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Exam #2 - A
Chemistry 130
Name:
November 2, 2011
Lab Day and Time:
Instructions
1. Do not open the exam until you are told to start.
2. This exam is closed note and closed book. You are not allowed to use any outside material
while taking this exam.
3. Use the spaces provided to write down your answers. To receive full credit, you must
show all work. Do not write answers on any other pieces of paper. If you need more room,
write on the back of the exam and be sure to include a note describing where the work is
located.
4. When solving numerical problems, make sure you include the proper units in your final
answer as well as the proper number of significant digits.
5. If a question asks for a response in sentence or paragraph form, make sure you respond in
that format.
6. Useful data for the exam and a periodic table are provided on the last page of the exam.
Carefully tear out these sheets if you wish.
Page #
Points possible
2-5
48
6
21
7
14
8
14
Attendance
3
In-Class EC
3
Total
100
1
Points awarded
Exam #2 - A
Chemistry 130
November 2, 2011
Multiple Choice
Unless otherwise directed, choose the single best answer for each question. When balancing
chemical equations, use the smallest whole number coefficients.
1. Which of the following is the correct name for V(NO2)2?
a.
b.
c.
d.
e.
vanadium nitrate
vanadium nitrite
vanadium(II) nitride
vanadium(II) nitrate
None of the above.
2. Which of the following is/are ionic compounds?
I.) CF4
II.) NaCl
III.) NH4IO
a.
b.
c.
d.
e.
IV.)
V.)
NH3
AlN
II, V
I, II, IV
II, III, V
II, III, IV, V
All are examples of ionic compounds.
3. Use the unbalanced chemical equation shown below to answer the following question. If one
molecule of O2 reacts, how many molecules of SO2 will react?
SO2(g) + O2(g) Æ SO3(g)
a.
b.
c.
d.
e.
1 molecule of SO2
2 molecules of SO2
3 molecules of SO2
4 molecules of SO2
None of the above.
4. When Ba(BrO3)2(aq) is mixed with Li3PO4(aq) a reaction occurs. What is the sum of all the
coefficients for the balanced chemical equation for this reaction? Hint: If the balanced
chemical equation was 2A + B Æ 3C, the sum of the coefficients would be 6.
a.
b.
c.
d.
e.
12
10
7
4
None of the above.
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Exam #2 - A
Chemistry 130
November 2, 2011
5. When the following chemical equation is balanced, what is the coefficient in front of the H2O?
CO(g) + H2O(g) Æ O2(g) + C4H10(g)
a.
b.
c.
d.
e.
4
5
7
10
None of the above.
6. What is the oxidation state/number of chromium in K2Cr2O7?
a.
b.
c.
d.
e.
+2
+3
+5
+6
None of the above.
7. When C5H12O(l) is combusted, what is the sum of all of the coefficients in the balanced
chemical equation? Hint: If the balanced chemical equation was 2A + B Æ 3C, the sum of the
coefficients would be 6.
a.
b.
c.
d.
e.
38
13
27
39
None of the above.
8. When H3PO3(aq) is mixed with KOH(aq) a reaction occurs. What is the sum of all the
coefficients for the balanced chemical equation for this reaction? Hint: If the balanced
chemical equation was 2A + B Æ 3C, the sum of the coefficients would be 6.
a.
b.
c.
d.
e.
4
6
8
10
None of the above.
9. Which of the following is the correct name for P2O5?
a. diphosphorus pentoxide
b. potassium oxide
c. potassium(V) oxide
d.
e.
phosphorus oxide
None of the above.
3
Exam #2 - A
Chemistry 130
November 2, 2011
10. How many silver atoms are contained in a 6.00 g sample of Ag?
a.
b.
c.
d.
e.
3.35x1022 atoms
3.90x1024 atoms
0.0556 atoms
3.61x1024 atoms
None of the above.
11. Which of the following would you expect to be strong electrolytes when placed in deionized
water?
I.) LiF
II.) H2SO4
III.) BeS
a.
b.
c.
d.
e.
IV.)
V.)
HCN
Ca(OH)2
I, II, III, IV, V
II, III, IV, V
I, II, IV, V
I, IV, V
I, II, V
12. A sample of 2.00 moles of Na2SO4 contains how many moles of oxygen?
a.
b.
c.
d.
e.
1.00 moles
2.00 moles
4.00 moles
8.00 moles
None of the above.
13. How many moles of NO2 are there in a 22.06 g sample of NO2?
a.
b.
c.
d.
e.
0.4795 moles NO2
0.7352 moles NO2
1.328x1025 moles NO2
2.888x1023 moles NO2
None of the above.
4
Chemistry 130
Exam #2 - A
November 2, 2011
14. When N2 gas reacts with H2 gas, NH3 gas is formed. What is the sum of all the coefficients for
the balanced chemical equation for this reaction? Hint: If the balanced chemical equation was
2A + B Æ 3C, the sum of the coefficients would be 6.
a.
b.
c.
d.
e.
3
4
5
6
7
15. When a sample of manganese metal is heated in a fluorine gas atmosphere, the mass of
manganese fluoride produced is 7.218|3 g. If the manganese fluoride compound contains
4.573|3 g of atomic fluorine, calculate the empirical formula of the compound.
a.
b.
c.
d.
e.
MnF5
MnF4
MnF3
MnF2
None of the above.
16. When Pb(NO3)2(aq) reacts with KI(aq), which ions are the spectator ions?
a.
b.
c.
d.
e.
Pb2+(aq) and I-(aq)
K+(aq) and NO3-(aq)
NO3-(aq) and I-(aq)
There are no spectator ions.
They are all spectator ions because there is no reaction.
5
Exam #2 - A
Chemistry 130
November 2, 2011
17. In the table below, the name or formula for a chemical compound is given. Fill in the table
with the corresponding name or formula of the chemical compound. (16 points)
NAME
FORMULA
lithium oxalate
BrF5
HCl
ammonium acetate
HIO2
CoN
silver thiosulfate
barium hypochlorite
18. What are the complete, total ionic, and net ionic equations for the reaction that occurs when an
aqueous solution of HClO4 reacts with an aqueous solution of Ba(OH)2? Assume the reaction
takes place in a beaker of deionized water. (5 points)
Complete
Total Ionic
Net-Ionic
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Chemistry 130
Exam #2 - A
November 2, 2011
19. In the space below, write the balanced chemical equation for the reaction of NH3(aq) with H2SO4(aq)?
(2 points)
20. A sample of H3PO4 is placed in a beaker of deionized water. In the diagram below, show what
will exist in the water if two H3PO4 particles are placed in the beaker. (3 points)
Beaker Full of Deionized Water
21. In a reaction, phosphorus starts with an oxidation state of -3. During the reaction, 5 electrons
are transferred and phosphorus is oxidized. Use this information to complete the equation
below. Show what the P3- is converted into and put the transferred electrons on the correct side
of the equation. (4 points)
P3-
Æ
22. What are the complete, total ionic, and net ionic equations for the reaction that occurs when an
aqueous solution of Al2(SO4)3 reacts with an aqueous solution of Cs2S? Assume the reaction
takes place in a beaker of deionized water. (5 points)
Complete
Total Ionic
Net-Ionic
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Exam #2 - A
Chemistry 130
November 2, 2011
23. What is the molar mass of PtMnO4? (4 points)
24. A sample of H5IO6 contains 9.25 grams of H. How many molecules of H5IO6 are contained in
the sample? (4 points)
25. Use the balanced oxidation reduction reaction below to answer the following question.
(6 points)
6HBr(aq) + 2In(s) Æ 2InBr3(aq) + 3H2(g)
a. Which element is oxidized?
_________
b. Which element is reduced?
__________
c. Which element is the reducing agent?
__________
d. Which element is the oxidizing agent?
__________
e. How many electrons are transferred?
__________
a. Which element are the electrons transferred to?
__________
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Chemistry 130
Exam #2 - A
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November 2, 2011
Chemistry 130
Exam #2 - A
10
November 2, 2011
Exam #2 - A
Chemistry 130
November 2, 2011
Conversion Factors, Constants, and Periodic Table
Avogadro’s Number:
Mass of Proton:
6.022 x 1023 particles/mole
1.0073 amu
Mass of Neutron:
1.0087 amu
Mass of Electron:
-4
Mass of 1 amu:
Temperature conversion:
5.486 x 10 amu
1.66 x 10-24 g
Solubility Rules
SOLUBLE COMPOUNDS
group 1 metals + any anion
Æ soluble
NH4+ + any anion
Æ soluble
Any cation + NO3-, ClO4-, C2H3O2-
Æ soluble
Mostly Soluble Compounds
Any cation + Cl-, Br-, I(except Pb2+, Ag+, Hg22+ Æ insoluble)
Æ soluble
Æ soluble
Any cation + SO42(except Sr2+, Ba2+, Pb2+, Hg22+, Ca2+ Æ insoluble)
T [K] = 273.15 + T [°C]
Insoluble Compounds
Any cation + OHÆ insoluble
(except group I, NH4+, Ca2+, Ba2+ Æ soluble)
Æ Insoluble
Any cation + S2(except group I, NH4+, group II Æ soluble)
Æ Insoluble
Any cation + CO32-, PO43(except group I, NH4+ Æ soluble)
1
2
H
He
1.0079
4.0026
3
4
5
6
7
8
9
10
Li
Be
B
C
N
O
F
Ne
6.941
9.0122
10.811
12.011
14.0067
15.9994
18.9984
20.1797
11
12
13
14
15
16
17
18
Na
Mg
Al
Si
P
S
Cl
Ar
22.9898
24.3050
26.9815
28.0855
30.9738
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
39.0983
40.078
44.9559
47.88
50.9415
51.9961
54.9380
55.847
58.9332
58.693
63.546
65.409
69.723
72.61
74.9216
78.96
79.904
83.80
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
85.4678
87.62
88.9059
91.224
92.9064
95.94
(98)
101.07
102.906
106.42
107.868
112.411
114.82
118.710
121.757
127.60
126.904
131.29
55
56
57
72
73
74
75
76
77
78
79
80
81
82
83
84
85
86
Cs
Ba
La
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn
132.905
137.327
138.906
178.49
108.948
183.85
186.207
190.2
192.22
195.08
196.967
200.59
204.383
207.2
208.980
(209)
(210)
87
88
89
104
105
106
107
108
109
110
111
112
Fr
Ra
Ac
Rf
Db
Sg
Bh
Hs
Mt
(223)
226.025
227.028
(261)
(262)
(263)
(262)
(265)
(266)
114
116
Uun Uuu Uub
(269)
(272)
(277)
58
59
60
61
62
63
64
65
66
67
68
69
70
71
Ce
Pr
Nd
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
140.12
140.908
144.24
(145)
150.36
151.96
157.25
158.925
162.50
164.930
167.26
168.934
173.04
174.967
90
91
92
93
94
95
96
97
98
99
100
101
102
103
Th
Pa
U
Np
Pu
Bk
Cf
Es
Fm
Md
No
Lr
232.038
231.036
238.029
(237)
(244)
(247)
(251)
(252)
(257)
(258)
(259)
(260)
Am Cm
(243)
(247)
11
(222)
118