KING FAHD UNIVERSITY OF PETROLEUM AND MINERALS
CHEMISTRY DEPARTMENT
CHEM-102-081-SECOND MAJOR 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 20 multiple choice questions and the time allowed is 80 min (1 hr.and 20 min). Time will be announced after 40 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 values for CO2(g) , H2O(l) and C2H2(g) are –394.4, –237.2 and 209.2 , respectively. The free energy for the reaction
               
                                       2 C2H2(g)   +   5 O2(g)        4 CO2(g)    +    2 H2O(l)

is:
A.
–4720
B.
–2470
C.
–3740
D.
–1580
E.
–1682


2.
For the reaction,

                                         

the equilibrium constant at is . The free energy of formation () of COCl2 at is :

(The free energy of formation of CO at is )
.
A.
 
B.
C.
D.
.0
E.


3.
In which of the following processes is the entropy change negative?
A.
2 KClO4(s) → 2 KClO3(s) + O2(g)
B.
H2O(g) → H2O(l)
C.
2 Na(s) + 2 H2O(l) → 2 NaOH(aq) + H2(g)
D.
N2(g) → 2 N(g)
E.
NH4Cl (s) → NH3 (g) + HCl (g)


4.
Ammonium nitrate dissolves spontaneously and endothermically in water. Which of the following statements is correct for this process?
A.
Both ΔH and ΔS are positive.
B.
Both ΔH and ΔS and negative.
C.
ΔH is negative; ΔS is positive.
D.
ΔH is positive; ΔS is negative.
E.
is positive at all temperatures.


5.
For the reaction,

2 Fe (s)   +   3/2 O2 (g)   +   3 H2O (l)   →   2 Fe(OH)3 (s)      ;    = –790.5

at and 1 atm. the following data are given.
Substance
Fe(OH)3 (s)
Fe (s)
O2 (g)
H2O (l)
107
27
205
70  

Calculate in . (Hint: )
A.
0.27
B.
2.3
C.
0.36
D.
2.7
E.
3.6


6.
Which of the following is true for the galvanic cell

Zn(s)  Zn2+(aq)  Cr3+(aq)  Cr(s)    
A.
The electrons flow from the cathode to the anode.
B.
The electrons flow from the zinc electrode to the chromium electrode.
C.
The electrons flow from the chromium electrode to the zinc electrode.
D.
Chromium is oxidized.
E.
Zinc is reduced.


7.
Given the standard reduction potentials,

      = V
   = +1.090 V

Calculate E at for the galvanic cell

Cr (s) | Cr3+ (aq, 0.20 M) || Br2 (aq, 0.50 M) , Br– (aq, 0.10 M) | Pt (s)


A.
1.760 V
B.
1.824 V
C.
1.838 V
D.
1.888 V
E.
2.208 V


8.
Calculate the solubility product of silver iodide at 25°C given the following data:
 
E˚(V)
AgI(s) + e– → Ag(s) + I–
 
–0.15
 
 
 
Ag+ + e– → Ag(s)
 
+0.80
 
A.
2.9 × 10–3
B.
1.9 × 10–4
C.
2.1 × 10–12
D.
8.7 × 10–17
E.
2.4 × 10–24


9.
Electrolysis of a molten salt MCl, using a current of 3.86 amp for 16.2 min, deposits 1.52 g of the metal M. Identify the metal.
A.
Li
B.
Na
C.
K
D.
Rb
E.
Ca


10.
Calculate the potential of the of the following concentration cell (as it is written) at 25°C.

Ni (s) | Ni2+ (aq, 1.00 x10–4 Μ) || Ni2+ (aq, 1.00 Μ) | Ni (s)
A.
–0.368   V
B.
+0.132   V
C.
–0.132   V
D.
+0.118   V
E.
+0.0591 V


11.
The best name for K[Cr(NH3)2Cl2SO4] is
A.
potassium diamminedichlorosulfatochromium(III).
B.
potassium diamminedichlorosulfatochromate(II).
C.
potassium diamminedichlorochromatium(III) sulfate.
D.
potassium diamminedichlorochromate(II) sulfate.
E.
potassium diamminedichlorosulfatochromate(III).


12.
The ion [Co(NH3)6]2+ is octahedral and high spin. This complex is
A.
paramagnetic, with 1 unpaired electron.
B.
paramagnetic, with 3 unpaired electrons.
C.
paramagnetic, with 4 unpaired electrons.
D.
paramagnetic, with 5 unpaired electrons.
E.
diamagnetic.


13.
Which of the following complexes can exhibit optical isomerism? (en = H2NCH2CH2NH2 and is bidentate)
A.
cis–Co(NH3)4Cl2
B.
trans–Co(en)2Br2
C.
cis–Co(en)2Cl2
D.
Co(NH3)3Cl3
E.
trans–Co(NH3)2Cl4


14.
Hemoglobin is a complex of
A.
Co3+
B.
Mg2+
C.
Fe2+
D.
Sc3+
E.
Fe3+


15.
Calculate the energy change when one mole of Polonium-214 decays according to the equation

   

Atomic masses: Pb-210 = 209.98284, Po-214 = 213.99519 and He-4 = 4.00260 .
A.
8.78 × 1014     J/mol
B.
–7.20 × 1014   J/mol
C.
–8.78 × 1011   J/mol
D.
–9.75 × 10–3   J/mol
E.
1.46 × 10–9     J/mol


16.
The missing missing product in this nuclear reaction,



is:
A.
B.
C.
D.
E.


17.
What fraction of radioactive atoms remains in a sample after 3 half-lives?
A.
1/12
B.
1/6
C.
1/16
D.
1/2
E.
1/8


18.
A bone sample produces 5.22 disintegrations per minute per gram Carbon (d min–1 gC–1). Given that living organisms produce 15.3 d min–1 gC–1 calculate the age of the bone.
(for is 5730 years)    
A.
yr
B.
yr
C.
yr      
D.
yr
E.
yr


19.
Iron-56 () has a binding energy of 8.79 MeV per nucleon. Determine the difference in mass between one mole of iron-56 nuclei and the component nucleons of which it is made. ()  
A.
B.
C.
D.
E.


20.
In the coordination compound [Co(en)2Cl2]Cl, the coordination number and oxidation number of the central atom are, respectively,
A.
4, +3.
B.
6, +2.
C.
4, +2.
D.
6, +3.
E.
4, +1.


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