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Exam 3 Special Code 111111 Name:
__________________,________________ Petrovich, Fall 2010 print last
print first
Student Number: ___________________(000######)
1. To what temperature must a substance be heated to contain 10
kJ/mol of thermal energy?
A) 1203 K B) 930 K C) 122 K D) -151 K
2. What is the concentration of Ne in a container at 40 C and
3.2 atmospheres of pressure?
A) 0.974 mol/L B) 0.124 mol/L C) 0.00123 mol/L D) 0.0096
mol/L
E) cannot be answered without volume.
3. A balloon is filled with 2.00 liters of gas at 300 K. What is
the volume of the balloon at 100K?
A) 0.75 L B) 1.50 L C) 6.00 L D) 0.67 L
4. Choose the correct letter(A-D) to make a true statement. At
25 C, iodine (I2) is a solid and fluorine(F2) is a gas. This is
because..
A) the thermal energy of I2 is greater than the thermal energy
of F2.
B) the thermal energy of I2 is less than the thermal energy of
F2.
C) the interaction energy of I2 is greater than the interaction
energy of F2.
D) the interaction energy of I2 is less than the interaction
energy of F2.
5. The pressure of the atmosphere is 755 mm Hg. What is the
pressure in atmospheres of the Argon gas in the bulb if the height
difference is 145 mm Hg?
A) 0.803 atm
B) 900 atm
C) 1.18 atm
D) 610 atm
6. How many moles of atoms are in 51.0 grams of S8?
A) 1.64x103 mol atoms B) 7.66 x 1024 mol atoms C) 1.59 mol atoms
D) 12.7 mol atoms
7. In Phoenix, Arizona, a typical summer day is 40o C (104o F)
with 10.% humidity. What is the vapor pressure of water in the air.
The vapor pressure of water at 40o C is 55.3 mm Hg.
A) 5.5 mm Hg B) 4.0 mm Hg C) 55.3 mm Hg D) 22 mm Hg
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Exam 3
Pre
ssure
(atm
)
1.00
0.75
0.50
0.25
10 20 30 40 50 60 70 80
Temperature (C)
90
A
B
C
D EF
G
H I
J
KLP
ress
ure
(atm
)
1.00
0.75
0.50
0.25
10 20 30 40 50 60 70 80
Temperature (C)
90
A
B
C
D EF
G
H I
J
KL
C HN
H
..H
H
C
H
H
C
H
H
H C H
H
NC
H
H
C
H
H
H
H
H
C H
H
CC
H
H
C
H
H
H
H
H
H
C HN
H
..H
H
C
H
H
H
A B
..
C D
Consider the phase diagram below for kryptonite for the next two
questions. 8. Under what conditions is kryptonite a solid and gas,
but NOT a liquid?
A) 70o C, 0.75 atm
B) 20o C, 0.25 atm
C) 30o C, 1.0 atm
D) 40o C, 0.50 atm
9. What process is occurring along arrow C?
A) freezing B) evaporation C) melting D) sublimation
10. Which compound below would have the LOWEST boiling
point?
11. Which numeric combination (A-E) belongs together in the
diagrams below?
A) 1,4,5 B) 2,3,6 C) 1,4,6 D) 2,4,6 E) 2,4,5
12. Select that pair in which hydrogen bonding will NOT
occur.
A) I with I B) II with II C) I with II D) I with III E) No
correct answer
1
2 H-Cl
5
temperature
43
F-F
6
H
H
H
H
CN
C
CC
C
H
H
H
H
H
CN
C
CC
C
H H
..H
..
F
FNF..
I II III
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Exam 3
13. Choose the POLAR compounds from the choices below.
A) I & II B) III & IV C) I & III D) II & IV E)
II & III
14. The unit cell of an ionic compound is shown below. The X
atom occupies the center and edges of the unit cell. The Y atom
occupies the faces of the unit cell. Choose the correct formula for
the compound below.
A) X13Y6
B) X4Y3
C) X7Y4
D) X3Y4
15. In the band diagram shown below, which letter represents the
valence band?
16. A weak, light metal would likely pack in this type of unit
cell.
17. Choose the correct set of words to complete the statement
below. ZnS is a(n) ____i_____ substance. SO3 is a(n) ____ii_____
substance. A) i=network covalent, ii=ionic B) i=network covalent,
ii=molecular
C) i=metallic, ii=ionic D) i=ionic, ii=molecular
Energ
y
A
B
C
D
E
Energ
y C
A B C
Y
X
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Exam 3
18. E for a system is 12.0 kJ. If the system is an endothermic
reaction with a value of 17.5 kJ, what is the work component?
A) 5.5 kJ done by the system B) 5.5 kJ done on the system
C) 29.5 kJ done by the system D) 29.5 kJ done on the system
19. The reaction for the reaction of nitrogen with chlorine is
shown below. Using bond
enthalpies, determine the value of H for the reaction. Be sure
to draw Lewis structures of the products and reactants, to assist
in determining the bond order.
N2 (g) + 3Cl2 (g) 2NCl3 (g)
Table of Bond Energies (kJ/mol)
A) -17 kJ/mol B) +889 kJ/mol C) -56 kJ/mol D) +467 kJ/mol E)
+1067 kJ/mol
20. The reaction below is similar to the thermite reaction, but
uses black iron ore instead of
red iron ore. What is the value of Ho when 94.0 grams of Fe is
formed?
3Fe3O4 (s) + 8 Al (s) 4Al2O3 (s) + 9Fe (s) Ho = -3347.6
kJ/mol
A) -6.7 kJ B) -5.08x104 kJ C) -5.63x103 kJ D) -59.9 kJ E) -626
kJ
21. Liquid hydrogen peroxide decomposes according to the
reaction:
2H2O2 (l) 2H2O (l) + O2 (g) Ho = -196 kJ/mol
What is the value of H for the reaction shown below?
6H2O (l) + 3O2 (g) 6H2O2 (l)
A) + 196 / 3 kJ B) +6 x 196 kJ C) +3 x 196 kJ D) -196 / 3 kJ
C-H 413 N-H 391 O-H 463 H-H 436
C-F 485 N-F 272 O-F 190 H-F 565 F-F 155
C-Cl 328 N-Cl 200 O-Cl 203 H-Cl 431 Cl-Cl 242
C-Br 276 N-Br 243 O-Br 235 H-Br 366 Br-Br 193
C-I 234 O-I 234 H-I 299 I-I 151
C-C 347 N-N 163 C-N 293 C-O 358 O-O 146
C=C 612 N=N 418 C=N 615 C=O 799 O=O 495
C C 820 N N 941 C N 891 C O 1072
C-H 413 N-H 391 O-H 463 H-H 436
C-F 485 N-F 272 O-F 190 H-F 565 F-F 155
C-Cl 328 N-Cl 200 O-Cl 203 H-Cl 431 Cl-Cl 242
C-Br 276 N-Br 243 O-Br 235 H-Br 366 Br-Br 193
C-I 234 O-I 234 H-I 299 I-I 151
C-H 413 N-H 391 O-H 463 H-H 436
C-F 485 N-F 272 O-F 190 H-F 565 F-F 155
C-Cl 328 N-Cl 200 O-Cl 203 H-Cl 431 Cl-Cl 242
C-Br 276 N-Br 243 O-Br 235 H-Br 366 Br-Br 193
C-I 234 O-I 234 H-I 299 I-I 151
C-HC-H 413413 N-HN-H 391391 O-HO-H 463463 H-HH-H 436436
C-FC-F 485485 N-FN-F 272272 O-FO-F 190190 H-FH-F 565565 F-FF-F
155155
C-ClC-Cl 328328 N-ClN-Cl 200200 O-ClO-Cl 203203 H-ClH-Cl 431431
Cl-ClCl-Cl 242242
C-BrC-Br 276276 N-BrN-Br 243243 O-BrO-Br 235235 H-BrH-Br 366366
Br-BrBr-Br 193193
C-IC-I 234234 O-IO-I 234234 H-IH-I 299299 I-II-I 151151
C-C 347 N-N 163 C-N 293 C-O 358 O-O 146
C=C 612 N=N 418 C=N 615 C=O 799 O=O 495
C C 820 N N 941 C N 891 C O 1072
C-C 347 N-N 163 C-N 293 C-O 358 O-O 146
C=C 612 N=N 418 C=N 615 C=O 799 O=O 495
C C 820 N N 941 C N 891 C O 1072
C-C 347 N-N 163 C-N 293 C-O 358 O-O 146
C=C 612 N=N 418 C=N 615 C=O 799 O=O 495
C C 820 N N 941 C N 891 C O 1072
C-CC-C 347347 N-NN-N 163163 C-NC-N 293293 C-OC-O 358358 O-OO-O
146146
C=CC=C 612612 N=NN=N 418418 C=NC=N 615615 C=OC=O 799799 O=OO=O
495495
C CC C 820820 N NN N 941941 C NC N 891891 C OC O 10721072
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Exam 3
22. What is the approximate value of S for the reaction
below?
Ca2+ (aq) + 2HCO31-
(aq) CaCO3 (s) + CO2 (g) + H2O (l)
A) S < 0 B) S > 0 C) S ~ 0 D) cannot be predicted
23. Choose the correct statement that describes the reaction
below.
MgCO3 (s) MgO (s) + CO2 (g) H = +117.3 kJ/mol
A) The reaction is extensive at high temperature.
B) The reaction is extensive at low temperature.
C) The reaction is extensive at any temperature.
D) The reaction is not extensive at any temperature.
24. Mustard gas is prepared according to the reaction below.
Given that Keq = 5.48x10-1,
[SCl2] = 0.385 M and [C2H4] = 0.831 M, what is the concentration
of S(CH2CH2Cl)2 in the mixture?
SCl2 (g) + 2 C2H4 (g) S(CH2CH2Cl)2 (g)
A) 0.175 B) 0.485 C) 0.351 D) 0.146 E) 0.268
Use the reaction coordinate diagram below to answer the next
three questions regarding the
reaction: A-B + C A + B-C .
25. Which reaction above has the largest forward rate
constant?
A) I B) II C) III
26. Which reaction above has the smallest value of
Kequilibrium?
A) I B) II C) III
27. Which reaction(s) above will increase in the concentration
of [B-C] when heated?
A) I only B) II only C) III only D) I & II E) II &
III
5 kJ
10 kJ
15 kJ
A-B, C
A, B-C
reaction coordinate
1 kJ2 kJ
5 kJ
A-B, C
A, B-C
reaction coordinate
3 kJ
6 kJ
9 kJ
A-B, C
A, B-C
reaction coordinate
I II III
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Exam 3
28. Consider the following reaction at equilibrium.
2 C2H6O (aq) + 2CO2 (g) C6H12O6 (aq) H > 0 ethanol
glucose
Which changes would shift the equilibrium to the right?
I) addition of CO2
II) removal of CO2
III) removal of glucose
IV) heating the reaction
V) cooling the reaction
A) I, III, & IV B) II, III, & V C) I & IV D) I &
V E) II, III, & IV
I pledge that I have neither given nor received aid on this
exam.
Signature:______________________
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Exam 3 Special Code 111111 Petrovich, Fall 2010
Directions:
1) Please put away all papers, cell phones and clear the memory
on your calculators. 2) On the scantron sheet, fill and bubble in
your last name, first name, special code (111111)
and student identification number (000######). 3) On the paper
exam, print your last name and first name on page 1 of the exam. 4)
Completely bubble in your answers for questions 1-28 on the
scantron. 5) Please sign the honor pledge at the end of the exam.
6) Return all exam materials to Dr. Petrovich/TA before leaving
DAB222. 7) Failure to follow the exam labeling instructions will
result in a loss of 2 points on your
exam score.
Oxidation State Rules
1) The oxidation states of the atoms in an element are all
zero.
2) Fluorine is always assigned an oxidation number of -1.
3) Group 1A metals are +1, Group 2A metals are +2, and aluminum
is +3.
4) H is +1 when bonded to non-metals. H is 1 when bonded to
metals. 5) Oxygen is assigned an oxidation number of 2. 6) Group 7A
elements are assigned an oxidation number of -1.
PV = nRT G = H - T S R = 0.0821 L*atm/K*mol or 8.314 J/K*mol 1
atm = 760 mm Hg = 760 torr
K = C + 273.15 H = coeffxDbonds broke coeffxDbonds formed
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Exam 3
Key:
1) A 15) E
2) B 16) B
3) D 17) B
4) C 18) A
5) A 19) D
6) C 20) E
7) A 21) C
8) B 22) B
9) C 23) A
10) C 24) D
11) E 25) A
12) B 26) B
13) D 27) E
14) B 28) A