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ISBN 10: 1-292-02062-8
ISBN 13: 978-1-292-02062-4
British Library Cataloguing-in-Publication Data
A catalogue record for this book is available from the British Library
Printed in the United States of America
CHEMICAL REACTIONS AND QUANTITIES
111
112
113
Gasohol is a fuel that contains ethanol 1C2H6O2, which burns
in oxygen 1O22 to give carbon dioxide and water. (6, 7)
a. Write the balanced equation for the combustion of ethanol.
b. How many moles of O2 are needed to completely react with
4.0 moles of C2H6O?
c. If a car produces 88 g of CO2, how many grams of O2 are
used up in the reaction?
d. If you add 125 g of C2H6O to your fuel, how many grams
of CO2 and H2O can be produced from the ethanol?
114
When ammonia 1NH32 reacts with fluorine, the products are
dinitrogen tetrafluoride and hydrogen fluoride. (1, 6, 7)
a. Write the balanced equation for the reaction.
b. How many moles of each reactant are needed to produce
4.00 moles of HF?
c. How many grams of F2 are required to react with 25.5 g of
NH3?
d. How many grams of N2F4 can be produced when 3.40 g of
NH3 reacts?
When peroxide 1H2O22 is used in rocket fuels, it produces
water and oxygen 1O22. (1, 6, 7)
a. Write the balanced equation for the reaction.
b. How many moles of peroxide are needed to produce
3.00 moles of water?
c. How many grams of peroxide are required to produce
36.5 g of O2?
d. How many grams of water can be produced when 12.2 g of
peroxide reacts?
Ethane gas, C2H6, reacts with chlorine gas, Cl2, to form
hexachloroethane gas, C2Cl6, and hydrogen chloride gas.
(1, 6, 7)
a. Write the balanced equation for the reaction.
b. How many moles of chlorine gas must react to produce
1.60 moles of hexachloroethane?
c. How many grams of hydrogen chloride are produced when
50.0 g of ethane reacts?
d. How many grams of hexachloroethane are produced when
50.0 g of ethane reacts?
Propane gas, C3H8, a fuel for many barbecues, reacts with
oxygen to produce water and carbon dioxide. Propane has a
density of 2.02 g/L at room temperature. (1, 4, 6, 7)
Pearson Education
110
Propane is converted to carbon
dioxide and water when used as a
fuel in a barbecue.
115
116
a. Write the balanced equation for the reaction.
b. How many grams of water form when 5.00 L of propane
gas completely react?
c. How many grams of CO2 are produced from 18.5 g of oxygen gas and excess propane?
d. How many grams of H2O can be produced from the reaction of 8.50 * 1022 molecules of propane gas?
Acetylene gas, C2H2, burns in oxygen to produce carbon
dioxide and water. If 62.0 g of CO2 is produced when 22.5 g
of C2H2 reacts with sufficient oxygen, what is the percent
yield of CO2 for the reaction? (1, 6, 7, 8)
When 50.0 g of iron(III) oxide reacts with carbon monoxide,
32.8 g of iron is produced. What is the percent yield of Fe for
the reaction? (6, 7, 8)
Fe 2O31s2 + 3CO1g2 h 2Fe1s2 + 3CO21g2
C HA LLE NG E Q UES TIO NS
117
Pentane gas, C5H12, reacts with oxygen to produce carbon
dioxide and water. (6, 7, 8)
119
C5H121g2 + 8O21g2 h 5CO21g2 + 6H2O1g2
Pentane
118
a. How many grams of pentane must react to produce
4.0 moles of water?
b. How many grams of CO2 are produced from 32.0 g of oxygen and excess pentane?
c. How many grams of CO2 are formed if 44.5 g of C5H12 is
reacted with 108 g of O2?
120
121
3NO21g2 + H2O1l2 h 2HNO31aq2 + NO1g2
256
2Na1s2 + Cl21g2 h 2NaCl1s2
If a mixture of 35.8 g of CH4 and 75.5 g of S reacts, how many
grams of H2S are produced? (6, 7, 8)
CH41g2 + 4S1g2 h CS21g2 + 2H2S1g2
The formation of nitrogen oxide, NO, from N21g2 and O21g2,
requires 21.6 kcal of heat. (9)
N21g2 + O21g2 h 2NO1g2
When nitrogen dioxide 1NO22 from car exhaust combines with
water in the air, it forms nitric acid 1HNO32, which causes acid
rain, and nitrogen oxide. (6, 7, 8)
a. How many molecules of NO2 are needed to react with
0.250 mole of H2O?
b. How many grams of HNO3 are produced when 60.0 g of
NO2 completely reacts?
c. How many grams of HNO3 can be produced if 225 g of
NO2 is reacted with 55.2 g of H2O?
When a mixture of 12.8 g of Na and 10.2 g of Cl2 reacts, what
is the mass of NaCl that is produced? (6, 7, 8)
122
H = +21.6 kcal
a. How many kilocalories are required to form 3.00 g
of NO?
b. What is the complete equation (including heat) for the
decomposition of NO?
c. How many kilocalories are released when 5.00 g of NO
decomposes to N2 and O2?
The formation of rust 1Fe 2O32 from solid iron and oxygen gas
releases 1.7 * 103 kJ. (9)
4Fe1s2 + 3O21g2 h 2Fe 2O31s2
H = - 1.7 * 103 kJ
CHEMICAL REACTIONS AND QUANTITIES
a. How many kilojoules are released when 2.00 g of Fe
reacts?
b. How many grams of rust form when 150 kcal are
released?
c. What is the complete equation (including heat) for the formation of rust?
123
124
Write a balanced equation for each of the following reaction
descriptions and identify each type of reaction: (1, 2)
a. An aqueous solution of lead(II) nitrate is mixed with aqueous sodium phosphate to produce solid lead(II) phosphate
and aqueous sodium nitrate.
b. Gallium metal heated in oxygen gas forms solid
gallium(III) oxide.
c. When solid sodium nitrate is heated, solid sodium nitrite
and oxygen gas are produced.
d. Solid bismuth(III) oxide and solid carbon react to form bismuth metal and carbon monoxide gas.
126
2C2H21g2 + 5O21g2 h 4CO21g2 + 2H2O1g2
127
A gold bar is 2.31 cm long, 1.48 cm wide, and 0.0758 cm
thick. (4, 5)
a. If gold has a density of 19.3 g/mL, what is the mass, in
grams, of the gold bar?
b. How many atoms of gold are in the bar?
c. When the same mass of gold combines with oxygen, the
oxide product has a mass of 5.61 g. How many moles of O
are combined with the gold?
Consider the following equation: (1, 2, 6, 7, 8)
a. Balance the equation.
b. Identify the type of reaction.
c. How many moles of oxygen are needed to react with
4.50 moles of Al?
d. How many grams of aluminum oxide are produced when
50.2 g of aluminum reacts?
e. When 13.5 g of aluminum is reacted with 8.00 g of oxygen,
how many grams of aluminum oxide can form?
f. If 45.0 g of aluminum and 62.0 g of oxygen undergo a
reaction that has a 70.0% yield, what mass of aluminum
oxide forms?
Components in
toothpaste include
triclosan and NaF.
125
a. How many moles of water are produced from the complete
reaction of 2.50 moles of oxygen?
b. How many grams of oxygen are needed to react completely
with 2.25 g of acetylene?
c. How many grams of carbon dioxide are produced from the
complete reaction of 78.0 g of acetylene?
d. If the reaction in part c produces 186 g of CO2, what is the
percent yield of CO2 for the reaction?
Al1s2 + O21g2 h Al2O31s2
A toothpaste contains 0.24% by mass sodium fluoride 1NaF2
used to prevent dental caries and 0.30% by mass triclosan,
C12H7Cl3O2, a preservative and antigingivitis agent. One tube
contains 119 g of toothpaste. (4, 5)
Pearson Education
a. How many moles of NaF are in the tube of toothpaste?
b. How many fluoride ions 1F -2 are in the tube of
toothpaste?
c. How many grams of sodium ion 1Na+2 are in 1.50 g of
toothpaste?
d. How many molecules of triclosan are in the tube of
toothpaste?
The gaseous hydrocarbon acetylene, C2H2, used in welders’
torches, releases a large amount of heat when it burns according to the following equation: (6, 7, 8)
128
Consider the equation for the reaction of sodium and nitrogen
to form sodium nitride. (1, 2, 6, 7, 8)
Na1s2 + N21g2 h Na 3N1s2
a. Balance the equation.
b. If 80.0 g of sodium is reacted with 20.0 g of nitrogen gas,
what mass of sodium nitride forms?
c. If the reaction in part b has a percent yield of 75.0%, how
many grams of sodium nitride are actually produced?
AN SW ER S
Answers to Study Checks
Answers to Selected Questions and Problems
1 2Al1s2 + 3Cl21g2 h 2AlCl31s2
2 Sb 2S31s2 + 6HCl1aq2 h 2SbCl31s2 + 3H2S1g2
3 0.432 mole of H2O
4 0.120 mole of aspirin
5 138.1 g/mole
6 80.9 g of Ag
3 a.
b.
c.
d.
e.
b. balanced
d. balanced
N21g2 + O21g2 h 2NO1g2
2HgO1s2 h 2Hg1l2 + O21g2
4Fe1s2 + 3O21g2 h 2Fe 2O31s2
2Na1s2 + Cl21g2 h 2NaCl1s2
2Cu2O1s2 + O21g2 h 4CuO1s2
5 a. Mg1s2 + 2AgNO31aq2 h Mg1NO3221aq2 + 2Ag1s2
b. CuCO31s2 h CuO1s2 + CO21g2
7 0.945 mole of O2
c. C5H121g2 + 8O21g2 h 5CO21g2 + 6H2O1g2
d. Pb1NO3221aq2 + 2NaCl1aq2 h
PbCl21s2 + 2NaNO31aq2
e. 2Al1s2 + 6HCl1aq2 h 2AlCl31aq2 + 3H21g2
8 27.5 g of CO2
9 84.7% yield
10 14.2 g of SO2
11 a. endothermic
1 a. not balanced
c. not balanced
b. 10.5 kJ
257
CHEMICAL REACTIONS AND QUANTITIES
7 a.
b.
c.
d.
decomposition reaction
single replacement reaction
combustion reaction
double replacement reaction
9 a.
b.
c.
d.
e.
f.
single replacement reaction
combination reaction
decomposition reaction
combustion reaction
double replacement reaction
double replacement reaction
11 a. Mg1s2 + Cl21g2 h MgCl21s2
b. 2HBr1g2 h H21g2 + Br21g2
c. Mg1s2 + Zn1NO3221aq2 h
Zn1s2 + Mg1NO3221aq2
d. K2S1aq2 + Pb1NO3221aq2 h
2KNO31aq2 + PbS1s2
e. 2C5H101l2 + 15O21g2 h 10CO21g2 + 10H2O1g2
13 a. reduction
c. reduction
15 a.
b.
c.
d.
b. oxidation
d. reduction
Zn is oxidized; Cl2 is reduced.
Br - in NaBr is oxidized; Cl2 is reduced.
The O2- in PbO is oxidized; the Pb2+ is reduced.
Sn2+ is oxidized; Fe3+ is reduced.
17 a. reduction
b. oxidation
19 Linoleic acid gains hydrogen atoms and is reduced.
21 a. 1.20 * 1023 atoms of Ag
b. 4.52 * 1023 molecules of C3H8O
c. 7.53 * 1023 atoms of Cr
23 a. 5.42 moles of Al
c. 0.478 mole of Au
b. 14.1 moles of C2H5OH
25 a. 24 moles of H
c. 0.040 mole of N
b. 1.0 * 102 moles of C
27 a. 3.01 * 1023 atoms of C
b. 7.71 * 1023 molecules of SO2
c. 0.0867 mole of Fe
258
1 mole O2
2 moles SO2
and
1 mole O2
2 moles SO2
2 moles SO3
2 moles SO2
and
2 moles SO3
2 moles SO2
2 moles SO3
1 mole O2
and
1 mole O2
2 moles SO3
5 moles O2
4 moles P
b.
and
5 moles O2
4 moles P
2 moles P2O5
4 moles P
and
2 moles P2O5
4 moles P
2 moles P2O5
5 moles O2
and
2 moles P2O5
5 moles O2
45 a.
29 a. 6.00 moles of H
c. 1.20 * 1024 atoms of P
b. 8.00 moles of O
d. 4.82 * 1024 atoms of O
31 a. 188.2 g/mole
c. 329.2 g/mole
e. 58.3 g/mole
b. 159.8 g/mole
d. 342.3 g/mole
f. 365.3 g/mole
33 a. 46.0 g
c. 14.8 g
b. 112 g
d. 112 g
35 a. 29.3 g
c. 4.05 g
b. 109 g
d. 194 g
37 a. 602 g
b. 11 g
39 a. 0.463 mole of Ag
c. 0.882 mole of NH3
b. 0.0167 mole of C
d. 1.17 moles of SO2
41 a. 0.78 mole of S
c. 0.601 mole of S
b. 1.95 moles of S
43 a. 165 g of caffeine
c. 1.15 moles of C
b. 0.144 mole of caffeine
d. 8.08 g of N
47 a. 1.0 mole of O2
b. 10. moles of H2 c. 5.0 moles of H2O
49 a. 1.25 moles of C
c. 1.0 mole of SO2
b. 0.96 mole of CO
d. 0.50 mole of CS2
51 a. 77.5 g of Na 2O
b. 6.26 g of O2
c. 19.4 g of O2
53 a. 19.2 g of O2
b. 3.79 g of N2
c. 54.0 g of H2O
55 a. 3.65 g of H2O
b. 3.43 g of NO
c. 7.53 g of HNO3
57 a.
b.
c.
d.
2PbS1s2 + 3O21g2 h 2PbO1s2 + 2SO21g2
6.00 g of O2
17.4 g of SO2
137 g of PbS
59 a. 70.9%
b. 63.2%
61 70.8 g of Al2O3
63 60.4%
65 a. Eight taxis can be used to pick up passengers.
b. Seven taxis can be driven.
67 a. 5.0 moles of H2
b. 4.0 moles of H2 c. 3.0 moles of N2
69 a. limiting reactant SO2; 2.00 moles of SO3
b. limiting reactant H2O; 0.500 mole of Fe 3O4
c. limiting reactant O2; 1.27 moles of CO2
71 a. limiting reactant Cl2; 25.1 g of AlCl3
b. limiting reactant O2; 13.5 g of H2O
c. limiting reactant O2; 26.7 g of SO2
73 a. The activation energy is the energy required to break the
bonds of the reacting molecules.
b. In exothermic reactions, the energy of the products is lower
than that of the reactants.
c.
Energy
Reactants
Products
Reaction progress
75 a. exothermic
b. endothermic
77 a. exothermic; H = -890 kJ
b. endothermic; H = +65.3 kJ
c. exothermic; H = -205 kcal
79 578 kJ are released
c. exothermic
CHEMICAL REACTIONS AND QUANTITIES
81 a. 1, 1, 2 combination reaction
b. 2, 2, 1 decomposition reaction
83 a. reactants NO, O2; product NO2
b. 2NO1g2 + O21g2 h 2NO21g2
c. combination reaction
89 1. a. S2Cl2
2. a. C6H6
b. 135.2 g/mole
b. 78.1 g/mole
c. 0.0740 mole
c. 0.128 mole
91 a. 252 g/mole
b. 0.0991 mole
c. 0.991 mole of C
93 a.
b.
c.
d.
66.2 g of propane
0.771 mole of propane
27.8 g of C
2.77 * 1022 atoms of H
95 a. NH31g2 + HCl1g2 h NH4Cl1s2 Combination
b. Fe 3O41s2 + 4H21g2 h 3Fe1s2 + 4H2O1g2
Single replacement
c. 2Sb1s2 + 3Cl21g2 h 2SbCl31s2 Combination
d. C5H121g2 + 8O21g2 h 5CO21g2 + 6H2O1g2
Combustion
e. 2KBr1aq2 + Cl21aq2 h 2KCl1aq2 + Br21l2
Single replacement
f. Al21SO4231aq2 + 6NaOH1aq2 h
3Na 2SO41aq2 + 2Al1OH231s2 Double replacement
97 a.
b.
c.
d.
99 a.
b.
c.
d.
e.
f.
101 a.
b.
c.
d.
b. 389.9 g/mole
c. 169.1 g/mole
105 a. 5.87 g
b. 10.7 g
c. 15.9 g
107 a. 0.568 mole
b. 0.321 mole
c. 0.262 mole
109 a. 242 g of glucose
b. 123 g of ethanol
85 a. reactant NI 3; products N2, I 2
b. 2NI 31s2 h N21g2 + 3I 21g2
c. decomposition reaction
87 a. reactants Cl2, O2; product OCl2
b. 2Cl21g2 + O21g2 h 2OCl21g2
c. combination reaction
103 a. 161.5 g/mole
Zn1s2 + 2HCl1aq2 h ZnCl21aq2 + H21g2
BaCO31s2 h BaO1s2 + CO21g2
NaOH1aq2 + HCl1aq2 h NaCl1aq2 + H2O1l2
2Al1s2 + 3F21g2 h 2AlF31s2
Cu01s2 is oxidized and H +1aq2 is reduced.
Fe01s2 is oxidized and Ni2+1aq2 is reduced.
Ag 01s2 is oxidized and Cu2+1aq2 is reduced.
Cr01s2 is oxidized and Ni2+1aq2 is reduced.
Zn01s2 is oxidized and Cu2+1aq2 is reduced.
Zn01s2 is oxidized and Pb2+1aq2 is reduced.
111 a.
b.
c.
d.
2NH31g2 + 5F21g2 h N2F41g2 + 6HF1g2
1.33 moles of NH3 and 3.33 moles of F2
143 g of F2
10.4 g of N2F4
113 a.
b.
c.
d.
C2H61g2 + 6Cl21g2 h C2Cl61g2 + 6HCl1g2
9.60 moles of chlorine
364 g of HCl
394 g of hexachloroethane
115 81.4%
117 a. 48 g of C5H12
b. 27.5 g of CO2
c. 92.8 g of CO2
119 16.8 g of NaCl
121 a. 1.08 kcal are released
b. 2NO1g2 h N21g2 + O21g2 + 21.6 kcal
c. 1.80 kcal are required
123 a. 3Pb1NO3221aq2 + 2Na 3PO41aq2 h
Pb 31PO4221s2 + 6NaNO31aq2 Double replacement
b. 4Ga1s2 + 3O21g2 h 2Ga 2O31s2 Combination
c. 2NaNO31s2 h 2NaNO21s2 + O21g2 Decomposition
d. Bi2O31s2 + 3C1s2 h 2Bi1s2 + 3CO1g2
Single replacement
125 a. 5.00 g of gold
b. 1.53 * 1022 atoms of Au
c. 0.038 mole of oxygen
127 a.
b.
c.
d.
e.
f.
4Al1s2 + 3O21g2 h 2Al2O31s2
combination reaction
3.38 moles of oxygen
94.8 g of aluminum oxide
17.0 g of aluminum oxide
59.5 g of aluminum oxide
90.1 g/mole
3.01 * 1023 molecules
2.71 * 1024 atoms of C
220 g of lactic acid
259
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