4500
CaCl2 3540
NaOH 2080
C2H6O 0
Which two of the solutions have similar con-a. ductivities? Why would you expect this?The ratio of the conductivity of the alumi-b. num chloride solution to the conductivity of the potassium chloride solution is approxi-mately two to one. Why would you expect this result?
R64 Appendix D
APPEN
DIX
D181. a. 20.0 mL b. 160 mL
c. 75 mL d. 38.0 mL
182. 63 mL of alcohol
183. a. 2.39% CsI b. 17.6% NaOHc. 4.75% K2CO3 d. 37.5% NaNO3
184. a. 0.309 CH4O and 0.691 C2H6O
b. 0.342 H2O and 0.658 HCl
c. 0.484 C2H6O and 0.516 H2O
d. 0.120 C2H6O and 0.880 CH4O
185. a. true b. falsec. false
186. a. 0.148m KCl b. 0.137m LiNO3
c. 5.34 × 10–2m CsI d. 2.66m MgBr2
187. a. f.p. = –8.70ºC; b.p. = 102.40ºC
b. f.p. = –6.53ºC; b.p. = 101.80ºC
c. f.p. = –5.36ºC; b.p. = 101.47ºC
d. f.p. = –2.19ºC; b.p. = 100.60ºC
188. a. 76.2 mL of 0.366M Ni(NO3)2
b. 3.31 g NiCO3
189. a. 38.2 mL Al2(SO4)3(aq)
b. 0.811 g Al(OH)3
190. a. KCl and NaOH, because they both dissociate to give two particles/formula unit in solution.
b. Since AlCl3 dissociates to give 4 particles/formula unit and KCl dissociates to give 2 particles/formula unit, the conductivity of the aluminum chloride solution should be about twice that of the potassium chloride solution.
Problem Bank R65
Chapter 17
As the mass of a substance increases,191.does its heat capacity increase, decrease, ora.remain constant?does its specific heat increase, decrease, or b.remain constant?
The temperature of a 6.42-gram piece of glass 192.is 15°C. How many calories would it take to increase the temperature of the glass to 96°C?The specific heat of glass is 0.12 cal/(g °C).
Ethanol has a specific heat of 2.43 J/(g193. °C). If 468 J of heat is added to 29.0 g of ethanol ini-tially at 25.0°C, what is the final temperature of the liquid?
When 1564 J of energy is added to a sample 194.of gold at 25.0°C, the temperature of the goldincreases by 424.0°C. What is the mass of the gold? The specific heat of gold is 0.129 J/(g °C).
Identical masses of aluminum and lead at the195.same temperature absorb identical amounts of heat energy. The specific heat of aluminum is 0.901 J/(g °C); the specific heat of lead is0.129 J/(g °C). Which gets hotter, the alumi-num or the lead?
Suppose your diet provides 2100 Cal (kcal) in a196.day, and your body weight is 68 kg. Start withan initial body temperature of a normal 37°C. Calculate the maximum temperature that your body would reach by absorbing all 2100 kcalat once. For purposes of this problem, assumethat your body is 100% water. The specific heat of water is 1.00 cal/(g °C).
Nitrogen monoxide is formed from its elements.197.N2(g)gg O2(g) gg 2NO(g)gg
H 181 kJ/mol
Is this reaction exothermic or endothermic?a.How many kilojoules of energy are needed tob.form 8.70 mol NO?
Carbon dioxide and water are produced by the 198.complete combustion of propane, C3H8.C3H8(g) gg 5O2 (g) gg
3CO2(g) gg 4H2O(g)gg 526 kcalIs this reaction exothermic or endothermic?a.How many kcal of energy are produced whenb.14.4 g C3H8 burns in an excess of oxygen?
The following reaction was used to fuel the199.rockets in the Apollo mission landing module.2N2H4(l) N2O4(l) 3N2(g)gg 4H2O(g)gg
H 1049 kJ
Is this reaction endothermic or exothermic?a.How many grams of Nb. 2H4 must be reacted with an excess of N2O4 to produce 645 kJ of energy?How many kilojoules of energy are produced c.when 5.40 g N2O4 reacts with an excess of N2H4?
The heat of fusion of mercury is 2.30 kJ/mol. 200.How much heat (in J) is released when 24.0 g Hg changes from the liquid state to the solidstate at its freezing point?
How much heat energy is required to change 201.50.0 g of liquid water at 100°C to water vapor at 100°C? The molar heat of fusion is 6.01 kJ/mol, and the molar heat of vaporization is 40.7 kJ/mol.
There is a dramatic temperature change when202.solid ammonium nitrate is dissolved in water.
NH4NO3(s) NH4 (aq) NO3 (aq)HsolnHH 25.7kJ/mol
Is there a temperature increase or decreasea.when ammonium nitrate dissolves in water?Calculate the heat change when 55.0 gb.NH4NO3(s) dissolves in water.s
Use the data in Table 17.4 and the additional 203.values for H° given below to calculate thestandard heat of reaction ( H°) for each of these reactions.
Ethanol is manufactured by reacting water204.with ethane, C2H4.
C2H4(g) gg H2O(l) C2H6O(l)
Use the following equations to calculate theH° for this reaction.
C2H6O(l) 3O2(g)gg 2CO2(g) gg 3H2O(l)H 1367 kJ
C2H4(g) gg 3O2(g)gg 2CO2(g)gg 2H2O(l) H 1411 kJ
Use the following equations to calculate the 205.standard heat of formation, in kJ/mol, of mag-nesium nitrate:2MgO(s) 2Mg(s) O2(g)gg H 1203 kJMg3N2(s) 3Mg(s) N2(g)gg H 463 kJMg(NO3)2(s(( )s 8Mg(s(( )s 6MgO(s(( )s Mg3N2(s(( )s
H 3884 kJ
The heat of sublimation of dry ice (solid CO206. 2)is 25.2 kJ/mol. How many grams of water at 0.0°C would be frozen by the complete sub-limation of 48.0 g of dry ice that is dropped into the water? The heat of fusion of water is 6.01 kJ/mol.
Chapter 18
Nitric oxide reacts with hydrogen to form207.nitrogen gas and water.
2NO(g) gg 2H2(g) gg N2(g) gg 2H2O(g)gg
In an experiment, doubling the H2 concen-tration causes the rate of reaction to double.When the NO concentration is doubled, therate of the reaction increases by a factor of eight. Write the rate law for the reaction.
At equilibrium, are the reactants or the prod-208.ucts favored for reactions that have the follow-ing equilibrium constants?
Ka. eqKK 5.6 10 7 c. KeqKK 5.6 10 14
Kb. eqKK 5.6 1021 d. KeqKK 5.6 105
Write the expression for the equilibrium con-209.stant for each reaction.
Using the equations in Problem 209, calculate 210.the value of KeqKK when the following amountsqof reactants and products are present in a 1-Lcontainer at equilibrium.
1.44 mol PCla. 3, 1.44 mol O2, and 2.60 molPOCl3
0.220 mol HOCl, 4.68 mol Clb. 2O, and 6.82 mol H2O0.0500 mol Brc. 2, 1.00 mol F2, and 0.0465 molBrF5
List three ways to cause a shift in this equilib-211.rium to the right, forming more CH4O(g).gg
CO(g) gg 2H2(g) gg CH4O(g)gg heat
A yellow gas (Y) reacts with a colorless gas (C) 212.to produce a blue gas (B), according to thisequation:
C(g) gg 3Y(g) gg 2B(g)gg heat
The system is initially at equilibrium and has a green color. What happens to the color of thesystem if the following stresses are placed on the system? Note: Blue and yellow mix to form green.
A large amount of colorless C is removeda.from the reaction container.The reaction container is heated.b.
Assume that the following chemical system is213.originally at equilibrium and the color of the liquid is purplish (a mixture of the colors pink and blue):
heat [Co(H2O)6]2 (aq) 4 Cl (aq)
[CoCl4]2 (aq) 6 H2O(l)
How does the color change if chloride ion is a.added to the system?How does the color change if the reactionb.mixture is cooled?
Use Table 18.1 to predict whether a precipitate 214.will form when the following pairs of sub-stances are mixed.
Ka. 2S(aq) Cu(NO3)2(aq)NHb. 4Cl(aq) Pb(NO3)2(aq)Nac. 2CO3(aq) ZnCl2(aq)KNOd. 3(aq) BaCl2(aq)
pink
blue
R66 Appendix D
APPEN
DIX
D204. –44 kJ
205. –188 kJ/mol
206. 82.3 g H2O
Chapter 18
207. rate = [NO]3 [H2]
208. a. reactants b. products
c. reactants d. products
209. a. Keq 53POCl3 4
2
3PCl3 42 3 3O2 4
b. Keq 53Cl2O 4 3 3H2O 4
3HOCl 42
c. Keq 53BrF5 4
2
3Br2 4 3 3F2 45
d. Keq 53NO2 4
2 3 3H2O 48
3N2H4 4 3 3H2O2 4
210. a. Keq = 2.26 b. Keq = 659
c. Keq = 4.32 × 10–2 d. Keq = 3.60 × 106
211. add more CO; add more H2, remove CH4O as it forms, cool the reaction.
212. a. the color turns more yellowish
b. the color turns more yellowish
213. a. the color turns more bluish
b. the color turns more pinkish
214. a. yes b. yes
c. yes d. no
Problem Bank R67
Find the equilibrium concentrations of zinc 215.and sulfide ions in a saturated solution of zincsulfide with KspKK 3.0 10 23.
For each change, does the entropy increase or216.decrease?
A gold nugget melts.a.Liquid wax solidifies.b.Liquid water forms from water vapor.c.Liquid water forms from hydrogen and oxy-d.gen gas.
Chapter 19
Identify each of the species in each equation217.as a Brønsted-Lowry acid or a Brønsted-Lowry base.
Ha. 2O(aq) CN (aq) OH (aq) HCN(aq)
HClOb. 3(aq) H2O(aq)ClO3 (aq) H3O (aq)
Cc. 5H5NH (aq) OH (aq)C5H5N(aq) H2O(aq)
HSOd. 4 (aq) H3O (aq)H2SO4(aq) H2O(aq)
Which of the following are conjugate acid-base218.pairs?
NHa. 4 , NH3
Hb. 3PO4, H2PO4
HSOc. 4 , SO42
Hd. 3O , OH
Ammonia can act as a Lewis base toward 219.which of these compounds?
CHa. 4
BClb. 3
NFc. 3
OFd. 2
Calculate the pH of each solution and classify 220.it as acidic or basic.
Calculate the [H221. ] and the [OH ] from the pH of each solution.
pHa. 6.03pHb. 1.18pHc. 12.68pH d. 4.33pH e. 9.16pH f. 3.46
Rank these acids from strongest to weakest.222.HX, a. KaKK 1 10 4
HY,b. KaKK 1 10 11
HP,c. KaKK 1 10 2
HQ,d. KaKK 1 10 9
Acetylsalicylic acid (aspirin) has a 223. KaKK of 3 × 10 4. A 0.00056M solution of aspirinMwould be best described by which terms: weak, strong, dilute, concentrated?
A 0.10000224. M solution of an unknown acid, MHX, has a hydrogen ion concentration of 3.65 × 10 4M. Calculate the value of KaKK for thisacid.
Name and write the formula for the salt225.formed in each of the following acid-base neutralizations.
aluminum hydroxide with phosphoric acida.oxalic acid with magnesium hydroxideb.sulfurous acid with lithium hydroxidec.sodium hydroxide with carbonic acidd.
How many moles of sulfuric acid are required 226.to neutralize 1.40 mol of potassium hydroxide?2KOH(aq) H2SO4(aq)
K2SO4(aq) 2H2O(l)
What is the molarity of a hydrochloric acid227.solution if 25.0 mL of the solution reacts com-pletely with 1.66 g NaHCO3?HCl(aq) NaHCO3(s)
NaCl(aq) H2O(l) CO2(g)gg
In an acid base titration, how many mL of 228.0.180M HCl are required to neutralize 20.0 mLof 0.220M NaOH?M
How many milliliters of 0.456229. M Ca(OH)M 2 are needed to neutralize 25.0 mL of 0.300M HCl?M
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Problem Bank R67
215. [Zn2+] = [S2–] = 5.5 × 10–12 M
216. a. increase b. decrease
c. decrease d. decrease
Chapter 19
217. a. H2O(aq) + CN–(aq) OH–(aq) + HCN(aq) acid base base acid
b. HClO3(aq) + H2O(aq) ClO3–(aq) + H3O
+(aq) acid base base acid
c. C5H5NH+(aq) + OH–(aq) C5H5N(aq) + H2O(aq) acid base base acid
d. HSO4– (aq) + H3O
+(aq) H2SO4(aq) + H2O(aq) acid base base acid
218. a. yes b. yesc. yes d. no
219. a. no b. yesc. no d. no
220. a. 3.34, acidic b. 7.92, basicc. 10.92, basic d. 3.45, acidice. 1.41, acidic f. 5.18, acidic
221 a. [H+] = 9.3 × 10–7M , [OH–] = 1.1 × 10–8M
b. [H+] = 6.6 × 10–2M, [OH–] = 1.5 × 10–13M
c. [H+] = 2.1 × 10–13M, [OH–] = 4.8 × 10–2M
d. [H+] = 4.7 × 10–5M, [OH–] = 2.1 × 10–10M
e. [H+] = 6.9 × 10–10M, [OH–] = 1.4 × 10–5M
f. [H+] = 3.5 × 10–4M, [OH–] = 2.9 × 10–11M
222. c. > a. > d. > b.
223. a dilute solution of a weak acid
224. 1.34 × 10–6
225. a. aluminum phosphate, AlPO4
b. magnesium oxalate, MgC2O4
c. lithium sulfite, Li2SO3
d. sodium carbonate, Na2CO3
226. 0.700 mol H2SO4
227. 0.790M HCl
228. 24.4 ml HCl
229. 8.22 mL Ca(OH)2
R68 Appendix D
A buffer (HBrO/BrO230. ) solution is made by mixing together equal quantities of hypobro-mous acid (HBrO) and sodium hypobromite (NaBrO).
Write an equation for the reaction that a.occurs when an acid is added to this buffer.Write an equation for the reaction that b.occurs when a base is added to this buffer.
Chapter 20
What is the oxidation number of sulfur in each231.of these species?
SFa. 6 d. SO3
CaSb. 2O3 e. SKc. 2SO3 f. H2SO4
What is the oxidation number of bromine in232.each of the following?
CsBra. d. Br2
NaBrOb. 3 e. BrClBrOc. 2 f. NaBrO
Consider the following reaction: 233.CuCl2(aq) Fe(s) Cu(s) FeCl2(aq)
Which reactant lost electrons?a.What is the oxidizing agent?b.Which reactant was oxidized in this reaction?c.What is the reducing agent?d.
In each of these reactions, is sulfur oxidized or 234.reduced?
HgS(a. s)s Hg(l) S(s)sS(b. s) s O2(g) gg SO3(g)ggHc. 2SO4(aq) Ca(s)s H2S(g)gg Ca2 (aq)Al(d. s)s S(s) s Al2S3(s)s
Balance each of the equations in Problem 234.235.
Balance each of the following redox reactions 236.and classify each as a combination, decomposi-tion, or single-replacement reaction.
Mg(a. s) s H2O(l) Mg(OH)2 H2(g)ggPFb. 3(g) gg F2(g) gg PF5(g)ggCc. 2H2(g) gg H2(g) gg C2H6(g)ggNaNOd. 3(s) s NaNO2(s) s O2(g)gg
Iron(II) sulfite reacts with an acid solution of 237.permanganate ion.5FeSO3 14H 3MnO4
3Mn2 5Fe3 5SO42 7H2O
What is the oxidation number of iron and of a.manganese in the reactants?What is the oxidation number of sulfur andb.of oxygen in SO4
2 ?Identify the oxidizing agent in this reaction.c.What is reduced in this reaction?d.
Write a balanced chemical equation for each 238.of these reactions, and identify the element oxidized and the element reduced.
Nitrogen monoxide reacts with hydrogen to a.form nitrogen and water.Potassium permanganate, iron(II) sul-b.fate, and sulfuric acid react, producing manganese(II) sulfate, iron(III) sulfate, potassium sulfate, and water.Elemental phosphorus (Pc. 4) and nitrogen monoxide react to form tetraphosphorushexoxide and nitrogen.Sulfur dioxide, nitric acid, and water react to d.produce sulfuric acid and nitrogen monoxide.
Balance each redox equation by the oxidation-239.number-change method. Identify the oxidizing agent and the reducing agent.
What happens when a strip of zinc is dipped241.into a solution of aluminum chloride?
A strip of aluminum is dipped into a solution242.of nickel(II) sulfate. Explain the result.
A voltaic cell is constructed using the follow-243.ing half-ff reactions:Ag (aq) e Ag(s) E°Ag 0.80 VAl3 (aq) 3e Al(s) E°Al3 1.66 VDetermine the cell reaction.
Calculate the standard cell potential for the244.voltaic cell described in Problem 243.
What process, reduction or oxidation, always 245.occurs at the anode of an electrolytic cell?
Chapter 22
What bonding properties make carbon 246.uniquely suited to make a very large number of organic compounds?
Draw structural formulas for these com-247.pounds.
3-phenylpentanea.2-phenyl-1-buteneb.
Describe the structural features of an alkene 248.molecule that permits the existence of cisf , transisomers.
How is an asymmetric carbon produced in an249.organic molecule?
Which of these structures are250. cis isomers?
a.
b.
HH
c.
d.
C CH
CH3CH2 H
CH2CH3
C CCH3
H H
CH3
C CH
H CH3
CH3
e.C C
H
CH3CH2 H
CH2CH2CH3
C CCH3
H H
Write the IUPAC names for these structures. 251.Use cis and trans prefixes when appropriate.
a.
C CH
CH3CH2 CH3
H
e. C CCH3
CH3 H
CH2CH3
c. C CHCH2CH2CH3
CH3
CH3
CH3CH(CH2)7CH3
CH2CH3
CH3
CH3
b.
d.
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Problem Bank R69
Chapter 21
241. nothing
242. The aluminum strip will become nickel plated.
243. Al(s) + 3Ag+(aq) → Al3+(aq) + 3Ag(s)
244. Standard cell potential is: +9.66 V
245. oxidation
Chapter 22
246. the ability of carbon atoms to form four stable covalent bonds with other carbon atoms
247. a. CH2CH3
CH2CH3
b.
CH3CH2CHCH2CH3
c. CH2CH3
CH2CH2CH3
d.
CH2 CCH2CH3H
e. CH2CH3
CH3CH2 CH2CH3
248. carbon–carbon double bond
249. four different groups attached to a carbon atom
250. b., d.
251. a. cis-2-pentene b. methylcyclooctane c. 2-methyldecane d. 2-methyl-2-pentene e. 2-methyl-3-ethyl-2-hexene
R70 Appendix D
What name is given to a benzene ring when it 252.is a substituent in an organic molecule?
Are benzene rings more resistant or less resis-253.tant to chemical reactions than the carbon-carbon double bond in an alkane? Explainyour answer.
Which structural feature(s) characterize 254.alkanes?
carbon-hydrogen single bondsa.carbon-carbon double bondsb.carbon-carbon single bondsc.may contain branched chainsd.may contain phenyl substituentse.
Draw structural formulas for these com-255.pounds.
If you want to devise an industrial process256.to prepare methylbenzene, would you preferpetroleum or coal as your starting material? Explain your choice.
Chapter 23
Name the functional group in these molecular257.structures.
CH3CH2Br
CO2H
CH3CH2CH2OCH3
CH3CH2CCH2CH
O CH3
CH3
CH2NHCH3
a.
b.
c.
e.
d.
Which of these structures represent aryl 258.halides?
CH2CH3
Br
a.
Fb.
CH2Clc.
F
CF3
e.
CH Id.
Cl
If 5.23 g of an alkene is required to completely 259.decolorize 9.92 g of bromine, what is the molar mass of the alkene?
Write structural formulas for the organic prod-260.uct of these reactions.
CH2 CHCH2CH3 Cl2a.
CH CH2
Br2b.
HClc.
Br2d. catalyst
R70 Appendix D
APPEN
DIX
D252. phenyl
253. more resistant because the benzene ring is stabilized by resonance
254. a., c., d., e.
256. coal, because it contains aromatic compounds from which benzene can be readily made.
Chapter 23
257. a. halogen b. carboxyl c. amino d. carbonyle. ether
258. b., d, e.
259. 84.2 g/mol
260.
b.CHCH2
Br Br
a.CH2CHCH2CH3
Cl Cl
d.Br
c.
ClH
Problem Bank R71
Treatment of 7.57 g of pentanoic acid with a 261.large excess of ethanol in the presence of a catalytic amount of hydrochloric acid pro-duced 8.21 g of ethyl pentanoate after purifica-tion. Write a balanced equation for the reac-tion and calculate the percent yield of the ester.
Classify these reactions as oxidation or reduc-262.tion.
CHCH3 CCH3K2Cr2O7
H2SO4
a.
CH3CH2CH2CH2CHOCH3CH2CH2CH2CO2H
CuSO4b.
CH2CH3 3H2
CH2CH3
c.
d. CH4 2O2 CO2 2H2O
Pt
OOH
How many liters of hydrogen gas at STP are 263.required to saturate 0.150 mole of benzene?
Write complete equations for the following or-264.ganic reactions. Be sure to include all reactants and catalysts required for the transformations.
1-pentene to pentanea.2,3-dimethyl-2-butene to 2-chloro-2,3-dime-b.thylbutaneethane to chloroethanec.cyclohexene to 1,2-dibromocyclohexaned.
A sample of benzaldehyde is oxidized to pro-265.duce the crystalline white solid, benzoic acid. Write the structural formula of benzoic acid.
Complete these reactions.266.
Classify each of these reactions as a hydration,267.hydrogenation, hydrolysis, or substitution.
a.
b.
c.
d.
H2OH
100°C
H
CH2Cl KOH
CH2OH KCl
H2O
100°C
CH2CH3
C CH 2H2
COCH3 H2O
O
COH CH3OH
O
OH
Pt
Chapter 24
Saliva contains an enzyme called amylase,268.which catalyzes the breakdown of starch to its monomers. Suggest a reason why a piece of bread begins to taste sweet when it has been chewed for a short time.
262. a. oxidation b. oxidationc. reduction d. oxidation
263. 10.1 L
264. a.
b.
c.
d.
265. CO2H
266. a.
b.
c.
d.
267. a. substitution b. hydrolysisc. hydration d. hydrogenation
Chapter 24
268. Action of amylase breaks down starch to its glucose monomers; glucose tastes sweet.
PtCH2 CHCH2CH2CH3 + H2 CH3CH2CH2CH2CH3
Br
Br
+ Br2
CH3CH3 + Cl2UV light + HClCH3CH2Cl
C CCH3 CH3
CH3CH3
+ HCl C C
CH3 CH3
CH3CH3
H Cl
CH3CH2CH2OH + KI
CH3CH2COOH
CHCH2
OH
CCH2
O
R72 Appendix D
Which of these statements apply to enzymes?269.do not change position of equilibriuma.catalyze biological reactionsb.bind substrates and sometimes cofactors at c.active siteschange position of equilibrium to favor d.productsare almost always nucleic acidse.
If one molecule of the enzyme catalase can 270.break down 3.60 106 peroxide molecules in one minute, how many minutes would it take this enzyme molecule to break down 1 mole of peroxide? How many hours?
The level of glucose in the blood is normally 271.70–120 mg/dL. If a student’s volume of blood is 4.5 L and her blood glucose level is 90 mg/dL,what is the total number of grams of glucose inher blood?
Sucrose, ordinary table sugar, has the molecu-272.lar formula C12H22O11.
What is the molar mass of sucrose?a.What is the molarity of an aqueous solution b.containing 7.12 g/L of sucrose?Write a balanced equation for the completec.combustion of sucrose in air.
A student eats a 115-g hamburger that contains273.20.0% by mass of fat. The chemical potential energy of fat is 37.7 kJ/gram.
How many grams of fat does the hamburger a.contain?How many kilojoules of energy are stored in b.the fat?What is this amount of energy in dietary c.Calories?What percentage of total Calories does d.this amount of energy represent in a 2.00 103 Calorie/day diet?
Walnuts, rich in fats and oils and with a chem-274.ical potential energy of 25.8 kJ/g, are a nutri-tious treat for many people. Suppose you eat27.3 g of walnuts and then take a brisk walk.If you burn 3.76 102 kJ of kinetic energy foreach kilometer you walk, how far will you need to walk to use up the energy provided by thewalnuts?
There are 3.4 base pairs in every complete turn 275.of the double helix in a DNA molecule. How many turns are in a DNA molecule that con-tains 5.0 108 base pairs?
ATP is not the only biological molecule capable 276.of transmitting energy. For example, hydrolysisof the molecule phosphoenolpyruvic acid re-leases even more free energy than the hydroly-sis of ATP. Use the equations below to write anet equation showing that the energy releasedby the hydrolysis of phosphoenolpyruvic acid can be coupled to the phosphorylation of ADPto form ATP in a spontaneous reaction.Phosphoenolpyruvic acid H2O
pyruvic acid Pi
G 61.4 kJ/mol
ADP Pi ATP H2OG 30.5 kJ/mol
The hydrolysis of ATP to ADP and inorganic 277.phosphate releases 30.5 kJ/mol of free energy. If all of this energy is wasted as heat, how many moles of ATP must be hydrolyzed to raise the temperature of 1 L of water at 20°C to 37°C?
Chapter 25
How do the mass number and the atomic278.number of radioactive atom A change if itfirst emits an alpha particle and the resultingatom then emits a beta particle to finally give atom C?
A radioactive active atom undergoes beta 279.decay to yield cesium-133. Write a balanced equation for this nuclear reaction.
Which nuclei would you predict to be stable?280.Explain your answer.
9a. 3Li c. 208O
59b. 27Co d. 14660Nd
Write a balanced nuclear equation for the fol-281.lowing:
beta decay of sodium-26a.alpha decay of b. 234
92U
Plutonium-239 presents a serious nuclear282.waste disposal problem. If seven half-ff lives arerequired for the radioactivity from the wasteto reach a tolerable level and if Pu-239 has at1/2 2.41 104 years, how long must the Pu-239 be stored?
R72 Appendix D
APPEN
DIX
D269. a., b., c.
270. 1.67 x 1017 minutes; 2.78 x 1015 hours
271. 4.1 g
272. a. 342.0 g/mol b. 2.08 x 10–2M c. C12H22O11 + 12O2 → 12CO2 + 11H2O
273. a. 23.0 g b. 8.67 x 102 kJc. 2.07 x 102 Cal d. 10.4%
274. 1.87 km
275. 1.5 x 108 turns
276. Add the equations and the free energies to obtain
phosphoenolpyruvic acid + ADP ATP + pyruvic acid
ΔG = –30.9 kJ/mol
Transfer of a phosphoryl group from phosphoenolpyruvate to ADP to form ATP is spontaneous.
277. 2.33 mol ATP
Chapter 25
278. The mass number of atom C is 4 less than that of atom A; the atomic number of C is 1 less than that of atom A.
279. 54
133Xe → 55133Cs + −1
0β
280. b. and d. stable; neutron-to-proton ratio in Band of Stability.
