TEST 4, VERSION A
CHEM 1110.24492
Spring 2016, Dr. Potts
Put your NAME, TEST VERSION, and ALL YOUR ANSWERS on the SCANTRON and submit the scantron
for grading. Do not wait until the end of the test to transfer your answers.
IA
VIIIA
1
1
2
H
1.008
3
2
3
IIA
IIIA
4
IVA
VA
VIA
VIIA
He
4.00
Be
9.01
6
7
8
9
10
B
C
N
O
F
Ne
10.81 12.01 14.01 16.00 19.00 20.18
11
12
Na
Mg
22.99 24.31
13
14
15
16
17
18
Al
Si
P
S
Cl
Ar
26.98 28.09 30.97 32.06 35.45 39.95
Li
6.94
5
IIIB
IVB
VB
VIB
VIIB
VIIIB
IB
IIB
4
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
K
Ca
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
39.10 40.08 44.96 47.90 50.94 52.00 54.94 55.85 58.93 58.71 63.55 65.37 69.72 72.59 74.92 78.96 79.90 83.80
5
37
38
39
40
41
42
43
44
45
46
47
48
49
50
51
52
53
54
Rb
Sr
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
85.47 87.62 88.91 91.22 92.91 95.94 [98] 101.1 102.9 106.4 107.9 112.40 114.8 118.7 121.8 127.60 126.90 131.30
6
55
56
71
72
73
74
75
76
77
78
79
80
81
82
83
84
85
86
Cs
Ba
Lu
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn
132.9 137.3 175 178.5 181 183.9 186.2 190.2 192.2 195.1 197 200.59 204.4 207.2 209 [209] [210] [222]
7
87
88
103
104
105
106
107
108
109
110
111
112
113
114
115
116
Fr
Ra
Lr
Rf
Db
Sg
Bh
Hs
Mt
Ds
Rg
Uub
Uut Uuq Uup Uuh
[223] [226] [262] [267] [268] [271] [272] [270] [276] [281] [280] [285] [284] [289] [288] [293]
57
58
59
60
61
62
63
64
65
66
67
68
69
70
La
Ce
Pr
Nd
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
138.9 140.1 140.9 144.2 [145] 150.4 152 157.3 158.9 162.5 164.93 167.3 168.9 173
89
90
91
92
93
94
95
96
97
98
99
100
101
102
Ac
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
[227] 232 [231] 238 [237] [244] [243] [247] [247] [251] [252] [257] [258] [259]
Test 4, Version A, Page 1
118
Uuo
[294]
Part I (60pts). 15 multiple-choice questions worth 4 points each. Choose the best answer from the options given,
and record your final answer on your scantron.
1.
What is the process in which molecules undergo a phase change directly from the solid phase to the gas
phase?
A. sublimation
B. deposition
C. freezing
D. condensation
E. melting
2.
Which of the following is a weak acid?
A. HF
B. HBr
C. HCl
D. HNO3
E.
H2SO4
3.
Which is the net ionic equation for the reaction between aqueous solutions of LiOH and HBr?
A. Li+(aq) + OH–(aq)+ H+(aq) + Br–(aq)  H2O(l) + LiBr(aq)
B. H+(aq) + OH–(aq)  H2O(l)
C. LiOH(aq)  Li+(aq) + OH–(aq)
D. HBr(aq)  H+(aq) + Br–(aq)
E. Li+(aq) + Br–(aq)  LiBr(aq)
4.
If aqueous solutions of ammonium sulfide and copper(II) nitrate are mixed, which insoluble precipitate is
formed?
A. Cu2S
B. NH4NO3
C. CuSO4
D. CuS
E. NH4(NO3)2
5.
If aqueous solutions of Na2CO3 and BaCl2 are mixed, which insoluble precipitate is formed?
A. Ba2CO3
B. BaCO3
C. NaCl2
D. BaO
E. NaCl
6.
Based on the solubility rules, which of these processes will occur if solutions of CuSO 4(aq) and BaCl2(aq)
are mixed?
A. No precipitate will form.
B. CuCl2 will precipitate; Ba2+ and SO42– are spectator ions.
C. CuSO4 will precipitate; Ba2+ and Cl– are spectator ions.
D. BaCl2 will precipitate; Cu2+ and SO42– are spectator ions.
E. BaSO4 will precipitate; Cu2+ and Cl– are spectator ions.
7.
Based on the solubility rules, which one of these compounds is soluble in water?
A. Ag2S
B. Na2S
C. Ag2CO3
D. Hg2Cl2
E.
BaCO3
8.
The location that indicates conditions under which two phases can exist in equilibrium is called the
A. transition state. B. phase diagram. C. phase boundary. D. critical point. E. triple point.
9.
What is the net ionic equation if sodium sulfate is mixed with barium hydroxide?
A. Ba2+(aq) + SO42– (aq)  BaSO4(s)
B. 2Ba+(aq) + SO42– (aq)  Ba2SO4(s)
C. Na+(aq) + OH–(aq)  NaOH(s)
D. Ba2+(aq) + 2OH–(aq)  Ba(OH)2(s)
E. 2Na+(aq) + SO42–(aq)  Na2SO4(s)
10.
Which of the following gases effuses most rapidly?
A. N2
B. O2
C. HCl
11.
D. NH3
E.
CO
What name is given to the phenomenon where a thin film of water contracts and adheres to the wall of a
glass cylinder?
A. Cohesion B. Polarity
C. Surface tension
D. Capillary action
E. Adhesion
Test 4, Version A, Page 2
12.
Based on the solubility rules, which one of these compounds is insoluble in water?
A. AgBr
B. NaCl
C. ZnCl2
D. MgBr2
E.
13.
The distinguishing characteristic of all electrolyte solutions is that they
A. contain molecules.
D. conduct heat.
B. react with other solutions.
E. always contain acids.
C. conduct electricity.
14.
Based on the solubility rules, which one of these compounds is soluble in water?
A. PbSO4
B. CaSO4
C. K2SO4
D. BaSO4
15.
E.
FeCl2
Ag2SO4
Which chemical equation describes an acid–base neutralization reaction?
A. LiOH(aq) + HNO3(aq)  LiNO3(aq) + H2O(l)
B. 2Al(s)+ 3H2SO4(aq)  Al2 (SO4)3 (aq) + 3H2(g)
C. 2KBr(aq) + Cl2(g)  2KCl(aq) + Br2(l)
D. 2SO2(g) + 2H2O(l) + O2(g)  2H2SO4(aq)
E. CaBr2(aq) + H2SO4(aq)  CaSO4(s) + 2HBr(g)
Part 2 (40pts). Calculations: Clearly (and legibly) show all work on the blank space on the scantron answer sheet
for full credit. Do not wait until the end of the test to transfer your answers.
1. (10 pts) A sample of gas has an initial volume of 5.65 L at a pressure of 735 mmHg. If the volume of the
gas is increased of 9.45 L, what is its new pressure in mmHg?
2. (10 pts) A chemist wants to make 5.50 L of a 0.300 M CaCl2 solution? What mass in grams should the
chemist use? (MM of CaCl2 = 110.98 g/mol)
3. (10 pts) Methanol gas can be synthesized by the reaction below. What volume of methanol gas is produced
if 2.5L of CO is reacted with 3.5 L of H2 at constant pressure and temperature?
CO (g) + 2 H2 (g)  CH3OH (g)
4. (10 pts) Oxygen gas reacts with powdered aluminum to make aluminum oxide according to the balanced
reaction below. What mass of aluminum oxide is produced if 2.75 L of O2 at 1.00 atm and 298K is
reacted with excess aluminum? (MM of Al2O3 = 101.96 g/mol)
4 Al (s) + 3 O2 (g)  2 Al2O3 (s)
Test 4, Version A, Page 3