Chemistry And Chemical Reactivity International Edition 8th Edition By John C. Kotz – Test Bank
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Sample Test
Chapter 3—Chemical Reactions
MULTIPLE CHOICE
1. Nitroglycerin
decomposes violently according to the balanced chemical equation below.
2 C3H5(NO3)3() ® 3 N2(g) + 1/2 O2(g) +
6 CO2(g) + 5 H2O(g)
Which of the following statements concerning this reaction
is/are CORRECT?
|
|
1. |
Two moles of nitroglycerine will
produce three moles of nitrogen and five moles of water. |
|
|
2. |
Four molecules of nitroglycerine will
produced one molecule of oxygen and twelve molecules of carbon dioxide. |
|
|
3. |
Six grams of nitroglycerine will
produce nine grams of nitrogen and fifteen grams of water. |
|
a. |
1 only |
|
b. |
2 only |
|
c. |
3 only |
|
d. |
1 and 2 |
|
e. |
1, 2, and 3 |
ANS: D
2. The
reaction of tetraphosphorus decaoxide with water produces phosphoric acid.
__ P4O10 + __ H2O ®
__ H3PO4
What are the respective coefficients when the equation is
balanced with the smallest integer values?
|
a. |
1, 1, 1 |
|
b. |
1, 3, 1 |
|
c. |
2, 4, 1 |
|
d. |
2, 6, 2 |
|
e. |
1, 6, 4 |
ANS: E
3. When
propane undergoes complete combustion, the products are carbon dioxide and
water.
__ C3H8(g) + __ O2(g) ® __ CO2(g) +
__ H2O(g)
What are the respective coefficients when the equation is
balanced with the smallest whole numbers?
|
a. |
1, 1, 1, 1 |
|
b. |
1, 3, 1, 3 |
|
c. |
1, 3, 3, 1 |
|
d. |
1, 5, 3, 4 |
|
e. |
2, 5, 3, 4 |
ANS: D
4. The
reaction of elemental chlorine with potassium iodide yields elemental iodine
and potassium chloride. Write a balanced chemical equation for this reaction.
|
a. |
Cl2(g) + KI(s) ® I(s) + KCl2(s) |
|
b. |
Cl2(g) + 2 KI(s) ® I2(s) + 2 KCl(s) |
|
c. |
Cl2(g) + KI2(s) ® I2(s) + KCl2(s) |
|
d. |
Cl(g) + KI(s) ® I(s) + KCl(s) |
|
e. |
Cl2(g) + 2 K2I(s) ® I2(s) + 2 K2Cl(s) |
ANS: B
5. Metals
react with oxygen gas to produce oxides with the general formula MxOy.
Write a balanced chemical equation for the reaction of titanium with oxygen to
yield titanium(IV) oxide.
|
a. |
4 Ti(s) + O2(g) ® 2 Ti2O(s) |
|
b. |
Ti(s) + O2(g) ® TiO2(s) |
|
c. |
2 Ti(s) + O2(g) ® 2 TiO(s) |
|
d. |
Ti(s) + O(g) ® TiO(s) |
|
e. |
8 Ti(s) + O2(g) ® 2 Ti4O(s) |
ANS: B
6. The
products of the complete combustion of octane, C8H18, are
carbon dioxide and water. Write a balanced chemical equation for this reaction.
|
a. |
C8H18() ® 8 C(s) + 9 H2(g) |
|
b. |
C8H18() + 25 O2(g) ® 8 CO2 (g) + 9 H2O(g) |
|
c. |
2 C8H18() + 25 O2(g) ® 16 CO2(g) + 18 H2O(g) |
|
d. |
C8H18() + 16 O2(g) ® 8 CO2(g) + 9 H2(g) |
|
e. |
2 C8H18() + 17 O2(g) ® 16 CO(g) + 18 H2O(g) |
ANS: C
7. What
is the balanced chemical equation for the complete combustion of benzoic acid,
C6H5CO2H, to form carbon dioxide and water?
|
a. |
C6H5CO2H(s) ® 6 C(s) + CO2(g) + 3 H2(g) |
|
b. |
C6H5CO2H(s) ® 7 CO2(g) + 3 H2O(g) |
|
c. |
C6H5CO2H(s) + O2(g) ® CO2(g) + H2O(g) |
|
d. |
C6H5CO2H(s) + 8 O2(g) ® 7 CO2(g) + 3 H2O(g) |
|
e. |
2 C6H5CO2H(s) + 15 O2(g) ® 14 CO2(g) + 6 H2O(g) |
ANS: E
8. Which
of the following statements is/are CORRECT?
|
|
1. |
A solution is a homogeneous mixture of
two or more substances. |
|
|
2. |
A solute is a mixture of a solvent and
a soluble compound. |
|
|
3. |
Aqueous solutions are solutions in
which water is a solvent. |
|
a. |
1 only |
|
b. |
2 only |
|
c. |
3 only |
|
d. |
1 and 2 |
|
e. |
1 and 3 |
ANS: E
9. Which
of the following statements is/are CORRECT?
|
|
1. |
All ionic compounds that are soluble in
water are electrolytes. |
|
|
2. |
All ionic compounds dissolve in water. |
|
|
3. |
Molecular compounds are never soluble
in water. |
|
a. |
1 only |
|
b. |
2 only |
|
c. |
3 only |
|
d. |
1 and 2 |
|
e. |
2 and 3 |
ANS: A
10.
Which of the following statements is/are CORRECT?
|
|
1. |
Water soluble ionic compounds, such as
NaCl, are strong electrolytes. |
|
|
2. |
Some molecular compounds, such as HCl,
are strong electrolytes. |
|
|
3. |
Some molecular compounds, such as
acetic acid, are weak electrolytes. |
|
a. |
1 only |
|
b. |
2 only |
|
c. |
3 only |
|
d. |
1 and 2 |
|
e. |
1, 2, and 3 |
ANS: E
11.
Which one of the following compounds is a nonelectrolyte when
dissolved in water?
|
a. |
HCl |
|
b. |
CaCl2 |
|
c. |
CCl4 |
|
d. |
Cu(NO3)2 |
|
e. |
NaCH3CO2 |
ANS: C
12.
Which of the following statements is/are CORRECT?
|
|
1. |
Most ionic compounds containing nitrate
ion are soluble in water. |
|
|
2. |
Most ionic compounds containing sulfate
ion are insoluble in water. |
|
|
3. |
Most ionic compounds containing
carbonate ion are soluble in water. |
|
a. |
1 only |
|
b. |
2 only |
|
c. |
3 only |
|
d. |
1 and 2 |
|
e. |
1, 2, and 3 |
ANS: A
13.
Which of the following statements is/are CORRECT?
|
|
1. |
Most ionic compounds containing
phosphate ion are insoluble in water. |
|
|
2. |
Most ionic compounds containing
potassium ion are insoluble in water. |
|
|
3. |
Most ionic compounds containing
hydroxide ion are soluble in water. |
|
a. |
1 only |
|
b. |
2 only |
|
c. |
3 only |
|
d. |
1 and 2 |
|
e. |
1, 2, and 3 |
ANS: A
14.
Which of the following compounds are soluble in water: K2CO3,
CaCO3, NiCO3, and Fe2(CO3)3?
|
a. |
K2CO3 only |
|
b. |
K2CO3 and CaCO3 |
|
c. |
CaCO3 and NiCO3 |
|
d. |
NiCO3 and Fe2(CO3)3 |
|
e. |
CaCO3, NiCO3, and Fe2(CO3)3 |
ANS: A
15.
Which of the following compounds are soluble in water: NH4NO3, Fe2S3,
CuCO3, and SrCl2?
|
a. |
NH4NO3 only |
|
b. |
NH4NO3 and Fe2S3 |
|
c. |
Fe2S3 and CuCO3 |
|
d. |
CuCO3 and SrCl2 |
|
e. |
NH4NO3 and SrCl2 |
ANS: E
16.
All of the following compounds are insoluble in water except
____.
|
a. |
BaCO3 |
|
b. |
PbF2 |
|
c. |
Fe(OH)3 |
|
d. |
Ni(ClO4)2 |
|
e. |
PbCrO4 |
ANS: D
17.
A precipitate will form when aqueous Pb(NO3)2 is
added to an aqueous solution of ____.
|
a. |
Cu(NO3)2 |
|
b. |
NaI |
|
c. |
NaCH3CO2 |
|
d. |
Pb(ClO4)2 |
|
e. |
KNO3 |
ANS: B
18.
A precipitate will form when aqueous nickel(II) chloride is
added to an aqueous solution of ____.
|
a. |
SrI2 |
|
b. |
Cu(NO3)2 |
|
c. |
KOH |
|
d. |
Na2SO4 |
|
e. |
NaBr |
ANS: C
19.
If an aqueous solution of ____ is added to a mixture of Pb2+ and
Ba2+, the lead ion will precipitate, but the barium ion will remain
in solution.
|
a. |
NaOH |
|
b. |
Na2SO4 |
|
c. |
K3PO4 |
|
d. |
KCO3 |
|
e. |
Ca(CH3CO2)2 |
ANS: A
20.
If an aqueous solution of ____ is added to a mixture of F– and
SO42–, the fluoride ion
will precipitate, but the sulfate ion will remain in solution.
|
a. |
LiBr |
|
b. |
HNO3 |
|
c. |
Pb(ClO4)2 |
|
d. |
MgNO3 |
|
e. |
AlCl3 |
ANS: D
21.
Write a balanced chemical equation for the reaction of aqueous
solutions of sodium sulfide and zinc(II) chloride.
|
a. |
Na2S(aq) + ZnCl2(aq) ® ZnS(s) + 2 NaCl(aq) |
|
b. |
Na2S(aq) + ZnCl2(aq) ® ZnS(s) + 2 NaCl(s) |
|
c. |
Na2S(aq) + ZnCl2(aq) ® Na2Zn(s) + SCl2(aq) |
|
d. |
Na2S(aq) + ZnCl2(aq) ® Na2Zn(aq) + SCl2(g) |
|
e. |
No reaction occurs. |
ANS: A
22.
Write a balanced chemical equation for the reaction of aqueous
solutions of magnesium chloride and potassium phosphate.
|
a. |
MgCl2(aq) + K3PO4(aq) ® K3Mg(s) + PO4Cl2(aq) |
|
b. |
3 MgCl2(aq) + 2 K3PO4(aq) ® 3 K2Mg(s) + 2 PO4Cl3(aq) |
|
c. |
MgCl(aq) + KPO4(aq) ® MgPO4(s) + KCl(aq) |
|
d. |
MgCl2(aq) + 2 KPO4(aq) ® Mg(PO4)2(s) + 2 KCl(aq) |
|
e. |
3 MgCl2(aq) + 2 K3PO4(aq) ® Mg3(PO4)2(s) + 6 KCl(aq) |
ANS: E
23.
What is the net ionic equation for the reaction of aqueous
nickel(II) acetate and aqueous sodium carbonate?
|
a. |
Ni2+(aq) + 2 CH3CO2–(aq) ® Ni(CH3CO2)2(s) |
|
b. |
Na+(aq) + CH3CO2–(aq) ® NaCH3CO2(aq) |
|
c. |
Na+(aq) + CH3CO2–(aq) ® NaCH3CO2(s) |
|
d. |
Ni2+(aq) + CO32–(aq) ® NiCO3(s) |
|
e. |
Ni2+(aq) + 2 Na+(aq) ® NiNa2(s) |
ANS: D
24.
What is the net ionic equation for the reaction of aqueous
sodium hydroxide and aqueous iron(II) chloride?
|
a. |
Na+(aq) + OH–(aq) ® NaOH(s) |
|
b. |
Na+(aq) + Cl–(aq) ® NaCl(s) |
|
c. |
Fe2+(aq) + 2 OH–(aq) ® Fe(OH)2(s) |
|
d. |
Fe2+(aq) + OH–(aq) ® FeOH+(s) |
|
e. |
Fe2+(aq) + 2 Cl–(aq) ® FeCl2(s) |
ANS: C
25.
Which of the following compounds is a weak acid?
|
a. |
HCl |
|
b. |
H3PO4 |
|
c. |
HNO3 |
|
d. |
HClO4 |
|
e. |
H2SO4 |
ANS: B
26.
Which of the following compounds is a weak base?
|
a. |
NaOH |
|
b. |
H2CO3 |
|
c. |
LiCl |
|
d. |
NH3 |
|
e. |
CH3CO2H |
ANS: D
27.
Sulfuric acid is the product of the reaction of ____ and H2O.
|
a. |
SO3 |
|
b. |
SO2 |
|
c. |
S8 |
|
d. |
H2S |
|
e. |
SO42– |
ANS: A
28.
Write a balanced equation for the reaction that occurs when hydrogen
sulfate ion behaves as a Brønsted-Lowry acid in water.
|
a. |
HSO4–(aq) + H2O() H2SO4(aq) + H3O+(aq) |
|
b. |
SO42–(aq) + H2O() HSO4–(aq) + OH–(aq) |
|
c. |
HSO4–(aq) + H2O() SO42–(aq) + H3O+(aq) |
|
d. |
HSO4–(aq) + H2O() H2SO4(aq) + OH–(aq) |
|
e. |
H2SO4(aq) + H2O() HSO4–(aq) + H3O+(aq) |
ANS: C
29.
What is the balanced equation for carbonate ion (CO32–)
acting as a Brønsted base in a reaction with water?
|
a. |
CO32–(aq) + 3 H2O() CO44–(aq) + 2 H3O+(aq) |
|
b. |
CO32–(aq) + H2O() HCO3–(aq) + OH–(aq) |
|
c. |
CO32–(aq) + H2O() CO2(g) + 2 OH–(aq) |
|
d. |
CO32–(aq) + 2 H2O() HCO3–(aq) + H3O+(aq) |
|
e. |
CO32–(aq) + H2O() H2CO42–(aq) |
ANS: B
30.
What is the net ionic equation for the reaction of aqueous
hydrochloric acid and aqueous potassium hydroxide?
|
a. |
HCl(aq) + OH–(aq) ® H2O() + Cl–(aq) |
|
b. |
Cl–(aq) + K+(aq) ® KCl(s) |
|
c. |
HCl(aq) + KOH(aq) ® KCl(aq) + H2O() |
|
d. |
Cl–(aq) + K+(aq) ® KCl(aq) |
|
e. |
H+(aq) + OH–(aq) ® H2O() |
ANS: E
31.
What are the spectator ions in the reaction between aqueous
hydrobromic acid and aqueous sodium hydroxide?
|
a. |
Na+ only |
|
b. |
H+ and OH– |
|
c. |
Na+ and Br– |
|
d. |
Br– only |
|
e. |
H+, Br–, Na+, and OH– |
ANS: C
32.
What are the spectator ions in the reaction between aqueous
nitric acid and ammonia?
|
a. |
H+ only |
|
b. |
NO3– only |
|
c. |
H+ and NH4+ |
|
d. |
NO3– and NH4+ |
|
e. |
H+, NO3–, and NH4+ |
ANS: B
33.
Hydrocyanic acid, HCN, is a weak acid. Write a net ionic
equation for the reaction of aqueous hydrocyanic acid and aqueous sodium
hydroxide.
|
a. |
HCN(aq) + NaOH(aq) ® Na+(aq) + CN–(aq) + H2O() |
|
b. |
HCN(aq) + H2O(aq) ® CN–(aq) + H3O+(aq) |
|
c. |
H+(aq) + OH–(aq) ® H2O() |
|
d. |
HCN(aq) + OH–(aq) ® CN–(aq) + H2O() |
|
e. |
H+(aq) + NaOH(aq) ® Na+(aq) + H2O() |
ANS: D
34.
Which of the following compounds will produce a basic solution
when dissolved in water?
|
a. |
CaO |
|
b. |
NaHSO4 |
|
c. |
CO2 |
|
d. |
SO2 |
|
e. |
KCl |
ANS: A
35.
Metal oxides react with water to produce ____.
|
a. |
bases |
|
b. |
hydrogen gas |
|
c. |
oxygen gas |
|
d. |
acids |
|
e. |
hydronium ions |
ANS: A
36.
Write a balanced net ionic equation for the reaction of calcium sulfide
and aqueous nitric acid.
|
a. |
CaS(s) + 2 H+(aq) ® Ca2+(aq) + S2–(aq) + H2(g) |
|
b. |
CaS(s) + 2 H+(aq) ® Ca2+(aq) + H2S(g) |
|
c. |
CaS(s) + 2 HNO3(aq) ® Ca(NO3)2(aq) + H2S(g) |
|
d. |
CaS(s) + 2 HNO3(aq) ® Ca(NO3)2(s) + H2S(s) |
|
e. |
S2–(aq) + 2 H+(aq) ® H2S(g) |
ANS: B
37.
Write a balanced net ionic equation for the reaction of aqueous
solutions of baking soda (NaHCO3) and
acetic acid.
|
a. |
HCO3–(aq) + CH3CO2H(aq) ® CH3CO2–(aq) + H2O() + CO2(g) |
|
b. |
2 NaHCO3(aq) + CH3CO2H(aq) ® 2 Na2CO3(aq) + CH4(aq) + 2H2O() + CO2(g) |
|
c. |
NaHCO3(aq) + H+(aq) ® H2CO3(s) + Na+(aq) |
|
d. |
HCO3–(aq) + H+(aq) ® H2O() + CO2(g) |
|
e. |
HCO3–(aq) + H+(aq) ® H2CO3(aq) |
ANS: A
38.
Write a balanced chemical equation for the reaction of aqueous
solutions of ammonium sulfate and sodium hydroxide.
|
a. |
(NH4)2SO4(aq) + 2 NaOH(aq) ® 2 NH4OH(aq) + SO3(g) + Na2O(aq) |
|
b. |
(NH3)2SO4(aq) + NaOH(aq) ® 2 NH3(g) + NaOHSO4(aq) |
|
c. |
(NH3)2SO4(aq) + 2 NaOH(aq) ® 2 NH3(g) + Na2SO4(aq) + 2 OH–(aq) |
|
d. |
(NH4)2SO4(aq) + 2 NaOH(aq) ® 2 NH4+(g) + Na2SO4(aq) + 2 OH–(aq) |
|
e. |
(NH4)2SO4(aq) + 2 NaOH(aq) ® 2 NH3(g) + 2 H2O() + Na2SO4(aq) |
ANS: E
39.
Which molecule in the reaction below is the oxidizing agent?
2 C2H6(g) + 7 O2(g) ® 4 CO2(g) +
6 H2O(g)
|
a. |
C2H6 |
|
b. |
O2 |
|
c. |
H2O |
|
d. |
CO2 |
|
e. |
None |
ANS: B
40.
Which species in the reaction below undergoes reduction?
H2O(g) + CO(g) ® H2(g) +
CO2(g)
|
a. |
H2O |
|
b. |
CO |
|
c. |
H2 |
|
d. |
CO2 |
|
e. |
None |
ANS: A
41.
Which species is reduced in the reaction below?
I–(aq) + ClO–(aq) ® IO–(aq)
+ Cl–(aq)
|
a. |
I– |
|
b. |
H2O |
|
c. |
Cl– |
|
d. |
IO– |
|
e. |
ClO– |
ANS: E
42.
What is the oxidation number of iodine in potassium iodate, KIO3?
|
a. |
–1 |
|
b. |
0 |
|
c. |
+3 |
|
d. |
+5 |
|
e. |
+7 |
ANS: D
43.
What is the oxidation number of sulfur in sulfur in H2S?
|
a. |
–2 |
|
b. |
0 |
|
c. |
+2 |
|
d. |
+4 |
|
e. |
+6 |
ANS: A
44.
What is the oxidation number of each atom in sulfurous acid, H2SO3?
|
a. |
H = +1, S = –2, O = –2 |
|
b. |
H = 0, S = +6, O = –2 |
|
c. |
H = 0, S = 0, O = 0 |
|
d. |
H = +1, S = +4, O = –2 |
|
e. |
H = –1, S = +8, O = –2 |
ANS: D
45.
What is the oxidation number of each atom in sodium hydrogen
carbonate, NaHCO3?
|
a. |
Na = +1, H = –1, C = +6, O = –2 |
|
b. |
Na = +1, H = +1, C = +4, O = –2 |
|
c. |
Na = +1, H = –1, C = +2, O = –2 |
|
d. |
Na = –1, H = +1, C = 0, O = –2 |
|
e. |
Na = 0, H = 0, C = 0, O = 0 |
ANS: B
46.
Which of the following elements generally acts as an oxidizing
agent?
|
a. |
Br2 |
|
b. |
H2 |
|
c. |
Fe |
|
d. |
C |
|
e. |
Li |
ANS: A
47.
Which of the following chemical equations show
oxidation-reduction reactions?
|
|
1. |
Mg(s) + I2(aq) ® MgI2(s) |
|
|
2. |
Pb(ClO4)2(aq) + 2 KI(aq) ® PbI2(s) + 2 KClO4(aq) |
|
|
3. |
Fe2O3(s) + 3 CO(g) ® 2 Fe(s) + 3 CO2(g) |
|
a. |
1 only |
|
b. |
2 only |
|
c. |
1 and 2 |
|
d. |
1 and 3 |
|
e. |
2 and 3 |
ANS: D
48.
Which of the following chemical equations is an acid-base
reaction?
|
a. |
Ba(OH)2(aq) + K2SO4(aq) ® BaSO4(s) + 2 KOH(aq) |
|
b. |
3 NaOH(aq) + AlCl3(aq) ® Al(OH)3(s) + 3 NaCl(aq) |
|
c. |
2 H+(aq) + Zn(s) ® H2(g) + Zn2+(aq) |
|
d. |
2 HCl(aq) + Pb(NO3)2(aq) ® PbCl2(s) + 2 HNO3(aq) |
|
e. |
H3PO4(aq) + NH3(aq) ® NH4+(aq) + H2PO4–(aq) |
ANS: E
49.
All of the following are oxidation-reduction reactions EXCEPT
|
a. |
CaCO3(s) ® CaO(s) + CO2(g) |
|
b. |
2 Na(s) + Br2(g) ® 2 NaBr(g) |
|
c. |
Fe(s) + 2 HCl(aq) ® FeCl2(aq) + H2(g) |
|
d. |
2 C(s) + O2(g) ® 2 CO(g) |
|
e. |
2 H2O() ® 2 H2(g) + O2(g) |
ANS: A
SHORT ANSWER
50.
A(n) ________ agent loses electrons in an oxidation-reduction
reaction.
ANS:
reducing
51.
________ acid is produced in a larger quantity than any other
chemical in the United States. This chemical is used in the production of
fertilizers, pigments, alcohol, paper and detergents.
ANS:
Sulfuric
52.
The net ionic equation for the reaction of barium chloride and
sodium sulfate is shown below.
Ba2+(aq) + SO42–(aq)
® BaSO4(s)
Chloride and sodium ions are referred to as ________ ions
because they are not involved in the reaction.
ANS:
spectator
53.
A solution is a homogeneous mixture composed of one or
more ____________ dissolved in a solvent.
ANS:
solutes
54.
Give the name of an acidic oxide and write a balanced chemical
equation for the reaction of the oxide with water.
ANS:
Sulfur dioxide. SO2(g) +
H2O() ® H2SO3(aq).
Other examples include carbon dioxide forming carbonic acid, sulfur trioxide
forming sulfuric acid, and nitrogen dioxide forming a mixture of nitrous acid
and nitric acid.
55.
If an aqueous sodium hydroxide solution is left in contact with
air, the concentration of hydroxide ion gradually decreases. The process can be
hastened if a person exhales over a sodium hydroxide solution. Write a balanced
chemical equation that describes the process by which the hydroxide ion
concentration decreases.
ANS:
OH–(aq) + CO2(aq) ® HCO3–(aq)
Chapter 5—Principles of Chemical Reactivity: Energy and Chemical
Reactions
MULTIPLE CHOICE
1. Which
of the following statements is/are CORRECT?
|
|
1. |
A system is defined as an object or
collection of objects being studied. |
|
|
2. |
Surroundings are defined as the entire
universe, including the system. |
|
|
3. |
In an endothermic reaction, heat is
transferred from the system to the surroundings. |
|
a. |
1 only |
|
b. |
2 only |
|
c. |
3 only |
|
d. |
1 and 3 |
|
e. |
1, 2, and 3 |
ANS: A
2. A hot
piece of iron is dropped into a beaker containing colder water. Which of the
following statements is/are CORRECT?
|
|
1. |
Energy is transferred as heat from the
iron to the water. |
|
|
2. |
Thermal equilibrium is attained when
the iron and the water reach the same temperature. |
|
|
3. |
Thermal energy from the iron is
converted to electrostatic energy in the water. |
|
a. |
1 only |
|
b. |
2 only |
|
c. |
3 only |
|
d. |
1 and 2 |
|
e. |
1, 2, and 3 |
ANS: D
3. Which
one of the following statements is INCORRECT?
|
a. |
Energy is neither created nor destroyed
in chemical reactions. |
|
b. |
Kinetic energy is the energy that
results from an object’s position. |
|
c. |
Exothermic processes transfer heat from
the system into the surroundings. |
|
d. |
Increasing the thermal energy of a gas
increases the motion of its atoms. |
|
e. |
Energy is the capacity to do work. |
ANS: B
4. Many
homes are heated using natural gas. The combustion of natural gas converts
|
a. |
chemical potential energy to thermal
energy. |
|
b. |
thermal energy to mechanical energy. |
|
c. |
mechanical energy to chemical
potential. |
|
d. |
electrostatic energy to mechanical
energy. |
|
e. |
gravitational energy to acoustic
energy. |
ANS: A
5. Which
of the following processes is/are endothermic?
|
|
1. |
the combustion of hydrogen |
|
|
2. |
the condensation of water |
|
|
3. |
the evaporation of isopropyl alcohol |
|
a. |
1 only |
|
b. |
2 only |
|
c. |
3 only |
|
d. |
1 and 3 |
|
e. |
1, 2, and 3 |
ANS: C
6. Which
of the following processes is/are exothermic?
|
|
1. |
the reaction of butane with oxygen |
|
|
2. |
the melting of gold |
|
|
3. |
cooling copper from 225 °C to 65 °C |
|
a. |
1 only |
|
b. |
2 only |
|
c. |
3 only |
|
d. |
1 and 3 |
|
e. |
1, 2, and 3 |
ANS: D
7. Specific
heat capacity is
|
a. |
the quantity of heat needed to change
the temperature of 1.00 g of a substance by 1 K. |
|
b. |
the quantity of heat needed to change
the temperature of 1.00 g of a substance by 4.184 K. |
|
c. |
the capacity of a substance to gain or
lose a 1.00 J of energy in the form of heat. |
|
d. |
the temperature change undergone when
1.00 g of a substance absorbs 4.184 J. |
|
e. |
the maximum amount of energy in the
form of heat that 1.00 g of a substance may absorb without decomposing. |
ANS: A
8. Heat
capacity is defined as
|
a. |
the amount of heat required to raise
the temperature of 1 gram of substance by 1 K. |
|
b. |
the amount of heat required to raise
the temperature of a substance by 1 K. |
|
c. |
the amount of heat required to vaporize
a solid or liquid. |
|
d. |
the maximum amount of heat that a substance
may absorb without decomposing. |
|
e. |
4.18 cal/g×K. |
ANS: B
9. Which
of the following statements is/are CORRECT?
|
|
1. |
Specific heat capacity is a positive
value for liquids and solids and a negative value for gases. |
|
|
2. |
The larger the heat capacity of an
object, the more thermal energy it can store. |
|
|
3. |
When heat is transferred from the
surroundings to the system, q is
negative. |
|
a. |
1 only |
|
b. |
2 only |
|
c. |
3 only |
|
d. |
1 and 2 |
|
e. |
1, 2, and 3 |
ANS: B
10.
If 495 J is required to change the temperature of 12.7 g of
sodium chloride from 275.0 K to 335.0 K, what is the specific heat capacity of
sodium chloride?
|
a. |
0.866 J/g×K |
|
b. |
2.60 J/g×K |
|
c. |
0.650 J/g×K |
|
d. |
1.15 J/g×K |
|
e. |
2.83 ´ 105 J/g×K |
ANS: C
11.
If the same amount of energy in the form of heat is added to
5.00 g samples of each of the metals below, which metal will undergo the
largest temperature change?
|
|
Metal |
Specific Heat Capacity (J/g×K) |
|
|
Ag |
0.235 |
|
|
Al |
0.897 |
|
|
Cu |
0.385 |
|
|
Fe |
0.449 |
|
|
Hg |
0.140 |
|
a. |
Ag |
|
b. |
Al |
|
c. |
Cu |
|
d. |
Fe |
|
e. |
Hg |
ANS: E
12.
If 50.0 g of benzene, C6H6, at
25.0 °C absorbs 2.71 kJ of energy in the form of heat, what is the final
temperature of the benzene? The specific heat capacity of benzene is 1.72
J/g×K.
|
a. |
25.0 °C |
|
b. |
31.5 °C |
|
c. |
56.5 °C |
|
d. |
32.3 °C |
|
e. |
57.3 °C |
ANS: C
13.
How much energy (in kJ) is required to change the temperature of
325 g aluminum from 32 °C to 815 °C? The specific heat capacity of aluminum is
0.897 J/g×K.
|
a. |
238 kJ |
|
b. |
284 kJ |
|
c. |
46.3 kJ |
|
d. |
228 kJ |
|
e. |
2.16 kJ |
ANS: D
14.
If 35.0 g H2O at 22.7 °C is
combined with 65.0 g H2O at 87.5 °C, what is
the final temperature of the mixture? The specific heat capacity of water is
4.184 J/g×K.
|
a. |
25.1 °C |
|
b. |
45.4 °C |
|
c. |
50.8 °C |
|
d. |
64.8 °C |
|
e. |
48.9 °C |
ANS: D
15.
If 46.1 g Cu at 11.6 °C is placed in 85.0 g H2O at
72.4 °C, what is the final temperature of the mixture? The specific heat
capacities of copper and water are 0.385 J/g×K and 4.184 J/g×K, respectively.
|
a. |
71.2 °C |
|
b. |
63.6 °C |
|
c. |
51.0 °C |
|
d. |
42.0 °C |
|
e. |
69.5 °C |
ANS: E
16.
When 66.0 g of an unknown metal at 28.5 °C is placed in 83.0 g H2O at
78.5 °C, the water temperature decreases to 75.9 °C. What is the specific heat
capacity of the metal? The specific heat capacity of water is 4.184 J/g×K.
|
a. |
0.055 J/g×K |
|
b. |
0.29 J/g×K |
|
c. |
0.69 J/g×K |
|
d. |
0.18 J/g×K |
|
e. |
2.6 J/g×K |
ANS: B
17.
Calculate the energy in the form of heat (in kJ) required to
convert 325 grams of liquid water at 20.0 °C to steam at 115 °C. Assume that no
energy in the form of heat is transferred to the environment. (Heat of fusion =
333 J/g; heat of vaporization = 2256 J/g; specific heat capacities: liquid
water = 4.184 J/g×K, steam = 1.92 J/g×K)
|
a. |
129 kJ |
|
b. |
121 kJ |
|
c. |
851 kJ |
|
d. |
914 kJ |
|
e. |
735 kJ |
ANS: C
18.
Calculate the energy in the form of heat (in kJ) required to
change 75.0 g of liquid water at 27.0 °C to ice at –20.0 °C. Assume that no
energy in the form of heat is transferred to the environment. (Heat of fusion =
333 J/g; heat of vaporization = 2256 J/g; specific heat capacities: ice = 2.06
J/g×K, liquid water = 4.184 J/g×K)
|
a. |
–13.4 kJ |
|
b. |
–17.7 kJ |
|
c. |
–36.5 kJ |
|
d. |
–10.2 kJ |
|
e. |
–30.3 kJ |
ANS: C
19.
44.0 g of ice at –20.0 °C is mixed with 325 g of water at 32.1
°C. Calculate the final temperature of the mixture. Assume that no energy in
the form of heat is transferred to the environment. (Heat of fusion = 333 J/g;
specific heat capacities: ice = 2.06 J/g×K, liquid water = 4.184 J/g×K)
|
a. |
–0.6 °C |
|
b. |
5.5 °C |
|
c. |
12.1 °C |
|
d. |
17.6 °C |
|
e. |
38.9 °C |
ANS: D
20.
What is the minimum mass of ice at 0.0 °C that must be added to
1.00 kg of water to cool the water from 28.0 °C to 12.0 °C? (Heat of fusion =
333 J/g; specific heat capacities: ice = 2.06 J/g×K, liquid water = 4.184
J/g×K)
|
a. |
175 g |
|
b. |
201 g |
|
c. |
244 g |
|
d. |
299 g |
|
e. |
1140 g |
ANS: A
21.
The heat of vaporization of benzene, C6H6, is
30.7 kJ/mol at its boiling point of 80.1 °C. How much energy in the form of
heat is required to vaporize 102 g benzene at its boiling point?
|
a. |
0.302 kJ |
|
b. |
23.6 kJ |
|
c. |
24.2 kJ |
|
d. |
40.1 kJ |
|
e. |
3.14 ´ 103 kJ |
ANS: D
22.
One statement of the first law of thermodynamics is that
|
a. |
the amount of work done on a system is
dependent of the pathway. |
|
b. |
the total work done on a system must
equal the heat absorbed by the system. |
|
c. |
the total work done on a system is
equal in magnitude, but opposite in sign of the heat absorbed by the system. |
|
d. |
the total energy change for a system is
equal to the sum of the heat transferred to or from the system and the work
done by or on the system. |
|
e. |
in any chemical process the heat flow
must equal the change in enthalpy. |
ANS: D
23.
Which of the following statements is/are CORRECT?
|
|
1. |
If a reaction occurs at constant
pressure, q =
DH. |
|
|
2. |
The change in energy for a system is
defined as the sum of the energies transferred as heat and work (i.e., DU = q + w). |
|
|
3. |
If a reaction occurs at constant
volume, q = w |
|
a. |
1 only |
|
b. |
2 only |
|
c. |
3 only |
|
d. |
1 and 2 |
|
e. |
1, 2, and 3 |
ANS: D
24.
Which of the following thermodynamic quantities are state
functions: heat (q),
work (w),
enthalpy change (DH),
and/or internal energy change (DU)?
|
a. |
q only |
|
b. |
w only |
|
c. |
DH only |
|
d. |
DU only |
|
e. |
DH and
DU |
ANS: E
25.
The thermochemical equation for the combustion of methanol is
shown below.
|
|
CH3OH() + 3/2 O2(g) ® CO2(g) + 2 H 2O(g) |
DrH° = –638.7 kJ/mol-rxn |
What is the enthalpy change for the combustion of 8.59 g CH3OH?
|
a. |
–171 kJ |
|
b. |
–19.9 kJ |
|
c. |
–2.38 ´ 103 kJ |
|
d. |
–5.49 ´ 103 kJ |
|
e. |
–1.76 ´ 106 kJ |
ANS: A
26.
The thermochemical equation for the combustion of butane is
shown below.
|
|
C4H10(g) + 13/2 O2(g) ® 4 CO2(g) + 5 H2O() |
DrH° = –2877 kJ/mol-rxn |
What is the enthalpy change for the following reaction?
8 CO2(g) + 10 H2O() ® 2 C4H10(g) +
13 O2(g)
|
a. |
+1439 kJ/mol-rxn |
|
b. |
+2877 kJ/mol-rxn |
|
c. |
–5754 kJ/mol-rxn |
|
d. |
–2877 kJ/mol-rxn |
|
e. |
+5754 kJ/mol-rxn |
ANS: E
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