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1021_2nd Exam_1021113
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
1) Identify LiBr.
A) strong acid
B) nonelectrolyte
C) weak acid
D) weak electrolyte
E) strong electrolyte
2) Balance the chemical equation given below, and determine the number of milliliters of 0.00300 M phosphoric
acid required to neutralize 45.00 mL of 0.00150 M calcium hydroxide.
_____ Ca(OH)2 (aq) + _____ H3 PO4 (aq) → _____ Ca3 (PO4 )2 (aq) + _____ H2 O(l)
A) 22.5 mL
B) 15.0 mL
C) 3.04 mL
D) 33.8 mL
3) Which of the following signs on q and w represent a system that is doing work on the surroundings, as well as
gaining heat from the surroundings?
A) q = -, w = +
B) q = +, w = +
C) q = +, w = D) q = -, w = E) None of these represent the system referenced above.
4) What is the oxidation number of the chromium atom in K2 CrO4 ?
B) -2
C) +7
A) +2
D) +6
5) The volume of a gas is inversely proportional to the pressure of a gas is known as
A) Ideal Gas Law
B) Avogadroʹs Law
C) Daltonʹs Law
D) Boyleʹs Law
E) Charlesʹs Law
6) Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of lithium sulfide
and copper (II) nitrate are mixed.
A) 2 Li+ (aq) + S2- (aq) + Cu2+(aq) + 2 NO3 - (aq) → CuS(s) + 2 Li+ (aq) + 2 NO3 - (aq)
B) Li+ (aq) + S- (aq) + Cu+ (aq) + NO3 - (aq) → CuS(s) + LiNO3 (aq)
C) Li+ (aq) + SO4 2- (aq) + Cu+ (aq) + NO3 - (aq) → CuS(s) + Li+ (aq) + NO3 -(aq)
D) 2 Li+ (aq) + S2- (aq) + Cu2+ (aq) + 2 NO3 - (aq) → Cu2+ (aq) + S2- (aq) + 2 LiNO3 (s)
E) No reaction occurs.
1021113_A­1
7) Identify the spectator ions in the following molecular equation.
LiCl(aq) + AgNO 3 (aq) → AgCl(s) + LiNO3 (aq)
A) Ag+ and NO3 B) Li+ and ClC) Ag+ and ClD) Li+ and NO3 E) There are no spectator ions in this reaction.
8) What is the volume of 9.783 x 1023 atoms of Kr at 9.25 atm and 512K?
A) 1.85 L
B) 7.38 L
C) 15.4 L
D) 3.69 L
E) 30.8 L
9) A balloon contains 0.76 mol N2 , 0.18 mol O2 , 0.031 mol He and 0.026 mol H2 at 749 mm Hg. What is the partial
pressure of O2 ?
A) 23 mm Hg
B) 570 mm Hg
C) 140 mm Hg
D) 20 mm Hg
10) Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction:
2H2 O2 (l) → 2H2 O(l) + O2 (g)
ΔH = -196 kJ
Calculate the value of q (kJ) in this exothermic reaction when 4.00 g of hydrogen peroxide decomposes at
constant pressure?
A) -2.31 × 104 kJ
B) -23.1 kJ
C) -0.0217 kJ
D) -11.5 kJ
E) 1.44 kJ
11) When 0.455 g of anthracene, C14H10, is combusted in a bomb calorimeter that has a water jacket containing
500.0 g of water, the temperature of the water increases by 8.63°C. Assuming that the specific heat of water is
4.18 J/(g · °C), and that the heat absorption by the calorimeter is negligible, estimate the enthalpy of combustion
per mole of anthracene.
B) -8120 kJ/mol
C) -7060 kJ/mol
D) -39.7 kJ/mol
A) +39.7 kJ/mol
12) Using the following equation for the combustion of octane, calculate the amount of moles of carbon dioxide
formed from 100.0 g of octane. The molar mass of octane is 114.33 g/mole. The molar mass of carbon dioxide is
44.0095 g/mole.
2 C8 H18 + 25 O 2 → 16 CO2 + 18 H2 O
A) 8.000 moles
B) 18.18 moles
13) Convert 1.50 atm to torr.
B) 1000 torr
A) 1520 torr
ΔH°rxn = -11018 kJ
C) 6.997 moles
D) 10.93 moles
E) 14.00 moles
C) 760 torr
D) 1140 torr
E) 875 torr
1021113_A­2
14) An instrument used to atmospheric pressure is called a
A) barometer
B) spectrometer
C) spectrophotometer
D) manometer
E) sphygmomanometer
15) A 6.55 g sample of aniline (C6 H5 NH2 , molar mass = 93.13 g/mol) was combusted in a bomb calorimeter. If the
temperature rose by 32.9°C, use the information below to determine the heat capacity of the calorimeter.
4 C6 H5 NH2 (l) + 35 O2 (g) → 24 CO2 (g) + 14 H2 O(g) + 4 NO2 (g)
ΔH°rxn = -1.28 x 104 kJ
A) 12.8 kJ/°C
B) 6.84 kJ/°C
C) 97.3 kJ/°C
D) 38.9 kJ/°C
E) 5.94 kJ/°C
16) Two solutions, initially at 24.69°C, are mixed in a coffee cup calorimeter (Ccal = 105.5 J/°C). When a 200.0 mL
volume of 0.100 M AgNO3 solution is mixed with a 100.0 mL sample of 0.100 M NaCl solution, the temperature
in the calorimeter rises to 25.16°C. Determine the 'H°rxn, in units of kJ/mol AgCl. Assume that the density and
heat capacity of the solutions is the same as that of water. Hint: Write a balanced reaction for the process.
A) -25 kJ/mol AgCl
B) -59 kJ/mol AgCl
C) -32 kJ/mol AgCl
D) -78 kJ/mol AgCl
E) -64 kJ/mol AgCl
17) Which of the following solutions will have the highest concentration of chloride ions?
A) 0.40 M MgCl2
B) 0.60 M AlCl3
C) 0.40 M CaCl2
D) 0.20 M LiCl
E) All of these solutions have the same concentration of chloride ions.
18) A mixture of 10.0 g of Ne and 10.0 g Ar have a total pressure of 1.6 atm. What is the partial pressure of Ne?
B) 0.54 atm
C) 0.40 atm
D) 1.3 atm
E) 0.80 atm
A) 1.1 atm
19) A syringe contains 589 mL of CO at 325 K and 1.2 atm pressure. A second syringe contains 473 mL of N 2 at 298
K and 2.6 atm. What is the final pressure if the contents of these two syringes are injected into a 1.00 L container
at STP?
A) 1.1 atm
B) 1.9 atm
C) 3.8 atm
D) 0.59 atm
E) 1.7 atm
20) Which of the following is TRUE if ΔE sys = - 115 J?
A) The system is losing 115 J, while the surroundings are gaining 115 J.
B) The system is gaining 115 J, while the surroundings are losing 115 J.
C) Both the system and the surroundings are losing 115 J.
D) Both the system and the surroundings are gaining 115 J.
E) None of the above are true.
1021113_A­3
21) Using the following equation for the combustion of octane, calculate the heat of reaction for 400.0 g of octane.
The molar mass of octane is 114.33 g/mole.
ΔH°rxn = -11018 kJ
2 C8 H18 + 25 O2 → 16 CO2 + 18 H2 O
A) 19.28 kJ
B) 19280 kJ
C) 38560 kJ
D) 50400 kJ
C) 11.1 g/L
D) 0.0823 g/L
22) Identify what a coffee cup calorimeter measures.
A) measures ΔE for oxidation reactions
B) measures ΔT for combustion solutions
C) measures ΔH for reduction solutions
D) measures ΔE for hydrolysis reactions
E) measures ΔH for aqueous solutions
23) What is the density of hydrogen gas at STP?
A) 0.0450 g/L
B) 0.0899 g/L
24) A 55.0-L steel tank at 20.0°C contains acetylene gas, C2 H2 , at a pressure of 1.39 atm. Assuming ideal behavior,
how many grams of acetylene are in the tank?
B) 1210 g
C) 82.9 g
D) 8.20 g
A) 3.17 g
25) Determine the reducing agent in the following reaction.
2 Li(s) + Fe(C2 H3 O2 )2 (aq) → 2 LiC2 H3 O2 (aq) + Fe(s)
A) Li
B) H
C) C
26) Determine the oxidation state of nitrogen in NO.
B) +4
A) 0
C) +5
D) Fe
E) O
D) +2
E) +3
27) Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction:
P4 (g) + 10 Cl2 (g) → 4PCl 5 (s)
ΔH°rxn = ?
PCl5 (s) → PCl3 (g) + Cl2 (g)
P4 (g) + 6 Cl 2 (g) → 4 PCl3 (g)
ΔH°rxn = +157 kJ
Given:
A) -1364 kJ
B) -1786 kJ
ΔH°rxn = -1207 kJ
C) -1835 kJ
D) -2100. kJ
E) -1050. kJ
28) How many grams of H2 gas can be produced by the reaction of 54.0 grams of Al(s) with an excess of dilute
hydrochloric acid in the reaction shown below?
2 Al(s) + 6 HCl(aq) → 2 AlCl3 (aq) + 3 H2 (g)
A) 2.68 g
B) 12.1 g
C) 4.04 g
1021113_A­4
D) 6.05 g
29) Which substance is the limiting reactant when 2.0 g of sulfur reacts with 3.0 g of oxygen and 4.0 g of sodium
hydroxide according to the following chemical equation :
2 S(s) + 3 O2 (g) + 4 NaOH(aq) → 2 Na2 SO4 (aq) + 2 H2 O(l)
A) S(s)
B) NaOH(aq)
C) O2 (g)
D) None of these substances is the limiting reactant.
30) What reagent could be used to separate Br- from CH3 CO2 - when added to an aqueous solution containing
both?
A) Ba(OH)2(aq)
B) AgNO3(aq)
C) CuSO4(aq)
D) NaI(aq)
31) Calculate the temperature, in K, of 2.20 moles of gas occupying 3.30 L at 3.50 atm.
A) 28.0 K
B) -209 K
C) 337 K
D) 64.0 K
32) If NO and NH3 are allowed to effuse through a porous membrane under identical conditions, the rate of
effusion for NH3 will be ________ times that of NO .
A) 0.75
B) 0.57
C) 1.3
D) 1.8
33) A 0.465 g sample of an unknown compound occupies 245 mL at 298 K and 1.22 atm. What is the molar mass of
the unknown compound?
A) 12.2 g/mol
B) 81.8 g/mol
C) 33.9 g/mol
D) 26.3 g/mol
E) 38.0 g/mol
34) Determine the theoretical yield of H2 S (in moles) if 64 mol Al 2 S3 and 64 mol H 2 O are reacted according to the
following balanced reaction. A possibly useful molar mass is Al2 S3 = 150.17 g/mol.
Al2 S3 (s) + 6 H 2 O(l) → 2 Al(OH)3 (s) + 3 H 2 S(g)
A) 64 mol H 2 S
B) 32 mol H 2 S
C) 128 mol H 2 S
D) 192 mol H 2 S
E) 96 mol H 2 S
35) Which of the following processes is exothermic?
A) a candle flame
B) the vaporization of water
C) the chemical reaction in a "cold pack" often used to treat injuries
D) baking bread
E) None of the above are exothermic.
36) A 21.8 g sample of ethanol (C2 H5 OH) is burned in a bomb calorimeter, according to the following reaction. If
the temperature rises from 25.0 to 62.3°C, determine the heat capacity of the calorimeter. The molar mass of
ethanol is 46.07 g/mol.
C2 H5 OH(l) + 3 O2 (g) → 2 CO2 (g) + 3 H2 O(g)
A) 15.7 kJ/°C
B) 63.7 kJ/°C
C) 4.99 kJ/°C
1021113_A­5
ΔH°rxn = -1235 kJ
D) 5.65 kJ/°C
E) 33.1 kJ/°C
37) When 5.00 mol of benzene is vaporized at a constant pressure of 1.00 atm and at its normal boiling point of
80.1°C, 169.5 kJ are absorbed and PΔV for the vaporization process is equal to 14.5 kJ then
A) ΔE = 169.5 kJ and ΔH = 184.0 kJ.
B) ΔE = 184.0 kJ and ΔH = 169.5 kJ.
C) ΔE = 169.5 kJ and ΔH = 155.0 kJ.
D) ΔE = 155.0 kJ and ΔH = 169.5 kJ.
38) A 12.8 g sample of ethanol (C2 H5 OH) is burned in a bomb calorimeter with a heat capacity of 5.65 kJ/°C. Using
the information below, determine the final temperature of the calorimeter if the initial temperature is 25.0°C.
The molar mass of ethanol is 46.07 g/mol.
C2 H5 OH(l) + 3 O2 (g) → 2 CO2 (g) + 3 H2 O(g)
A) 60.7°C
B) 28.1°C
C) 111°C
ΔH°rxn = -1235 kJ
D) 85.7°C
E) 74.2°C
39) A piece of iron (mass = 25.0 g) at 398 K is placed in a styrofoam coffee cup containing 25.0 mL of water at 298 K.
Assuming that no heat is lost to the cup or the surroundings, what will the final temperature of the water be?
The specific heat capacity of iron = 0.449 J/g°C and water = 4.18 J/g°C.
A) 388 K
B) 325 K
C) 308 K
D) 348 K
E) 287 K
40) Pure acetic acid (HC2 H3 O2 ) is a liquid and is known as glacial acetic acid. Calculate the molarity of a solution
prepared by dissolving 10.00 mL of glacial acetic acid at 25°C in sufficient water to give 500.0 mL of solution.
The density of glacial acetic acid at 25°C is 1.05 g/mL.
A) 3.50 × 10-4 M
B) 0.350 M
C) 21.0 M
D) 0.0210 M
E) 1.26 × 103 M
1021113_A­6
The Periodic Table of the Elements
1
2
H
He
Hydrogen
Helium
1.00794
4.003
3
5
4
6
7
8
9
10
Li
Be
B
C
N
O
F
Ne
Lithium
Beryllium
Boron
Carbon
Nitrogen
Oxygen
Fluorine
Neon
6.941
9.012182
10.811
12.0107
14.00674
11
12
13
14
15
15.9994 18.9984032 20.1797
16
17
18
Ar
Na
Mg
Al
Si
P
S
Cl
Sodium
Magnesium
Aluminum
Silicon
Phosphorus
Sulfur
Chlorine
Argon
22.989770
24.3050
26.981538
28.0855
30.973761
32.066
35.4527
39.948
19
20
31
32
33
34
35
36
21
22
23
24
25
26
27
28
29
30
K
Ca
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
Potassium
Calcium
Scandium
Titanium
Vanadium
Chromium
Manganese
Iron
Cobalt
Nickel
Copper
Zinc
Gallium
Germanium
Arsenic
Selenium
Bromine
Krypton
39.0983
40.078
44.955910
47.867
50.9415
51.9961
54.938049
55.845
58.933200
58.6934
63.546
65.39
69.723
72.61
74.92160
78.96
79.904
83.80
37
38
39
40
41
42
43
44
45
46
47
48
49
50
51
52
53
54
Xe
Rb
Sr
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Rubidium
Strontium
Yttrium
Zirconium
Niobium
Molybdenum
Technetium
Ruthenium
Rhodium
Palladium
Silver
Cadmium
Indium
Tin
Antimony
Tellurium
Iodine
Xenon
85.4678
87.62
88.90585
91.224
92.90638
95.94
(98)
101.07
102.90550
106.42
107.8682
112.411
114.818
118.710
121.760
127.60
126.90447
131.29
55
56
57
72
73
74
75
76
77
78
79
80
81
82
83
84
85
86
Rn
Cs
Ba
La
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Cesium
Barium
Lanthanum
Hafnium
Tantalum
Tungsten
Rhenium
Osmium
Iridium
Platinum
Gold
Mercury
Thallium
Lead
Bismuth
Polonium
Astatine
Radon
132.90545
137.327
138.9055
178.49
180.9479
183.84
186.207
190.23
192.217
195.078
196.96655
200.59
204.3833
207.2
208.98038
(209)
(210)
(222)
87
88
89
104
105
106
107
108
109
110
111
112
113
114
66
67
68
69
70
71
Fr
Ra
Ac
Rf
Db
Sg
Bh
Hs
Mt
Francium
Radium
Actinium
Rutherfordium
Dubnium
Seaborgium
Bohrium
Hassium
Meitnerium
(223)
(226)
(227)
(261)
(262)
(263)
(262)
(265)
(266)
(269)
(272)
(277)
58
59
60
61
62
63
64
65
Ce
Pr
Nd
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
Cerium
Praseodymium
Neodymium
Promethium
Samarium
Europium
Gadolinium
Terbium
Dysprosium
Holmium
Erbium
Thulium
Ytterbium
Lutetium
140.116
140.90765
144.24
(145)
150.36
151.964
157.25
158.92534
162.50
164.93032
167.26
168.93421
173.04
174.967
90
91
92
93
94
95
96
97
98
99
100
101
102
103
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
Lr
Thorium
Protactinium
Uranium
Neptunium
Plutonium
Americium
Curium
Berkelium
Californium
Einsteinium
Fermium
Mendelevium
Nobelium
Lawrencium
(237)
(244)
(243)
(247)
(247)
(251)
(252)
(257)
(258)
(259)
(262)
232.0381 231.03588 238.0289
1995 IUPAC masses and Approved Names from http://www.chem.qmw.ac.uk/iupac/AtWt/
masses for 107-111 from C&EN, March 13, 1995, p. 35
112 from http://www.gsi.de/z112e.html