Chemistry 116: General Chemistry
Syracuse University Project Advance
Final Exam, Spring 2007
Name
Date
The last page of this exam is a periodic Table
[Gas constant = 8.314J/mol K; 1 faraday = 96,500 J/V mol e- ]
1. Which of the reactants and/or products do not appear in the properly written Kc expression
for the heterogeneous reaction
NiCO3 (s) + 2H+ (aq)  Ni+2 (aq) + CO2 (g) + H2O (l) ?
A
B.
C.
D.
E.
NiCO3 (s)
CO2 (g) + H2O (l)
H+ (aq) and Ni+2 (aq)
CO2 (g)
NiCO3 (s) and H2O (l)
2. What is the pH of a 0.25 M solution of HNO2 (Ka = 4.0  10-4)?
A.
B.
C.
D.
E.
1.70
2.00
2.30
2.70
3.70
3. Given that Ksp = 1.0  10-12 for AgSCN (silver thiocyanate), what is its molar solubility?
A.
B.
C.
D.
E.
2.0  10-12 M
1.0  10-10 M
2.0  10-10 M
1.0  10-6 M
2.0  10-6 M
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Spring 2007 Final Exam
4. The average rate of disappearance of ozone in the reaction 2O3 (g) 
 3O2 (g) was found to
be 7.0  10-3 atm/sec over a certain time interval. What is the rate of appearance of O2 during
this interval?
A.
B.
C.
D.
E.
1.0  10-2 atm/sec
7.0  10-3 atm/sec
5.0  10-3 atm/sec
3.0  10-3 atm/sec
2.0  10-3 atm/sec
5. When 47 Be undergoes electron capture, what nuclide is produced?
A. 63 Li
7
 B. 36 Li
C. 5 B
D. 75 B

E. 126 C



6. Which statement is true?

A. Exothermic reactions are always spontaneous.
B. Free energy is independent of temperature.
C. At constant P and T, a decrease in free energy ensures an increase in the entropy of the
system.
D. A reaction that exhibits a negative value of S cannot be spontaneous.
E. None of the above statements is true.
7. The oxidation state of H in CaH2 is
A.
B.
C.
D.
E.
+2
+1
0
-1
-2
8. Suppose the reaction 2 CO(g) <======> CO2(g) + C(s) is already at equilibrium. If we
increased the pressure on the system
A. the reaction shifts to the left (more reactants)
B. the reaction shifts to the right (more products)
C. the reaction is unaffected.
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Spring 2007 Final Exam
9. For the reaction A + B C, the following data were obtained. What is the rate law?
Experiment
1
2
3
4
5
A.
B.
C.
D.
E.
[A]o
0.10
0.20
0.20
0.30
0.30
[B]o
0.20
0.20
0.30
0.30
0.50
Initial Rate (M/sec)
0.03
0.059
0.060
0.089
0.091
Rate = k[A]
Rate = k[B]
Rate = k[A][B]
Rate = k[A]2[B]
Rate = k[A][B]2
10. A solution that is formed by combining 400 mL of 0.30 M NaOH with 500 mL of 0.060 M
HCl has a pH of
A.
B.
C.
D.
E.
1.0
2.0
3.0
5.0
7.0
11. Consider the following reaction, and assume ideal gas behavior:
2NOBr(g)
2NO(g) + Br2(g)
A 1.0-L vessel was initially filled with pure NOBr to 4.0 atm. After equilibrium was
established at 300K, the partial pressure of NOBr was 2.5 atm. What is Kp for the reaction?
A.
B.
C.
D.
E.
0.18
0.27
0.45
0.54
0.75
12 Given the following equation:
CO2(g) + C(s) <========> 2 CO(g)
with Kc = 14.0 at 800° C
The equilibrium constant at 800° C
A.
B.
C.
D.
favors reactants
favors products
favors neither
can’t determine from the given data
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Spring 2007 Final Exam
13. 2-Ethylheptane is not a standard IUPAC name. The correct name for this compound is
A.
B.
C.
D.
E.
3-ethylheptane.
2-pentylbutane.
3-pentylbutane.
2-methyloctane.
3-methyloctane.
14. For the reaction
3C(s) + 4H2(g)
C3H8(g)
S˚ = 269 J/(mol.K)
H˚ = 103.8 kJ/mol
Calculate the equilibrium constant at 25oC for the reaction above.
A.
B.
C.
D.
E.
7.2  10-5
1.0
1.4  104
1.0  1017
3.7  1019
15 The equilibrium constant, Kp, for the reaction 2HgO (s)  2Hg (l) + O2 (g) is 1.2 x 10-30.
Calculate the Kp for the reaction :
½ O2 (g) + Hg (l)  HgO (s)
A.
B.
C.
D.
E.
9.1 x 1014
8.3 x 1029
1.1 x 10-15
–1.1 x 1015
4.2 x 1029
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Spring 2007 Final Exam
16. Which of the following is/are not a true statement?
(1) NH3 (aq) ( NH4OH (aq) ) is a base according to the Arrhenius, Bronsted-Lowrey and
Lewis Concepts of acids and bases.
(2) The Bronsted-Lowrey conjugate acid to OH- (regarded as base) is H2O.
(3) In the following reaction: HPO42- + NH4+<======> H2PO4- + NH3, H2PO4- is a
Bronsted-Lowrey base.
A.
B.
C.
D.
E.
1
2
2 and 3
1 and 3
3
17. The most stable allotrope of oxygen is
A.
B.
C.
D.
E.
O2
O3
H2O
H2O2
Fe2O3
18. The fusion reaction below has been of great interest as a potential energy source. How much
energy is released in the fusion of one mole each of deuterium and tritium? (The speed of
light is 2.9979 m/s. The masses of the atoms and neutron are shown below.)
2
1

H
2.0140
amu
A.
B.
C.
D.
E.

3
1
H
3.01605
amu

4
2
He
4.002603
amu

1
0
n

energy
1.008665
amu
56.3 J
5.63  108 J
8.44  1011 J
1.69  1012 J
7.84  1044 J
19. What is the concentration of H3O+ in a solution of 0.075 M KOH at 25° C?
A.
B.
C.
D.
E.
0.075 M
0.150 M
1.33 x 10-13 M
6.66 x 10-14 M
none of the above
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Spring 2007 Final Exam
20. At 760K, acetaldehyde decomposes to carbon monoxide and methane.
CH3CHO CH4 + CO
A plot of ln[CH3CHO] versus time was found to be linear, and it took 530 s for [CH3CHO] to
decrease from an initial value of 0.10 M to 0.050 M. The rate law for the reaction is
A.
B.

C.

D.

E.
[CH 3CHO]
 530[CH 3CHO]
t
[CH 3CHO]
 530[CH 3CHO]2
t
[CH 3CHO]
 265[CH 3CHO]2
t
[CH 3CHO]
1.9 103[CH 3CHO]2
t
[CH 3CHO]
1.3 103[CH 3CHO]
t

 21. What is the reducing agent in the following reaction?
3Cl2(g) + 2OH-(aq) + 2CrO42-(aq) + 2H2O(l) 6ClO-(aq) + 2Cr(OH)3(s)
A.
B.
C.
D.
E.
Cl2
OHCrO42H2O
ClO-
22. What is the minimum concentration of Mg2+ that is needed to begin the formation of a
precipitate of Mg(OH)2 in a aqueous solution of pH = 10.0? (Ksp of Mg(OH)2 = 6 x 10-12).
A.
B.
C.
D.
E.
3 x 10-8 M
3 x 10-4 M
1.5 x 10-4 M
6 x 10-8 M
6 x 10-4 M
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Spring 2007 Final Exam
23. Which of the following mixtures is a buffer solution? (OAc = acetate ion shorthand C2H5O2 )
A.
B.
C.
D.
E.
10 mL of 1 M NaOH + 10 mL of 1 M HCl
10 mL of 1 M NaOAc + 10 mL of 1 M NaCl
10 mL of 1 M NaOH + 10 mL of 1 M HOAc
10 mL of 1 M HOAc + 10 mL of 1 M NaOAc
10 mL of 1 M HOAc + 20 mL of 1 M HCl
24. What is the pH of a 0.10 M NH3 solution? (Ka = 5.6  10-10 for NH4+.)
A.
B.
C.
D.
E.
8.87
9.37
9.71
11.13
11.63
25. The heat of fusion of acetic acid is 11.5 kJ/mol. Its melting point is 16.6˚C. The change in
entropy for the melting of acetic acid in J/(mol K) is (Hint: FLM)
A.
B.
C.
D.
E.
-11.5
11.5
15.1
39.7
694
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Spring 2007 Final Exam
26. Given the following standard electrode potentials:
Reaction
E°
Li+ <======> Li
Cr3+ <======> Cr
Cu2+ <======> Cu
-3.05
-0.740
0.337
Which one of the reactions below will proceed spontaneously from left to right?
(equations below are not necessarily balanced)
A. Cu + Li+ ------> Cu2+ + Li
B. Cr3+ + Cu2+ ------> Cr + Cu
C. Cr + Cu2+ ------> Cr3+ + Cu
D. Cu + Cr3+ ------> Cu2+ + Cr
E. None of the above
27. How many grams of copper metal can be obtained by passing a current of 12 amps through a
solution of CuSO4 for 15 minutes?
A.
B.
C.
D.
E.
0.016 g
3.6 g
7.1 g
14 g
none of these
28. The reaction, 2A + B C, has the following proposed mechanism:
Step 1: A + B
D (fast equilibrium)
Step 2: D + B E (slow)
Step 3: E + A C + B (fast)
If this mechanism is correct, the anticipated rate law is
A.
B.
C.
D.
E.
Rate = k[A]
Rate = k[A][B]
Rate = k[A]2[B]
Rate = k[A][B]2
Rate = k[A]2[B]2
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Spring 2007 Final Exam
29. Which of the following equations represents the Haber process?
A.
B.
C.
D.
E.
2H2 + O2 2H2O
2NO2 + 7H2 2NH3 + 4H2O
Fe2O3 + 2Al 2Fe + Al2O3
Fe2O3 + 3H2 2Fe + 3H2O
3H2 + N2 2NH3
30. A sample of wood from an Egyptian mummy case was measured to have a 14C count of 9.4
cpm/gC (counts per minute per gram of carbon). How old is the wood? (The half-life of 14C
is 5730 years, and the 14C count of living wood is 15.3 cpm/gC.)
A.
B.
C.
D.
E.
2210 years
3520 years
4030 years
4570 years
6400 years
31. Given the reduction potentials,
Au3+ + 3e-  Au
Ni2+ + 2e-  Ni
E˚ = +1.50 V
E˚ = -0.23 V
What is G˚ at 25˚C for the reaction:
2Au3+ + 3Ni  2Au + 3Ni2+
A.
B.
C.
D.
E.
-5.00  102 kJ/mol
5.00  102 kJ/mol
-1.00  103 kJ/mol
1.00  103 kJ/mol
2.14  103 kJ/mol
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Spring 2007 Final Exam
32. Consider the following system at equilibrium:
H2(g) + I2(s) + 68.0 kJ/mol
2HI(g)
Which of the following will shift the equilibrium to the right?
1. increasing the temperature
2. decreasing the temperature
3. increasing the volume
4. decreasing the volume
5. removing some HI(g)
6. adding some HI(g)
7. removing some I2(s)
8. adding some I2(s)
A.
B.
C.
D.
E.
1, 3, 5
2, 6, 7
1, 5, 8
1, 3, 5, 8
2, 4, 6, 7
33. On the weak acid/strong base titration curve shown, identify the equivalence point and a
point corresponding to a buffer.
e
pH
f
d
b
c
a
volume of base
A.
B.
C.
D.
E.
equivalence point
c
d
b
b
d
buffer
a
b
e
f
f
34. Calcium carbonate reacts with hydrochloric acid to produce which gas?
A.
B.
C.
D.
E.
H2
O2
Cl2
CO
CO2
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Spring 2007 Final Exam
35. List, in order (i) through (iv), the functional group for each of the following compounds:
(i)
H3 C
C
C
H2
C
H2
CH 3
(iii) HO
C
H
C
CH3
O
O
(ii) H3 C
C
H2
C
H2
CH 3
OH
(iv) H
C
C
H2
CH3
O
(1) alcohol
(2) aldehyde
(3) amide
(4) carboxylic acid
(5) ester
(6) ether
(7) ketone
A.
B.
C.
D.
E.
2,1,3,7
7,2,3,6
7,1,4,2
5,6,4,2
3,1,5,2
36. Which of the following fundamental particles has the largest mass?
A.
B.
C.
D.
E.
beta
gamma
proton
neutron
alpha
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Spring 2007 Final Exam