KING FAHD UNIVERSITY OF PETROLEUM AND MINERALS
CHEMISTRY DEPARTMENT
CHEM 102-081 FINAL EXAM


TEST CODE NUMBER 001

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 3 hours. Time will be announced after 90 minutes and again 10 minutes before the end of the exam.

Important constants
Gas Constant (R)
= 0.0821
= 8.314
= 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.
The reaction :    2 A   +   B     C   occurs in one step.

If 3.0 moles of A and 2.0 moles of B react in a 1.0 L flask calculate the ratio,

                 
A.
1/18
B.
18/1
C.
1/9
D.
9/1
E.
2/9


2.
The reaction A   +   2 B   +   C     D occurs by the mechanism

                   (1)   A   +   B     X          very fast equilibrium
                   
                   (2)   X   +   C      Y          slow

                   (3)   Y   +   B      D          very fast

What is the rate law for the reaction?        
A.
Rate = k[A] [B]2 [C]
B.
Rate = k[D]
C.
Rate = k [C]
D.
Rate = k [A] [B] [C]
E.
Rate = k [A] [B]


3.
The rate of a reaction at 100 is four times its rate at 30 . The energy of activation of this reaction is:
A.
184
B.
18.6
C.
4.88
D.
8.09
E.
2.16


4.
A first-order reaction
                       A   → products
has a rate constant of . The time required for the concentration of A to drop to 25.0 % of its initial value is:
A.
95.8   s
B.
462    s
C.
231    s
D.
201    s
E.
41.7   s


5.
After 2.0 moles of NH3 were introduced into a 1.0 L container the equilibrium

                   2 NH3 (g)         3 H2 (g)     +     N2 (g)

was reached. Calculate if the equilibrium concentration of NH3 is 1.0 M.      
A.
0.42
B.
0.75
C.
1.0
D.
1.5
E.
1.7  


6.
If the equilibrium,

                   2 N2O (g)     +     N2H4 (g)         3 N2 (g)     +     2 H2O (g)

is moved to a new position by decreasing the volume at constant temperature then,
A.
the number of moles of N2O will increase.
B.
the equilibrium constant will decrease.
C.
the equilibrium constant will increase.
D.
the number of moles of H2O will increase.
E.
the molar concentration of N2H4 will decrease.


7.
What is in kJ for a process with at 25 when it is in a state at which also at
25 .
A.
+ 5.71
B.
10.0
C.
8.31
D.
+ 10.0
E.
+ 8.31


8.
Calculate for,

                            H2O (g)     +     1/2 O2 (g)         H2O2 (g)

using the following information,

                           H2 (g)      +         O2 (g)             H2O2 (g)                  

                         H2 (g)     +       1/2 O2 (g)             H2O (g)                  
           
A.
B.
C.
D.
E.


9.
All of the following are conjugate acid-base pairs EXCEPT:
A.
B.
C.
D.
E.


10.
A 0.10 M solution of B is 1.3 % ionized in water according to the equation,

                                ⇌  

The pH of the solution is:                                
A.
2.9
B.
2.1
C.
11.1
D.
11.9
E.
13.1


11.
Calculate the pH of a 0.014 M NaCN solution.
A.
5.58
B.
3.27
C.
8.42
D.
2.84
E.
10.7


12.
For arsenic acid ,

                                       

Calculate in a 2.0 M arsenic acid solution.          
A.
B.
C.
D.
E.


13.
Calculate the pH after 0.0100 moles HCl were added to a 1.00 L of a solution that is 0.0100 M in HA and 0.0200 M in NaA.
A.
3.68
B.
4.74
C.
5.05
D.
5.35
E.
4.05


14.
Given,

                                    ;        

                          ;        

Calculate the solubility of in 2.0 M aqueous ammonia.
A.
B.
C.
D.
E.


15.
How many moles of will dissolve in 1.0 L of water buffered at pH = 10.86?
A.
B.
C.
D.
E.


16.
For a spontaneous endothermic process
A.
B.
C.
D.
E.


17.
The normal freezing point of ammonia is –78°C. At –80°C and 1 atm the signs of ΔH, ΔS, and ΔG for the process,

NH3(l) → NH3(s)

are:

ΔH      ΔS     ΔG
A.
–        –        0
B.
–        +        –
C.
+        –        +
D.
+        +        0
E.
–        –        –


18.
Use the following table,
        –20.0
10.0
209.0                      
303.9                      

to determine (to the nearest whole number) the temperature above which the vaporization of is spontaneous.
A.
30
B.
316
C.
18
D.
30
E.
43


19.
For a certain process, at 300. K, = - 17.9 kJ and = -7.0 kJ. If the process is carried out reversibly, the amount of useful work that can be performed is
A.
- 24.9 kJ
B.
-7.0    kJ
C.
- 10.9 kJ
D.
- 17.9 kJ
E.
10.9   kJ


20.
Given that,

               Cu2+     +     2 e –     =     Cu          ;      ε°   =   + 0.34 V

            Zn2+    +     2 e –      =     Zn          ;      ε°   =   – 0.76 V

calculate the initial voltage of the cell,

                Zn | Zn2+ (0.0500 M) || Cu2+ (1.000 M ) | Cu
A.
1.14 V
B.
1.18 V
C.
1.10 V
D.
1.02 V
E.
1.06 V


21.
A nickel-cadmium (Nicad) battery involves the discharge reaction,

NiO2 (s)    +    Cd (s)    + 2 H2O (l )    →    Ni(OH)2 (s)    +    Cd(OH)2 (s)

What is the minimum mass of NiO2 that a Nicad battery must contain in order to supply a current of 1.00 ampere for one hour?

A.
0.91 g
B.
1.7   g
C.
2.3   g
D.
4.6   g
E.
9.1   g


22.
The solubility product for CuI(s) is . Given that,

                   Cu+      +      e –    =    Cu                       ;          ε° = 0.52 V

calculate ε° for the half-reaction

                  CuI      +      e –    =    Cu    +    I –            


     
A.
– 0.19 V
B.
+ 0.52 V
C.
– 0.71 V
D.
+ 1.23 V
E.
– 1.23 V


23.
Alpha particles are:
A.
protons.
B.
helium atoms.
C.
hydrogen atoms.
D.
helium nuclei.
E.
electrons.


24.
If 12% of a certain radioisotope decays in 5.2 years, what is the half-life of this isotope?
A.
0.59 yr
B.
1.7 yr
C.
22 yr
D.
28 yr
E.
32 yr


25.
decays to with a half-life of 1.3 × 109 yr. A sample of moon rock was found to contain 78 atoms of for every 22 atoms of . Assuming all comes from the age of the rock is:
A.
8.1 × 10–10 yr
B.
2.4 × 109   yr
C.
2.8 × 109   yr
D.
4.7 × 108   yr
E.
6.8 × 109   yr


26.
The mass of one nucleus is 58.918386 amu. Calculate the binding energy for in units of MeV per nucleon.

Proton () mass = 1.00728 amu,               Neutron () mass = 1.00866 amu,      
1 amu   =                       1 MeV =  
A.
514
B.
8.78
C.
19.0
D.
16.1
E.
7.76


27.
In the complex ion [Co(en)2Br2] + , the oxidation number of Co is:
A.
+1.
B.
+2.
C.
+3.
D.
–2.
E.
–1.


28.
The best name for [Ru(NH3)2(en)](NO3)2 is
A.
(ethylenediamine)diammineruthenium(II) nitrate.
B.
diamminebis(ethylenediamine)ruthenium(III) nitrate.
C.
diammine(ethylenediamine)ruthenium(II) nitrate.
D.
diammine(ethylenediamine)nitratoruthenium(III).
E.
bis(ethylene)diamminenitratoruthenate(II).


29.
The complex [MA2B2]X2 has no geometrical isomers and both A and B are monodentate ligands. The structure of the complex is:
A.
linear.
B.
square planar.
C.
tetrahedral.
D.
octahedral.
E.
pyramidal


30.
Given CN– is a strong-field ligand the number of unpaired electrons in the complex ion [Cr(CN)6]4– is:
A.
0
B.
1
C.
2
D.
3
E.
4


31.
Which of the following ions is diamagnetic.
A.
Fe2+
B.
Sc3+
C.
Cr3+
D.
Cu2+
E.
V2+


32.
A bidentate ligand always
A.
forms bonds to two metal ions.
B.
has a charge of 2+
C.
does not form a coordination compound.
D.
has two donor atoms.
E.
has medical uses.


33.
Organic compounds with the general formula R–O–R (where R is an alkyl group) are called
A.
alkenes.
B.
alcohols.
C.
ethers.
D.
aldehydes.
E.
organic acids.


34.
The reaction of ethylene and water yields
A.
an aldehyde.
B.
an ester.
C.
an alcohol.
D.
an ether.
E.
an organic acid.


35.
The reaction of Cl2 with CH4 to produce methyl chloride (CH3Cl), among other products, is an example of
A.
a free radical reaction.
B.
an addition reaction.
C.
a reduction reaction.
D.
an ester hydrolysis.
E.
polymerization.


36.
Which of the following are isomers with each other? ,

I.      pentane
II.     2-methylbutane
III.    2,3-dimethylbutane
IV. 2,2-dimethylpropane
V.     1-hexene

A.
I, II and IV
B.
I, III and V
C.
I, II and III
D.
IV and V
E.
III and IV


37.
Esters are synthesized by reacting
A.
acids with bases.
B.
amines with alcohols.
C.
alcohols with acids.
D.
amines with alkenes.
E.
alkenes with bases.


38.
Name the following:
             
A.
1-hexyne
B.
2-ethynyl butane
C.
2-ethyl-3-butyne
D.
3-methyl-1-pentyne
E.
3-methyl-4-pentyne


39.
What monomer(s) is (are) needed to make the polymer shown below?


I
HOCH2CH2OH
II
HOOCCH2CH2COOH
III
HOCH2CH2COOH
IV
HOCH = CHOH
V
HOOCCH = CHCOOH
 
A.
II
B.
III
C.
I and II
D.
IV and V
E.
II and III


40.
Identify the secondary amine.
A.
CH3NH2
B.
(CH3)2NH
C.

D.
NH3
E.
(CH3)3N


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