KING FAHD UNIVERSITY OF PETROLEUM AND MINERALS
CHEMISTRY DEPARTMENT
CHEM 102 FINAL EXAM
TERM 122
005
TEST CODE NUMBER
STUDENT NUMBER:
NAME :
SECTION NUMBER:
_____________________________
_____________________________
_____________________________
INSTRUCTIONS
1. Write your student number, name, and section number on the EXAM COVER page.
2. Write your student number, section number, and your name on your EXAM ANSWER FORM.
3. Bubble in pencil your student number and your section number on the EXAM ANSWER
FORM.
4. Bubble in pencil on your EXAM ANSWER FORM the correct answer to each of the questions.
You must not give more than ONE answer per question.
5. At the end of the exam return the EXAM ANSWER FORM to the proctor.
6. The exam contains 40 multiple choice questions and the time allowed is 160 min.
PLEASE TURN OFF YOUR CELL PHONE AND
PLACE IT UNDER YOUR SEAT
Important constants
Gas Constant (R)
Planck’s Constant (h)
Speed of light (c)
Avogadro’s number (N)
Bohr’s Constant (RH)
Faraday (F)
Specific heat of H2O
= 0.08206
= 8.314
= 8.31 x 107
= 6.626 x 10-34
= 6.626 x 10-34
= 2.998 x 108
= 6.022 x 1023
= 2.179 x 10-18
= 96500
= 4.184
Page 1
L.atm/(mol.K)
J/(mol.K)
g.cm2/(sec2.mol.K)
J.sec/particle
kg.m2/(sec.particle)
m/sec
particles/mole
J/particle
Coulombs/mol eJ/(g.oC)
Name: __________________________ Date: _____________
1. For a reaction that follows the general rate law, Rate = k [A] [B]2, suppose the rate of
the reaction at certain initial concentrations of A and B is 0.0115 M/s. What is the rate
of this reaction if concentrations of both A and B are doubled?
A)
B)
C)
D)
0.023 M/s
0.046 M/s
0.092 M/s
0.184 M/s
2. A certain reaction, A  products, has a rate that slows down as the reaction
proceeds. The half-life of the reaction is found to depend on the initial concentration
of A. Which of the following statement is true about this reaction?
A) A doubling of the concentration of A doubles the rate of the reaction.
B) A polt of 1/ [A] versus time is linear.
C) The half-life of the reaction gets longer when the initial concentration of A is
increased.
D) A polt of the concentration of A versus time has a constant slope.
3. Hydrogen iodide decomposes at 800 K via a second-order process to produce
hydrogen and iodine according to the following chemical equation.
2 HI(g) → H2(g) + I2(g)
At 800 K, it takes 142 seconds for the initial concentration of HI to decrease from
-2
-2
6.75×10 M to 3.50×10 M. What is the rate constant for the reaction at this
temperature?
A)
B)
C)
D)
-1 -1
10.3 M s
-4
-1 -1
5.12×10 M s
-1
1.95×103 M-1s
-1 -1
9.69×10-2 M s
Page 2
4. Each of the following diagrams (I, II, III, IV) describes a possible reaction:
A2(g)
+
B2(g)
⇌
2 AB(g)
Assume that you begin with equal amounts of A2 and B2, but no AB, and assuming
that ΔS is the same for all of the possible reactions, which of these diagrams would
represent that the amount of AB(g) at equilibrium is the greatest?
A)
B)
C)
D)
I
II
III
IV
5. When 2.00 mol each of H2(g) and Cl2(g) are reacted in a 1.00 L container at a certain
temperature, 3.50 mol of HCl is present at equilibrium.
H2(g)
+
Cl2(g)

2 HCl(g)
Calculate the value of the equilibrium constant, Kc.
A)
B)
C)
D)
196
140
56.0
33.0
6. For the following reaction:
CO(g) + Cl2(g)  COCl(g) + Cl(g)
Keq = 1.5×10-39
If the rate constant, k, for the forward reaction is 1.4×10-28 L.mol-1.sec-1 , what is k (in
L. mol-1.sec-1) for the backward reaction?
A)
B)
C)
D)
9.3×1010
1.0×10-11
2.1×10-67
7.1×1027
Page 3
7. Consider these reactions and their corresponding equilibrium constants.
½ N2
+

O2
2 NO2

2 NO
NOBr

NO
NO2
+
+
K1
O2
K2
½ Br2
K3
Express the K value for the reaction below in terms of K1, K2, and K3.
½ N2
+
½ O2
+
½ Br2

NOBr
K=?
A) K1 K 21/ 2
K3
B) K1 + K 21/ 2 – K3
C)
D)
K1 K 2
2K 3
K1 +
K2
– K3
2
8. Consider the equilibrium
2 NOBr(g)

2 NO(g)
+
Br2(g)
If nitrosyl bromide (NOBr) is 34 percent dissociated at 25oC and the total pressure is
0.25 atm, calculate Kp for the dissociation at this temperature.
A)
B)
C)
D)
9.6103
3.9104
4.5102
5.0102
9. Of the following carboxylic acids, which is the most acidic?
A)
B)
C)
D)
Cl3CCO2H
HCO2H
CH3CO2H
(CH3)3CCO2H
10. Calculate the [H+] in a 0.25 M solution of methylamine, CH3NH2 (Kb = 4.4×10-4).
A)
B)
C)
D)
1.0×10-2
9.5×10-13
9.1×10-11
1.1×10-4
Page 4
11. Which salt produces the most alkaline solution at a concentration of 0.1 M?
A)
B)
C)
D)
MgCl2
NH4I
KClO4
NaNO2
12. Calculate the concentration of H+, in a 0.25 M H2C2O4 solution. Ka1 and Ka2 for oxalic
acid (H2C2O4) are 6.5102 and 6.1105, respectively.
A)
B)
C)
D)
3.3105 M
0.099 M
0.13 M
6.1105 M
13. 1.0 L of an aqueous solution in which [H2CO3] = [HCO3-] = 0.10 M, has [H+] =
4.2×10-7. What is the [H+] after 0.005 mole of NaOH has been added?
A)
B)
C)
D)
2.2×10-8 M
2.1×10-9 M
3.8×10-7 M
4.6×10-7 M
14. The solubility product (Ksp) for Fe(OH)2 and Fe(OH)3 are 8.0×10-15 and 6.0×10-38,
respectively. What are the concentrations of Fe2+ and Fe3+at pH 8?
A)
B)
C)
D)
8.0×10-3
8.0×10-3
4.0×10-7
1.3×10-5
and
and
and
and
6.0×10-20
1.2×10-2
6.0×10-14
2.2×10-10
15. A solution of Pb(NO3)2 is added dropwise to a second solution in which [Cl-] = [F-] =
[I-] = [SO42-] = 0.001 M. What is the first precipitate that forms?
A)
B)
C)
D)
PbSO4
PbF2
PbI2
PbCl2
(Ksp = 1.8×10-8)
(Ksp = 3.7×10-8)
(Ksp = 8.5×10-9)
(Ksp = 1.5×10-5)
Page 5
16. For a certain process the entropy change, ΔS, is +148.3 J/molK and the free energy
change, ΔG, is +146 kJ/mol at 35°C. Find ΔH at 35°C.
A)
B)
C)
D)
192 kJ/mol
151 kJ/mol
141 kJ/mol
100. kJ/mol
17. Consider the reaction
2 SO2(g)
+
O2(g)

2 SO3(g)
carried out at 25oC and 1 atm. Calculate the equilibrium constant for this reaction at
25oC, using the following data:
A)
B)
C)
D)
Substance
ΔHf° (kJ/mol)
So (J/mol)
SO2(g)
-297
248
SO3(g)
-396
257
O2(g)
0
205
K = 2.06×1057
K = 1.98
K = 8.69×1024
K = 332
18. The following diagrams show a spontaneous chemical reaction. What can you
deduce about Ssurr for this process?
A)
B)
C)
D)
ΔSsurr is negative
ΔSsurr is positive
ΔSsurr is zero
This diagram alone is not enough to deduce the sign of ΔSsurr.
Page 6
19. Which of the following is true about carbon monoxide?
A)
B)
C)
D)
single largest source is from internal combustion engine
results from the actions of ultraviolet light on ozone
is a secondary pollutant
major cause of cancer in smokers
20. Of the following materials, which contributes most to the production of acid rain?
A)
B)
C)
D)
Nitric oxide
Uranium hexafluoride
Phosphate detergents
Chloroflurocarbons
21. Which of the following is a possible consequence of increasing carbon dioxide in the
atmosphere?
A)
B)
C)
D)
An increase in chlorofluorocarbons in the atmosphere.
An increase in ultraviolet radiation reaching the Earth's surface.
A rise in sea level.
depletion of ozone layer.
22. What is the oxidation number of vanadium, V, in the complex compound
K3[V(EDTA)(CN)Br]?
A)
B)
C)
D)
+3
+5
+6
+1
23. What is the coordination number of manganese, Mn, in the complex ion
[Mn(en)(C2O4)(CO)2] ?
A)
B)
C)
D)
6
3
4
8
24. What is the name of the coordination compound [Fe(NH3)3(CO)3](NO3)3?
A)
B)
C)
D)
Triamminetricarbonyliron(III) nitrate
Iron(III) triamminetricarbonyl nitrate
Iron(III)trisamminetriscarbonyl trinitrate
Triamminetricarbonylferrate(III) nitrate
Page 7
25. What is the formula of dichlorobis(ethylenediamine)platinum(IV) sulfate?
A)
B)
C)
D)
Pt[en)2Cl2]SO4
[Pt(en)2Cl2]SO4
[Pt(en)2Cl2]2SO4
[Pt(en)2Cl2(SO4)]
26. Predict the number of unpaired electrons in the two octahedral complex ions [PdI6]3and [Pd(CO)4(CN)2], respectively?
Note: I- is a weak-field ligand, whereas CO and CN- are strong-field ligands.
A)
B)
C)
D)
4, 0
5, 1
3, 2
4, 2
27. How many isomers exist for the square planar species Pt(H2O)(NH3)ClBr?
A)
B)
C)
D)
1
2
4
3
Page 8
28. A radioactive substance undergoes decay as follows:
Time Mass (g)
(days)
0
500
1
389
2
303
3
236
4
184
The half-life of the reaction of the first-order decay is:
A)
B)
C)
D)
5.56 day
2.76 day
1.39 day
0.67 day
29. An isotope with a high value of n/p will tend to decay through
A)
B)
C)
D)
 decay
 decay
electron capture
 decay
30. What nuclide is formed when
alpha, alpha, alpha?
A) 222
86
B) 226
88
C) 230
238
92
U undergoes the decay series: alpha, beta, beta,
Rn
Ra
Th
90
D) 206
Pb
82
Page 9
31. The term “critical mass” means the…
A) Amount of fissionable material which will self-sustain a nuclear chain reaction
B) Differences between mass of individual protons and neutrons and the mass of
nucleus
C) Energy which holds the nucleus together
D) Mass of fuel in a nuclear reactor core
32. Calculate the energy released in joules when one mole of polonium-214 decays
according to the equation
214
Po
84

4
210
Pb + He
2
82
[Atomic masses: Pb-210 = 209.98284 amu, Po-214 = 213.99519 amu, He-4 =
4.00260 amu, 1 amu = 1.66053892 × 10-27 kg ], [1 J = kg.m2/s2]
A)
B)
C)
D)
8.78 x 1014 J/mol
–9.75 x 10–3 J/mol
7.2 x 1014 J/mol
8.78 x 1011 J/mol
33. A redox reaction employed in an electrochemical cell has a negative ΔGºrxn. Which of
the following must be true:
A)
B)
C)
D)
Eº is positive, K < 1
Eº is positive, K > 1
Eº is negative, K < 1
Eº is negative, K > 1
34. A galvanic cell employs the following reaction,
Sn2+(aq) + Mn(s)

Sn(s) + Mn2+(aq)
Calculate the cell potential at 25 oC if [Sn2+] = 0.010 M, [Mn2+] = 2.00 M.
(EoSn2+/Sn = - 0.14 V, EoMn2+/Mn = - 1.18 V)
A)
B)
C)
D)
+ 0.97
- 0.97
+ 1.11
- 1.11
Page 10
35. Which of the following metals, if coated onto iron, would prevent the corrosion of iron
Ag+ + e- → Ag(s)
Fe2+ + 2e- → Fe (s)
Cu2+ + 2e- → Cu(s)
Zn2+ + 2e- → Zn(s)
Sn2+ + 2e- → Sn (s)
A)
B)
C)
D)
Eo = + 0.80 V
Eo = - 0.44 V
Eo = + 0.34 V
Eo = - 0.76 V
Eo = - 0.14 V
Zn
Ag
Cu
Sn
36. Which one of these molecules cannot serve as a monomer for an addition polymer?
A) ClCH=CH2
B) H2C=CH–CN
C)
D)
37. What is the process called to prepare a ceramic by heating a slurry of a powder of an
inorganic substance in water to a very high temperature under pressure?
A)
B)
C)
D)
Sintering
Roasting
Firing
Sol-gel
38. Two-dimensional sheets of sp2-hybridized carbon atoms are called:
A)
B)
C)
D)
graphenes
diamond
fullerenes
carbon nanotubes
Page 11
39. Which of the following combination of elements would be expected to produce a
semiconductor?
A)
B)
C)
D)
Ga and Se
As and N
B and P
Zn and Sb
40. Which of the following molecules is likely to form a liquid crystalline phase?
A)
B)
C)
D)
41. Which of the following statements best describes the relationship between the two
structures shown?
A)
B)
C)
D)
They are the same compound.
They are constitutional isomers.
They are geometric isomers.
They are stereoisomers.
42. Which one of the following is considered a pair of constitutional isomers?
A)
B)
C)
D)
2-bromo-3,4-dimethylhexane & 3-bromooctane
3-bromo-4-ethylhexane & 2-methyl-3-bromohexane
3-methyl-5-bromoheptane & 3-methyl-4-bromohexane
3-bromo-4-ethylhexane & 2-bromo-2-methylhexane
Page 12
43. Which of the labeled atoms in the following structure are sp2 hybridized?
A)
B)
C)
D)
2, 3 and 4
3 and 4
2 and 4
2 and 3
44. Which of these pairs are geometric isomers?
A) CH3CH2–O–CH2CH3 and CH3CH2CH2CH2OH
B)
C)
D)
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Page 14
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Answer Key
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
31.
32.
33.
34.
35.
36.
37.
38.
39.
40.
41.
42.
43.
44.
C
B
D
D
A
A
A
A
A
B
D
B
C
A
A
A
C
A
A
A
C
A
A
A
B
C
D
B
B
A
A
D
B
A
A
D
A
A
C
C
A
A
D
C
Page 16