KING FAHD UNIVERSITY OF PETROLEUM AND MINERALS
CHEMISTRY DEPARTMENT
CHEM-102-061-FINAL EXAM


TEST CODE NUMBER 000

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 (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)
= 0.0821
= 8.31
= 8.31 x 107
L.atm/(mol.K)
J/(mol.K)
g.cm2/(sec2.mol.K)
Planck’s Constant (h)
= 6.626 x 10-34
= 6.626 x 10-34
J.sec/particle kg.m2/(sec.particle)
Velocity of light (c)
= 2.998 x 108
m/sec
Avogadro’s number (N)
= 6.022 x 1023
particles/mole
Bohr’s Constant (RH)
= 2.179 x 10-18
J/particle
Faraday (F)
= 96485
Coulombs
Specific heat of H2O
= 4.18
J/(g.oC)




1.
If for the reaction,
3 ClO – (aq)     →     ClO3 – (aq)     +     2 Cl – (aq)
doubling the concentration of ClO – increases the initial rate of formation
of ClO3 – four times, then the rate expression is
A.
rate = k [ClO –]2
B.
rate = k [ClO –]3
C.
rate = k [ClO –]2 [ClO –]4
D.
rate = k [ClO –] [Cl –]2


2.
The activation energy for a certain reaction is 30 kJ. When a catalyst is
used, the reaction takes place more rapidly. A possible value for the
activation energy of the catalyzed reaction would be,
A.
– 30 kJ
B.
  20 kJ
C.
  30 kJ
D.
  40 kJ


3.
If the overall reaction,
      NO2      +      CO      →      NO      +      CO2
occurs by the following two step mechanism,
                           2 NO2       →        NO3      +      NO        (slow)
           NO3      +      CO       →         NO2     +      CO2       (fast)
then the rate expression for the overall reaction is:
A.
rate = k [NO2] [CO]
B.
rate = k [NO3] [CO]
C.
rate = k [NO2]2
D.
rate = k [NO] [CO2]


4.
For the equilibrium,
   2 SO2 (g)       +       O2 (g)       ⇌       2 SO3 (g)         ΔH < 0
more SO2 can be produced by:
A.
expanding the container.
B.
lowering the temperature.
C.
removing some SO3.
D.
increasing the total pressure.


5.
Given the following equilibria and their equilibrium constants (K values)
        2 CO (g)     +    O2 (g)    ⇌    2 CO2 (g)             K = 200
   2 NO2 (g)    ⇌    2 NO (g)     +    O2 (g)            K = 0.50
at a particular temperature, determine the value of K for the equilibrium,
   CO (g)      +     NO2 (g)      ⇌     NO (g)      +       CO2 (g)
at the same temperature
A.
10
B.
100
C.
200
D.
400


6.
Consider the reaction
      2 HI (g)       ⇌      H2 (g)      +      I2 (g)            K = 0.040
If initially only pure HI is in a container at a pressure of 1.00 atm ,
the equilibrium partial pressure of H2 will be:
A.
0.02 atm
B.
0.075 atm
C.
0.14 atm
D.
0.16 atm


7.
A 1.00 M aqueous solution of a monoprotic acid has a pH of 2.42.
pKa for this acid is:
A.
1.21
B.
2.42
C.
3.63
D.
4.84


8.
Given Kb = 7.1 x 10 –10 for the acetate (C3H5O2 –) ion; what is the pH
of an aqueous 0.75 M NaC3H5O2 solution?
A.
4.64
B.
8.26
C.
9.15
D.
9.36


9.
Given the weak polyprotic acid H3A which of the following species
is expected to be the strongest acid?
A.
H3A (aq)
B.
H2A – (aq)
C.
HA 2– (aq)
D.
A 3– (aq)


10.
The solubility product (Ksp) of lead iodate, Pb(IO3)2, in water
is 2.6 x 10 –13. Calculate the molar solubility of lead iodate.
A.
5.1 x 10 –7 M
B.
4.0 x 10 –5 M
C.
6.4 x 10 –5 M
D.
2.2 x 10 –2 M


11.
A buffer solution of pH = 5.25 is to be prepared from acetic acid
(HC2H3O2 with Ka = 1.80 x 10 –5), sodium acetate (NaC2H3O2)
and water. What must the molar ratio of acetate ion to acetic acid,
( [C2H3O2–] / [HC2H3O2] ) be in this solution?
A.
0.31
B.
0.91
C.
1.1
D.
3.2


12.
Strontium sulfate (SrSO4) is slightly soluble in water. In which
of these aqueous solutions would it be least soluble?
A.
0.1 M Na2SO4
B.
0.01 M K2SO4
C.
0.2 M KNO3
D.
pure water.


13.
The formula of tris(ethylenediamine)chromium(III) tetrachloroferrate(III) is,
A.
[Cr(en)4][FeCl4]
B.
[CrFe(en)3Cl4]
C.
[Cr(en)3][FeCl4]3
D.
[Cr(NH3)3]3[FeCl3]4


14.
The wavelength of maximum absorption for the [Cr(H2O)6]2+ complex
ion is 719 nm. This corresponds to a splitting energy (Δo) of,
A.
166 kJ mol –1
B.
276 kJ mol –1
C.
417 kJ mol –1
D.
922 kJ mol –1


15.
Given that CN– is a strong field ligand how many unpaired electrons
does the manganese ion in [Mn(CN)6]4– have?
A.
1
B.
2
C.
3
D.
5


16.
Consider the oxidation of NO2 by the reaction:
      4 NO2 (g)      +      O2 (g)      →      2 N2O5 (g)
for which the following thermodynamic data is supplied:

       Substance          (kJ mol –1)             (J mol –1 K –1)
         
          N2O5                  – 2.40                             6.48
          NO2                      1.94                             13.7
          O2                         0.00                             11.7

Determine the temperature range over which this reaction is
spontaneous.
A.
T > 0 K
B.
T < – 38 ºC
C.
T > 4.3 ºC
D.
T < – 235 ºC


17.
Given that,

   CO (g) = – 110 kJ mol –1 and CO2 (g) = – 393 kJ mol –1

the reaction,

      2 CO2 (g)       ⇌    2 CO (g)      +       O2 (g)

is expected to be
A.
spontaneous at all temperatures.
B.
non-spontaneous at all temperature.
C.
spontaneous only at sufficiently low temperatures.
D.
spontaneous only at sufficiently high temperatures.


18.
If = – 95.8 kJ at 25 °C for the reaction,

      CH4 (g)      +      C2H2 (g)       ⇌      C3H6 (g)

determine the value of the equilibrium constant (K) for this

reaction at 25 °C.
A.
1.0
B.
460
C.
1.7 x 10 11
D.
6.1 x 10 16


19.
The electrochemical cell

      Ni Ni 2+ (aq, 0.10) H + (aq, M=?) H2 (g, 1atm.) Pt

Has a voltage of 0.050 V. Given the standard potentials;

       Ni 2+ (aq)     +     2 e –     →      Ni (s)          = – 0.236 V

       2 H + (aq)    +     2 e –     →      H2 (g)          =     0. 000 V

Calculate the pH of solution around the Pt cathode.
A.
1.08
B.
1.34
C.
2.95
D.
3.64


20.
Given that,

   Cu 2+ (aq)      +      2 e –     →      Cu (s)    =    0.34 V

   I2 (s)              +      2 e –     →      2 I – (aq)    =    0.54 V

then the reaction,

   Cu 2+ (aq)      +      2 I – (aq)      →      I2 (s)      +      Cu (s)
A.
is nonspontaneous under standard conditions.
B.
has a ΔG º < 1.
C.
has a K > 1.
D.
takes place in a voltaic cell.


21.
What is the current in amperes that is required to plate 10.0 g

of copper (Cu) metal from an aqueous Cu 2+ solution in an

electrolytic cell over a period of 10.0 minutes?
A.
0.157
B.
0.315
C.
30.4
D.
50.6


22.
The overall half-life for the multi-step decay process:

      

is 4.5 x 10 9 years. What is the age of a rock containing 50.0 mg

of and 24.0 mg of assuming that all the present

was produced by the decay process only? (Hint: determine how many

mg. of were consumed to produce 24.0 mg of )
A.
2.16 x 10 9 years.
B.
2.87 x 10 9 years.
C.
4.77 x 10 9 years.
D.
4.27 x 10 11 years.


23.
A radiation measuring device indicated that 2.50 x 10 10 radioactive

atoms in a sample decay at the rate of 237 atoms s –1. The half-life of

the radioactive atoms is:
A.
9.48 x 10 –9 s
B.
7.31 x 10 7 s
C.
1.05 x 10 8 s
D.
2.50 x 10 10 s


24.
Which of the following reactions would also result in the emission

of a positron?
A.
bombardment of with an particle to produce .
B.
decaying to .
C.
which decays to an particle and trtium ( ).
D.
decaying to .


25.
The number of structural isomers for the benzene derivative,
C6H3Br3 (three bromines are substituted for three hydrogens
in the benzene molecule), is,
A.
2
B.
3
C.
4
D.
5


26.
A polyester could be prepared from the condensation polymerization of
                                   
and,
A.
CH3–CH2–OH
B.
HO–CH2–CH2–OH
 
C.
CH2=CH2
D.
Br–CH2–CH2–Br
 
 


27.
The total number of isomers for the halogenated alkene C2Cl2Br2 is:
A.
3
B.
2
C.
4
D.
5


28.
The hybridization of the atomic orbitals for the carbon marked with
an asterisk (*) in    CH3–CH2–*CH=CH–CH3     is:
 
A.
sp
B.
sp3
C.
sp2
D.
sp3d2


29.
Which of the following is the functional group of aldehydes?
A.
B.
C.
D.


30.
The building blocks of proteins are:
A.
Fatty acids.
B.
Amines.
C.
Aldehydes.
D.
Amino acids.
 


31.
Which of the following will form a ketone when oxidized.
A.
A primary alcohol.
B.
A secondary alcohol.
C.
An aldehydyde.
D.
A carboxylic acid.


32.
The IUPAC name for the following compound


is:
A.
3-ethyl-2,2-dimethylpentane
B.
4,4,3-dimethylethylpentane
C.
1,1-dimethyl-2,2-diethylpropane
D.
2,2,3-trimethylpentane


33.
Which of the following statements for the reaction

   N2 (g)     +     3 H2 (g)      ⇌      2 NH3 (g)       ;            ΔH < 0

is false?
 
A.
The reaction is slow because of the high energy needed to break the

: N ≡ N : bond.
B.
A catalyst would increase the equilibrium constant of the reaction.
C.
Raising the temperature would increase the reaction rate.
D.
Raising the temperature would lower the equilibrium constant
 


34.
Use the following molecular orbital diagram,

            

                              

               

            

            

            

to determine which of the following statements is false.
A.
NO is paramagnetic.
B.
The bond order of NO is 2.5.
C.
The bond order of NO+ is 3.0.
D.
NO+ is paramagnetic.


35.
Which of the following statements about group 5A elements

(denoted by the letter M) is false?
A.
In the solid state MX5 (X = F or Cl and M ≠ N) molecules are a mix
octahedral MX6– anions and tetrahedral MX4+ anions.
B.
N, P and As form MX 3 (X = F or Cl) molecules with trigonal
planar structures.
C.
In the gas phase MX5 (X = F or Cl and M ≠ N) molecules have trigonal

bipyramidal structures.
 
D.
Bismuth behaves mostly as a metal.


36.
In which of the following is the hybridization of the atomic orbitals

on sulfur sp3?
A.
SF4
 
B.
SF6
 
C.
S2F10
D.
S2Cl2


37.
Which of the following gaseous molecules is nonlinear?
A.
CO2
B.
BeCl2
C.
SO2
D.
C2H2


38.
The chemical formula of strontium nitride is:
A.
SrN
B.
Sr2N
C.
SrN2
 
D.
Sr3N2


39.
Which of the following elements is a metalloid?
A.
Ge
B.
P
C.
Sn
D.
Pb


40.
Which of the following is ionic?
A.
HCl.
B.
NaH.
C.
H2O.
D.
H atoms absorbed on palladium.


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