KING FAHD UNIVERSITY OF PETROLEUM AND MINERALS
CHEMISTRY DEPARTMENT
CHEM 102-102
FINAL EXAM (JULY 07, 2011)
TEST CODE NUMBER 000
STUDENT NUMBER: _____________________________
NAME :
_____________________________
SECTION NUMBER: _____________________________
INSTRUCTIONS
1.
2.
3.
4.
5.
6.
Write your student number, name, and section number on the EXAM COVER page.
Write your student number, section number, and your name on your EXAM ANSWER FORM.
Bubble in pencil your student number and your section number on the EXAM ANSWER FORM.
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.
At the end of the exam return the EXAM ANSWER FORM to the proctor.
The exam contains 40 multiple choice questions and the time allowed is 160 min (2 hrs and 40 min). Time
will be announced after 80 minutes and again 10 minutes before the end of the exam.
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
= 0.0821
= 8.314
= 8.314 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
= 4.18
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)
IDENTIFYING SECTIONS USING RECITATION TIMES
ALHOOSHANI
Section
01
02
03
Day
T
U
T
Time
10 a.m.
10 a.m.
11 a.m.
Day
T
T
U
Time
8 a.m.
9 a.m.
9 a.m.
Day
U
U
T
Time
8 a.m.
9 a.m.
8 a.m.
AL-SAADI
Section
04
05
06
OWEIMREEN
Section
07
09
08
Page 2
1. Which of the following choices is correct for an Aspirin molecule?
Aspirin
Number of C atoms
Number of H atoms
A)
9
8
B)
9
10
C)
8
6
D)
8
12
2. Which of the following statements about isomerism in organic molecules is NOT
correct?
A) Optical isomers result from rotating the molecules about a double or a triple bond.
B) Optical isomers have structures that are mirror images of each other but are not
superimposable.
C) Optical isomers have almost identical physical properties but differ in their
chemical reactions.
D) An optical isomer rotates plane polarized light.
Page 4
3. What is the correct name for the following molecule?
A)
B)
C)
D)
3-ethyl heptane.
1-butyl-1-ethyl-2-methyl ethane.
1-butyl-1-ethyl propane.
3-butyl pentane.
4. What is the half-life (in minutes) of the first order reaction,
A
Æ
B
if 25 % of A decompose after 42 minutes?
A)
B)
C)
D)
101
21
84
120
Page 5
5. A study of the decomposition reaction,
RS2 Æ
R
+ 2S
gave the following data::
-1
Initial [RS2] (mol L
0.150
0.250
0.350
0.500
)
-1 -1
Initial Rate (mol L
0.0394
0.109
0.214
0.438
s )
The rate constant for this reaction is:
A) 1.74 L mol
B) 0.263 L mol
C) 0.571 L mol
D) 1.17
L mol
-1 -1
s
-1 -1
s
-1 -1
s
-1 -1
s
6. The equilibrium constant for the reaction,
H2 (g)
+ CO2 (g)  H2O (g)
+ CO (g)
is 4.2 at 1650 ∞C. If initially 0.80 mol of H2 and 0.80 mol of CO2 gases were
in a 5.0-L vessel at 1650 ∞C, what is the concentration of CO2 when the system
reaches equilibrium at 1650 ∞C?
-1
A) 0.052 mol L
-1
B) 0.16
mol L
C) 0.11
mol L
D) 0.27
mol L
-1
-1
7. Equilibrium is reached in a chemical reaction when,
A)
B)
C)
D)
the rates of the forward and backward reactions become equal.
the concentrations of reactants and products become equal.
the numbers of moles of reactants and products become equal.
the forward and backward reactions stop.
Page 6
8. Consider the equilibrium,
2 H2 (g)
+ O2 (g)

2 H2O (g)
An increase in pressure would produce more,
A) H2O.
B) H2 and O2.
C) H2 only.
D) O2 only.
9. What is the pH of a 0.050 M solution of triethylamine (C2H5)3N?
-4
Kb for triethylamine is 5.3 ¥ 10 .
A)
B)
C)
D)
11.71
8.68
5.32
2.29
10. What is the pH of a 0.20 M solution of NH4Cl?
-5
Kb (NH3) = 1.8 ¥ 10
A)
B)
C)
D)
.
4.98
3.74
6.53
9.02
-5
11. A 10.0 mL sample of 0.75 M CH3CH2COOH (Ka = 1.3 ¥ 10 ) is titrated
with 0.30 M NaOH. What is the pH of the solution after 22.0 mL of NaOH
have been added to the acid?
A)
B)
C)
D)
5.75
4.94
4.83
4.02
Page 7
12. When a weak acid is titrated with a strong base, the pH at the equivalence
point is :
A)
B)
C)
D)
greater than 7
less than 7
is equal to 7
equal to pKa of the acid
13. The solubility of PbCl2 in water is 0.45 g in 100 mL of solution. Ksp for
PbCl2 is :
-5
A) 1.7 ¥ 10
-6
B) 8.5 ¥ 10
-6
C) 4.2 ¥ 10
-2
D) 4.9 ¥ 10
14. Which of the following choices is correct for the reaction,
N2 (g) + 2 O2 (g)
Æ 2 NO2 (g)
at constant pressure and 25 ∞C?
DSsurr is
A) - 223 J K -1
B)
+ 223 J K
-1
The reaction is
Non-spontaneous
Spontaneous
C) - 2.66 kJ K -1
Spontaneous
D) + 2.66 kJ K -1
Non-spontaneous
Page 8
DH = + 66.4 kJ
15. For the vaporization process,
A (l)
Æ
A (g)
at the normal boiling point of 90 ∞C, DH∞ is 68.6 kJ mol
-1 -1
is 310 J mol K , calculate S∞, in J mol
A)
B)
C)
D)
-1
-1
-1
. If at 90 ∞C, S∞ for A(g)
K , for A (l) at 90 ∞C.
121
452
189
85.4
16. Calculate Ecell for the cell in which the reaction,
2 VO 2  (aq)  4 H  (aq)  Zn(s)  2 VO 2 (aq)  2H 2O(l)  Zn 2 (aq)
+
+
2+
occurs at 25 ∞C when [VO2 ] = 2.0 M , [H ] = 0.50 M , [VO ] = 0.0 10 M
2+
and [Zn ] = 0. 10 M. Given the following standard reduction potentials
at 25 ∞C.
VO2  (aq )  2 H  ( aq )  e   VO 2 ( aq )  H 2O (l )
Zn 2 (aq)  2 e   Zn( s )
A)
B)
C)
D)
1.89
1.31
1.63
2.06
V
V
V
V
Page 9
E∞ =
1.00 V
E∞ = - 0.76 V
17. Given the following data at 25 ∞C,
2+
Species
DGf ∞ ( kJ mol
-1
Pb (aq)
- 24.4
)
-
Br (aq)
- 104.0
PbBr2 (s)
- 261.9
-1
Calculate the solubility, in mol L , of PbBr2 in water, at 25 ∞C.
-2
A) 1.19 ¥ 10
-9
B) 9.89 ¥ 10
-4
C) 1.29 ¥ 10
-17
D) 7.87 ¥ 10
18. In the galvanic cell,
Fe(s)ΩFe
2+
+
(aq, 0.00100 M)ΩΩH (aq, x M), H2 (g, 1 atm)ΩPt(s)
+
the H ions are provided by a 1.00 M weak monoprotic acid HA.
At 25 ∞C the cell has a potential of 0.333 V. Given the following
standard reduction potential at 25 ∞C
Fe
2+
(aq) + 2 e
-
Æ
E∞ = - 0.440 V
Fe (s)
calculate Ka for the acid at 25 ∞C.
-7
A) 2.4 ¥ 10
-11
B) 5.7 ¥ 10
-10
C) 2.4 ¥ 10
-5
D) 1.6 ¥ 10
Page 10
19. Calculate the equilibrium constant at 25 ∞C for the reaction,
Ni (s)
+
Cd
2+
(aq)

Cd (s)
+
NI
2+
(aq)
given the following standard reduction potentials at 25 ∞C.
2+
Cd
NI
2+
(aq) + 2 e
(aq) + 2 e
-
-
Æ
Cd (s)
E∞ = - 0.25 V
Æ
Ni (s)
E∞ = - 0.40 V
5
A) 1.2 ¥ 10
-5
B) 1.0 ¥ 10
2
C) 3.4 ¥ 10
-6
D) 8.6 ¥ 10
20. What would the voltage of the fuel cell based on the reaction,
H2 (g)
+ 1/2 O2 (g) Æ H2O (l)
be assuming it is working reversibly at 25 ∞C and 1 atm?
-1
( G f  for H2O (l) = - 237 kJ mol )
A)
B)
C)
D)
1.23
0.246
0.0614
2.37
V
V
V
V
21. Which of the following occurs when a nuclide captures an electron?
Mass Number (A) Atomic Number (Z)
A) Unchanged
B)
Decreases
Decreases
Decreases
C) Increases
Increases
D) Unchanged
Increases
Page 11
22. How many neutrons are produced when an
spotaneous fission to
A)
B)
C)
D)
134
I and
107
244
95
Am nuclide undergoes
Mo ?
3
4
1
2
23. Which of the following processes is nuclear fusion?
H 
3
1
H 
A)
2
1
B)
241
95
Am 
C)
214
82
Pb 
D)
235
92
U 
1
0
He 
He 
237
93
e 
Bi
4
2
0
1
4
2
n 
214
83
139
56
1
0
n
Np
Ba 
94
36
K  3 01 n
24. How old is a geological sample containing 4.2017 mmoles 238 U and
1.6359 mmoles 206 Pb .
Assume that all the 206 Pb in the sample was originally 238 U and a
9
half-life of 4.5 ¥ 10 years for the overall decay steps from 238 U to
206
Pb .
9
A) 2.1 ¥ 10
years
B) 2.4 ¥ 10
years
C) 7.1 ¥ 10
years
D) 7.3 ¥ 10
years
10
9
10
25. The mass of a
107
Ag nucleus is 106.879289 amu. Determine its binding
-1
energy in units of MeV nucleon given the following information.
Mass of a proton = 1.007280 amu
Mass of a neutron = 1.008665 amu
-13
1 MeV = 1.6022 ¥ 10 J
23
1 g = 6.022 ¥ 10 amu
A)
B)
C)
D)
8.56
9.16
922
8.99
Page 12
9
26. What is the wavelength in nm (1 m = 10 nm) of the photon needed for the dissociation
reaction,
O3 (g)  O (g) + O2 (g)
-1
given that the energy of an O-O bond in O3 is 107.2 kJ mol .
3
A) 1.116 ¥ 10
B) 8944
6
C) 1.116 ¥ 10
5
D) 9.003 ¥ 10
27. Which of the following reactions is an example of nitrogen fixation?
A) N2 + O2 → 2NO
+
B) NH3 + H2O → NH4
-
+ OH
C) 2 N2O → 2 N2 + O2
D) 2 NO2 + H2O → HNO2 + HNO3
28. The presence of ozone (O3) in the upper atmosphere is important because it,
A)
B)
C)
D)
absorbs harmful solar UV radiation.
absorbs radiation from earth thus helping to keep the earth warm.
dissolves in water droplets and is very essential for plants.
is a major reactant in the photosynthesis process.
29. Which of the following gases is NOT a greenhouse gas?
A) Cl2
B) CO
C) CO2
D) H2O
Page 13
30. Which of the following statements is NOT correct?
A) CO is poinsoness and can lead to death because it binds very strongly to Fe(II) in
hemoglobin.
B) Both CO and CO2 bind to Fe(II) in hemoglobin which is present in blood.
C) Formaldehyde released from industrial products used in homes causes respiratory
illnesses.
D) Good ventillation of houses minimizes the risk from products of 222 Ra decay.
31. Which one of the following choices is completely correct for the
2compound K [ Co (C2O4)2 (H2O)2 ], where C2O4 is the oxalate ion?
Oxidation number Coordination number
A)
3
6
B)
2
4
C)
4
6
D)
3
4
-
32. The systematic name for [ Co Cl3 (H2O) ]
A)
B)
C)
D)
aquotrichlorocobaltate(II)
cobalt(II) chloride monohydrate
aquotrichlorocobalt(II)
aquotrichlorocobaltite(II)
-
33. Given that F is a weak-field ligand find the number of unpaired electrons
3-
in [ Co F6 ] .
A)
B)
C)
D)
4
0
1
2
Page 14
34. Which of the following complexes shows geometric isomerism?
A) K [ Co (NH3)2 Cl4 ]
B) [ Co (NH3)5 Cl ] Cl2
C) [ Co (NH3)6 ] Cl3
D) [ Co (NH3)5 Cl ] SO4
35. Which one of the following transition metals does NOT form colored compounds?
A)
B)
C)
D)
Zn
Cu
Ni
Cr
36. Which of the following is not a semiconductor?
A)
B)
C)
D)
Sn
Si
Ge
C (graphite)
37. The polymer,
O
(
HOCH2C
O
)n
OCHC
CH3
used in degradable stitches and prepared from reacting
O
H
glycolic acid
OCHC
CH3
O
OH
and
is :
A)
B)
C)
D)
a condensation copolymer.
an addition block copolymer.
a substitution graft copolymer.
a dehydgrogenation random copolymer.
Page 15
Lactic acid HOCH2C
OH
38. Which of the following statements is NOT correct?
A)
B)
C)
D)
3
The hybridization of C atoms in a nanotube is sp .
The smectic phase in a liquid crystal consists of ordered molecules in layers..
Doping Si with Sb produces a semiconductor of the n-type.
Combining Zn and Sb is not expected to produce a semiconductor.
39. The monomer from which the polymer,
[CCl2 ‒ CH2 ‒ CCl2 ‒ CH2 ‒ CCl2 ‒ CH2 ‒ CCl2 ‒ CH2] n
is produced, is :
A)
B)
C)
D)
CCl2 = CH2
Cl2C ‒ CH2
n Cl2C = CH2 = CCl2
n CHCl2
40. Which of the following statements is NOT correct?
A) Ceramic materials can be produced by sintering which produces particles of
a uniform size.
B) Electrical and heat insulation are very important properties of ceramic materials.
C) Ceramic materials are composed of polymeric inorganic materials that can stand
very high temperatures.
D) The sol-gel process produces ceramics through condensation polymerization.
Page 16
Answer Key
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40.
A
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A
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A
A
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