CHEM 1515
Exam V
John V. Gelder
December 14, 1993
Name ________________________
TA's Name ________________________
Lab Section ________________________
INSTRUCTIONS:
1. This examination consists of a total of 15 different
pages. The last umpteen pages include a whole heck of
alot of important mathematical equations, constants and
tables. All work should be done in this booklet. You
may carefully remove the last 5 pages of the
examination.
2. PRINT your name, your TA's name and your laboratory
section now in the space at the top of this sheet. DO
NOT SEPARATE THE PAGES.
3. Answer all questions that you can and whenever called
for show your work clearly. Your method of solving
problems should pattern the approach used in lecture.
You do not have to show your work for the multiple
choice or short answer questions.
4. No credit will be awarded if your work is not shown in
problems 2 – 6. Please circle your final answer!
5. Point values are shown next to the problem number.
6. Budget your time for each of the questions. Some
problems may have a low point value yet be very
challenging. If you do not recognize the solution to a
question quickly, skip it, and return to the question after
completing the easier problems.
7. Look through the exam before beginning; plan your
work; then begin.
8. R e l a x and do well.
SCORES
Page 2
Page 3
Page 4
Page 5
Page 6
TOTAL
_____
(19)
_____
(24)
_____
(20)
_____
(24)
_____
(63)
______
(150)
CHEM 1515 Exam V – F93
(9)
Page 2
1. Write the chemical formula(s) of the product(s) and balance the following reactions. Identify the phase
of each product as either (g)as, (l)iquid, (s)olid or (aq)ueous. Soluble ionic compounds should be
written in the form of their component ions.
a)
HC9H7O4(aq)
b)
C3H8(g)
c)
Al(s)
+ NaOH(aq) →
+ O2(g) →
+ Fe2O3(s) →
(10) 2. Balance the following oxidation-reduction reaction using the half-reaction method.
a)
H2O2(aq) + Cr(OH)3(s) → CrO42–(aq) basic solution
identify the oxidizing agent ________
identify the reducing agent ________
CHEM 1515 Exam V – F93
Page 3
(24) 3. The rate constant for the second order decomposition of NOBr
2NOBr(g) → Br2(g) + 2NO(g)
is 1.41 x 10–5 mm Hg–1·s–1 at 10 ˚C. A sample of NOBr at a pressure of 250 mm Hg is placed in a
flask at this temperature and sealed.
a) What will be the pressure of NOBr in the flask after 100 seconds?
b) Assuming there is no NO or Br2 in the container initially, calculate the total pressure in the flask
after 100 seconds?
c) How much time has elapsed when the total pressure in the flask is 350 mm Hg?
CHEM 1515 Exam V – F93
Page 4
(20)4a. Exactly 1 liter of a buffer solution contains 0.400 mol (CH 3)3N, trimethylamine, and 0.500 mol of
(CH3)3NHCl. Calculate the pH of the buffer solution.
b) Calculate the new pH if 0.0500 mol of hydrochloric acid, HCl, are added to the buffer solution in part
a).
CHEM 1515 Exam V – F93
Page 5
(14)5a. The mole fraction of ethylene glycol, C2H6O2, in a particular ethylene glycol–water solution
is equal to 0.03125. Determine the mass of ethylene glycol in 3.785 L (1 gallon) of this
solution if the density of the solution is 1.012 g·mL–1.
b. ethylene glycol dissolves in water. Draw a Lewis structure for ethylene glycol which supports this
experimental fact.
(10)6a. Write the half-reactions and determine the products of the reaction when a piece of sodium metal is added
to water at 25 ˚C.
b)
Is the reaction spontaneous or nonspontaneous? Briefly explain your answer. (Note: You may show
a calculation to support your conclusion.)
c)
If a piece of sodium with a mass 1.00 g is added to 100 mL of water, estimate the pH of the resulting
solution.
CHEM 1515 Exam V – F93
Page 6
Multiple Choice: (63 points)
Print the letter (A, B, C, D, E) which corresponds to the answer selected.
7. ________
8. ________
9. ________
10. ________
11.
________
12. ________
13. ________
14. ________
15. ________
16.
________
17. ________
18. ________
19. ________
20. ________
21.
________
22. ________
23. ________
24. ________
25. ________
26.
________
27. ________
ONLY THE ANSWERS IN THE AREA ABOVE WILL BE GRADED. Select the most correct answer
for each question. Each question is worth 3 points.
7. ∆G˚ for the reaction
BaO(s) + CO2(g) → BaCO3(s)
is – at 25 ˚C. Which of the following statements is true?
A)
B)
C)
D)
The reaction remains spontaneous at higher temperatures.
The reaction becomes nonspontaneous at higher temperatures.
The reaction is spontaneous at all temperatures.
There is not enough information to answer this question.
8. The standard entropy of formation, ∆S˚f of H2O(l) is
J
A) 70 K
J
B) 406 K
J
C) –163 K
J
D) –266 K
9. A hydrochloric acid solution is 38.0% by mass and it is also 12.5 M. Calculate the density of the
solution.
A)
B)
C)
D)
0.835 g·mL–1
1.04 g·mL–1
1.20 g·mL–1
1.31 g·mL–1
10. For the half-reaction
2H+(aq) (1.00 x 10–7 M) +2e– → H2(g) (1.00 atm)
Ecell is
A) +0.829 v
B) –0.829 v
C) +0.414 v
D) –0.414 v
CHEM 1515 Exam V – F93
Page 7
11. Which of the following compounds has the greater solubility in water?
A)
B)
C)
D)
H3C–CH2–CH3
CCl4
CH2Cl2
CH3CH2OH
12. Which of the following solutions will have the lowest freezing point?
A)
B)
C)
D)
0.100 M CaCl2
0.100 M NaCl
0.100 M C6H12O6
0.100 M NH4NO3
13. Which of the following mathematical relationships would be used to determine the time required for 30%
of a reactant to decompose in the first order reaction;
A(g) → products
1.20
A) t = k
0.357
B) t = k
2.33
C) t = k·[A
0]
0.428
D) t = k·[A ]
0
14. In the following reaction
aA(g) + bB(g) → cC(g) + dD(g)
1.00 mol of A is mixed with 2.00 mol of B in a 1.00 L container at a given temperature. After 10 minutes
the concentration of all species were found to be;
after 10 min
[A]
0.875 M
[B]
1.81 M
[C]
0.0625 M
[D]
0.250 M
The balanced chemical equation must be;
A)
B)
C)
D)
2A(g) + 3B(g) → C(g) + 4D(g)
A(g) + 2B(g) → C(g) + D(g)
A(g) + 2B(g) → C(g) + 4D(g)
2A(g) + B(g) → C(g) + D(g)
15. Increasing the temperature in an endothermic reaction will
A)
B)
C)
D)
E)
increase both the rate of the reaction and the magnitude of the equilibrium constant.
increase the rate of the reaction and decrease the magnitude of the equilibrium constant.
decrease the rate of the reaction and increase the magnitude of the equilibrium constant.
decrease both the rate of the reaction and the magnitude of the equilibrium constant.
increase the rate and have no affect on the equilibrium constant.
CHEM 1515 Exam V – F93
Page 8
16. Which of the following statements is true?
A) The half-life of a second order reaction is independent of the initial concentration of the reactant.
B) The decay of many radioactive elements follows second order kinetics.
C) When a plot of [reactant] versus time is a straight line the rate constant can be determined from the yintercept.
D) The units for the rate constant of a first and a second order reaction are different.
17. Which of the following statements is true?
A) The activation energy is the minimum energy required for a reaction to occur.
B) The number of collisions per second between molecules in the gas phase is independent of temperature.
C) The activation energy can be determined knowing the difference in energy of the reactants and the
products in a chemical reaction.
D) The activation energy is generally smallest for exothermic reactions.
18. Which of the following statements is true?
A) Bimolecular elementary reactions are less common compared to termolecular elementary reactions in
most mechanisms.
B) Intermediates in chemical reactions are short-lived species which initially appear as a product in a multistep reaction mechanism.
C) The overall rate law for a chemical reaction must be identical to the rate law for the fastest elementary
step in a multi-step mechanism.
D) A catalyst never appears in the elementary step(s) of a mechanism because by definition it is not
consumed in the reaction.
19. Which of the following reactions has the most positive value of ∆S˚?
A)
B)
C)
D)
2Mg(s) + CO2(g) → 2MgO(s) + C(s)
NH3(g) + HCl(g) → NH4Cl(s)
6Li(s) + N2(g) → 2Li3N(s)
CaSO4·2H2O(s) → CaSO4(s) + 2H2O(g)
20. A reaction rate for a particular reaction triples when the temperature is raised from 17 ˚C to 37 ˚C. The
activation energy is,
J
A) 287 mol
kJ
B) 20 mol
kJ
C) 41 mol
kJ
D) 57 mol
21. A solution which is 0.0100 M piperidine (C5H10NH2) has a pH of 11.53. Calculate Kb for piperidine.
A)
B)
C)
D)
1.13 x 10–3
1.70 x 10–3
3.36 x 10–3
2.95 x 10–12
CHEM 1515 Exam V – F93
Page 9
22. The mechanism,
Step 1)
Step 2)
NO2(g) + NO2(g) → NO3(g) + NO(g)
NO3(g) + CO(g) → NO2(g) + CO2(g)
(slow)
(fast)
has been proposed for the reaction
NO2(g) + CO(g) → NO(g) + CO2(g)
Based on this mechanism the expected rate law is,
A)
B)
C)
D)
rate = k[NO2]1[CO]1
rate = k[NO2]2[CO]0
rate = k[NO3]1[CO]1
rate = k[NO2]2[CO]1
23. Which of the following solutions is acidic?
A)
B)
C)
D)
0.100 M HCN/0.100 M NaCN
0.100 M NH3/0.900 M NH4NO3
0.100 M C5H5N/0.100 M C5H5NHCl
0.100 M HBrO/0.900 M NaBrO
(Ka for HCN = 4.9 x 10-10)
(Kb for NH3 = 1.8 x 10-5)
(Kb for C5H5N = 1.7 x 10-9)
(Ka for HBrO = 2.0 x 10-9)
24. Which of the following salts, when dissolved in water, produces a acidic solution?
A)
B)
C)
D)
(CH3)3NHCl
NaIO3
Na2CO3
KCl
25. Which is the strongest acid?
A)
B)
C)
D)
0.100 M H2SO3
(Ka1 = 1.7 x 10-2 Ka2 = 6.4 x 10-8)
0.100 M HF (Ka = 7.2 x 10-4)
0.100 M H3PO4
(Ka1 = 7.5 x 10-3 Ka2 = 6.2 x 10-8 Ka3 = 4.2 x 10-13)
0.100 M H3BO3
(Ka = 5.8 x 10-10)
26. Which of the following titrations has the highest equivalence point pH?
A)
B)
C)
D)
100.0 mL of 0.500 M HCl and 0.400 M NaOH
40.0 mL of 0.400 M HBr and 0.300 M (CH3)2NH
35.0 mL of 0.900 M HF and 0.450 M NaOH
30.0 mL of 0.800 M HCN and 0.600 M NaOH
27. Rank the pure substances NF3, F2, NaF and HF in terms of increasing strength of attractive forces
A)
B)
C)
D)
NaF < F2 < NF3 < HF
NF3 < F2 < HF < NaF
F2 < NF3 < HF < NaF
HF < F2 < NaF < NF3
CHEM 1515 Exam V – F93
Page 10
Useful Information
Equations
Constants
PV = nRT
L·atm
R = 0.0821 mol·K = 8.314
Psolution = χsolventP˚solvent
density of H2O = 1.00
∆T = ikm
kf(H2O) = 1.86
∆H˚rxn = ∑(∆Hf˚(products)) – ∑(∆Hf˚(reactants))
˚C
m
J
mole.K
g
cm3
˚C
kb(H2O) = 0.512 m
∆S˚rxn = ∑(S˚(products)) – ∑(S˚(reactants))
∆G˚rxn = ∑(∆Gf˚(products)) – ∑(∆Gf˚(reactants))
∆G˚ = ∆H˚ - T∆S˚
∆G˚ = –RT ln K
∆G = ∆G˚ + RT ln Q
J
F = 96,500 volt · mol = 96,500 coulombs
∆G˚ = –nFE˚
0.0257
ln Q
n
0.059
Ecell = E˚ –
n log Q
E 1
k
1
ln k1 = Ra  T - T 
1
 2
 2
[A]
ln [A] t  = -kt
 o
Ecell = E˚ –
0.0257
ln K
n
0.059
E˚ = n log K
E˚ =
1
1
[A]t [A]o = kt
Kp = Kc(RT)∆n
x1,2 =
–b± b 2 – 4ac
for ax2 + bx + c = 0
2a
pH = –log[H+]
pH + pOH = 14
Kw = 1.0 x 10–14
CHEM 1515 Exam V – F93
Periodic Table of the Elements
IA
1
VIIIA
1
2
H
He
1.008
3
2
Page 11
IIA
IIIA IVA VA VIA VIIA 4.00
4
Li Be
6.94 9.01
11
12
3
Na Mg
22.99 24.30
19
20
4
5
6
7
5
6
7
8
9
10
B
C
N
O
F
Ne
10.81 12.01 14.01 16.00 19.00 20.18
13
14
15
16
17
18
IIIB IVB VB VIB VIIB
21
22
K Ca Sc Ti
23
24
25
VIII
26
27
IB
28
29
Al
Si
P
S
Cl Ar
31
32
33
34
35
IIB 26.98 28.09 30.97 32.06 35.45 39.95
30
36
V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
39.10 40.08 44.96 47.88 50.94 52.00 54.94 55.85 58.93 58.69 63.55 65.38 69.72 72.59 74.92 78.96 79.90 83.80
37
38
39
40
41
42
43
44
45
46
47
48
49
50
51
52
53
54
Rb Sr
Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
I
Xe
85.47 87.62 88.91 91.22 92.91 95.94 (98) 101.1 102.9 106.4 107.9 112.4 114.8 118.7 121.8 127.6 126.9 131.3
55
56
57
72
73
74
75
76
77
78
79
80
81
82
83
84
85
86
Cs Ba La Hf Ta W Re Os Ir
Pt Au Hg Tl Pb Bi Po At Rn
132.9 137.3 138.9 178.5 180.9 183.8 186.2 190.2 192.2 195.1 197.0 200.6 204.4 207.2 209.0 (209) (210) (222)
87
88
89 104 105 106 107 108 109
Fr Ra Ac Rf Db Sg Bh Hs Mt
(223) 226.0 227.0 (261) (262) (263) (262) (265) (266)
58
Lanthanides
59
60
61
62
63
64
65
66
67
68
69
70
71
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
140.1 140.9 144.2 (145) 150.4 152.0 157.2 158.9 162.5 164.9 167.3 168.9 173.0 175.0
90
91
92
93
94
95
96
97
98
99 100 101 102 103
Actinides
Th Pa
U
Np Pu Am Cm Bk Cf Es Fm Md No Lr
232.0 231.0 238.0 237.0 (244) (243) (247) (247) (251) (252) (257) (258) (259) (260)
CHEM 1515 Exam V – F93
Page 12
E.1 DISSOCIATION CONSTANTS FOR ACIDS AT 25 ˚C
Name
Formula
Ka1
HC2H3O2
Arsenic
H3AsO4
1.8 x 10– 5
8.0 x 10– 3
5.6 x 10– 3
Arsenous
Benzoic
Boric
Butyric acid
Carbonic
Cyanic
Citric
H3AsO3
HC7H5O2
H3BO3
HC4H7O2
H2CO3
HCNO
H3C6H5O7
6.0
6.5
5.8
1.5
4.3
3.5
7.4
Formic
Hydroazoic
Hydrocyanic
Hydrofluoric
Hydrogen chromate ion
Hydrogen peroxide
Hydrogen selenate ion
Hydrogen sulfate ion
Hydrogen sulfide
Hypobromous
Hypochlorous
Hypoiodus
Iodic
Lactic
Malonic
Oxalic
HCHO2
HN3
HCN
HF
HCrO4–
H2O2
HSeO4–
HSO4–
H2S
HBrO
HClO
HIO
HIO3
HC3H5O3
H2C3H2O4
H 2C 2O 4
1.8
1.9
4.9
7.2
3.0
2.4
2.2
1.2
5.7
2.0
3.0
2.0
1.7
1.4
1.5
5.9
Nitrous
Phenol
Phosphoric
Paraperiodic
Propanoic
Pyrophosphoric
Selenous
Sulfuric
Sulfurous
Tartaric
HNO2
HC6H5O
H3PO4
H5IO6
HC3H5O2
H4P2O
H2SeO3
H2SO4
H2SO3
H2C4H4O6
Acetic
Ascorbic
E.2
HC6H7O6
10–10
10– 5
10–10
10– 5
10– 7
10– 4
10– 4
x 10– 4
x 10– 5
x 10–10
x 10– 4
x 10– 7
x 10–12
x 10– 2
x 10– 2
x 10– 8
x 10– 9
x 10– 8
x 10–11
x 10– 1
x 10– 4
x 10– 3
x 10– 2
x 10– 4
x
x
x
x
x
x
x
4.5
1.3 x 10–10
7.5 x 10– 3
2.8 x 10– 2
1.4 x 10– 5
3.0 x 10– 2
2.3 x 10– 3
strong acid
1.7 x 10– 2
1.0 x 10–3
Ka2
Ka3
1.0 x 10– 7
3.0 x 10–12
5.6 x 10–11
1.7 x 10– 5
4.0 x 10– 7
1.3 x 10–13
2.0 x 10– 6
6.4 x 10– 5
6.2 x 10– 8
5.3 x 10– 9
4.4
5.3
1.2
6.4
4.6
x
x
x
x
x
4.2 x 10–13
10– 3
10– 9
10– 2
10– 8
10– 5
DISSOCIATION CONSTANTS FOR BASES AT 25˚C
Name
Ammonia
Aniline
Dimethylamine
Ethylamine
Hydrazine
Formula
NH3
C6H5NH2
(CH3)2NH
C2H5NH2
H2NNH2
1.8
4.3
5.4
6.4
1.3
Kb
x 10– 5
x 10–10
x 10– 4
x 10– 4
x 10– 6
Name
Hydroxylamine
Methylamine
Pyridine
Trimethylamine
Formula
HONH2
CH3NH2
C5H5N
(CH3)3N
Kb
1.1 x 10– 8
4.4 x 10– 4
1.7 x 10– 9
6.4 x 10– 5
CHEM 1515 Exam V – F93
E. 3
Page 13
SOLUBILITY-PRODUCT CONSTANTS FOR COMPOUNDS AT 25˚C
Name
Formula
Barium carbonate
Barium chromate
Barium Fluoride
Barium hydroxide
Barium oxalate
Barium phosphate
Barium sulfate
Cadmium carbonate
Cadmium hydroxide
Cadmium sulfide
Calcium carbonate
Calcium chromate
Calcium fluoride
Calcium hydroxide
Calcium phosphate
Calcium sulfate
Cerium(III) fluoride
Chromium(III) fluoride
Chromium(III) hydroxide
Cobalt(II) carbonate
Cobalt(II) hydroxide
Cobalt(III) hydroxide
Copper(I) bromide
Copper(I) chloride
Copper(I) sulfide
Copper(II) carbonate
Copper(II) chromate
Copper(II) hydroxide
Copper(II) phosphate
Copper(II) sulfide
Gold(III) chloride
Iron(II) carbonate
Iron(II) hydroxide
Iron(II) sulfide
Iron(III) hydroxide
Lanthanum fluoride
Lanthanum iodate
Lead carbonate
Lead chloride
Lead chromate
Lead fluoride
Lead hydroxide
Lead sulfide
Magnesium hydroxide
Magnesium oxalate
Manganese carbonate
Mercury(I) sulfide
Mercury(II) sulfide
Silver sulfide
Strontium fluoride
BaCO3
BaCrO4
BaF2
Ba(OH)2
BaC2O4
Ba3(PO4)2
BaSO4
CdCO3
Cd(OH)2
CdS
CaCO3
CaCrO4
CaF2
Ca(OH)2
Ca3(PO4)2
CaSO4
CeF3
CrF3
Cr(OH)3
CoCO3
Co(OH)2
Co(OH)3
CuBr
CuCl
Cu2S
CuCO3
CuCrO4
Cu(OH)2
Cu3(PO4)2
CuS
AuCl3
FeCO3
Fe(OH)2
FeS
Fe(OH)3
LaF3
La(IO3)3
PbCO3
PbCl 2
PbCrO4
PbF 2
Pb(OH)2
PbS
Mg(OH)2
MgC2O4
MnCO3
Hg2S
HgS
Ag2S
SrF2
Ksp
5.1 x 10-9
1.2 x 10-10
1.0 x 10-6
5 x 10-3
1.6 x 10-7
3.4 x 10-23
1.1 x 10-10
5.2 x 10-12
2.5 x 10-14
8.0 x 10-27
2.8 x 10-9
7.1 x 10-4
3.9 x 10-11
5.5 x 10-6
2.0 x 10-29
9.1 x 10-6
8 x 10-16
6.6 x 10-11
6.3 x 10-31
1.4 x 10-13
1.6 x 10-15
1.6 x 10-44
5.3 x 10-9
1.2 x 10-6
2.5 x 10-48
1.4 x 10-10
3.6 x 10-6
2.2 x 10-20
1.3 x 10-37
6.3 x 10-36
3.2 x 10-25
3.2 x 10-11
8.0 x 10-16
6.3 x 10-18
4 x 10-38
7 x 10-17
6.1 x 10-12
7.4 x 10-14
1.6 x 10-5
2.8 x 10-13
2.7 x 10-8
1.2 x 10-15
8.0 x 10-28
1.8 x 10-11
8.6 x 10-5
1.8 x 10-11
1.0 x 10-47
4.0 x 10-53
6.3 x 10-50
2.5 x 10-9
CHEM 1515 Exam V – F93
Page 14
Table of Standard Reduction Potentials (25 ˚C)
CHEM 1515 Exam V – F93
Page 15
A. Acidic Solution
Eo(V)
Li+ + e– → Li(s)
K+ + e– → K(s)
–3.045
–2.925
Ba2+ + 2e– → Ba(s)
Sr2+ + 2e– → Sr(s)
–2.906
Ca2+ + 2e– → Ca(s)
Na+ + e– → Na(s)
–2.866
Mg2+ + 2e– → Mg(s)
H2(g) + 2e– → 2H–
Al3+ + 3e– → Al(s)
Mn2+ + 2e– → Mn(s)
–2.363
Zn2+ + 2e– → Zn(s)
Cr3+ + 3e– → Cr(s)
–0.763
Fe2+ + 2e– → Fe(s)
Cr3+ + e– → Cr2+
–0.440
Cd2+ + 2e– → Cd(s)
PbSO4(s) + 2e– → Pb(s) + SO42–
PbCl2(s) + 2e– → Pb(s) + 2Cl–
Ni2+ + 2e– → Ni(s)
Sn2+ + 2e– → Sn(s)
Pb2+ + 2e– → Pb(s)
2H+ + 2e– → H2(g)
S(s) + 2H+ + 2e– → H2S(aq)
Sn4+ + 2e– → Sn2+
–2.888
–2.714
–2.25
–1.662
–1.185
–0.744
–0.408
–0.403
–0.359
–0.268
–0.250
MnO4– + 8H+ + 5e– → Mn2+ + 4H2O(l)
2HClO(aq) + 2H+ + 2e– → Cl2(g) + 2H2O(l)
HClO2(aq) + 2H+ + 2e– → HClO(aq) + H2O(l)
H2O2(aq) + 2H+ + 2e– → 2H2O(l)
S2O 82– + 2e– → 2SO42–
O3(g) + 2H+ + 2e– → O2(g) + H2O(l)
F2(g) + 2e– → 2F–
F2(g) + 2H+ + 2e– → 2HF(aq)
~1.2
1.21
1.229
0.83
1.23
1.29
1.33
1.360
1.455
1.498
1.51
1.63
1.645
1.776
2.00
2.07
2.87
3.06
–0.136
–0.126
0.000
0.142
0.15
Sb2O3(s) + 6H+ + 6e– → 2Sb(s) + 3H2O(l)
Cu2+ + e– → Cu+
0.152
SO42– + 4H+ + 2e– → H2SO3(aq) + H2O(l)
AgCl(s) + e– → Ag(s) + Cl–
0.172
Cu2+ + 2e– → Cu(s)
SO42– + 8H+ + 6e– → S(s) + 4H2O(l)
H2SO3(aq) + 4H+ + 4e– → S(s) + 3H2O(l)
I2(s) + 2e– → 2I–
MnO4– + e– → MnO42–
[PtCl6]2– + 2e– → [PtCl4]2– + 2Cl–
O2(g) + 2H+ + 2e– → H2O2(aq)
Fe3+ + e– → Fe2+
Pt2+ + 2e– → Pt(s)
ClO3– + 3H+ + 2e– → HClO2(aq) + H2O(l)
O2(g) + 4H+ + 4e– → 2H2O(l)
O2(g) + 4H+(pH = 7) + 4e– → 2H2O(l)
MnO2(s) + 4H+ + 2e– → Mn2+ + 2H2O(l)
2HNO2(aq) + 4H+ + 4e– → N2O(g) + 3H2O(l)
Cr2O72– + 14H+ + 6e– → 2Cr3+ + 7H2O(l)
Cl2(g) + 2e– → 2Cl–
PbO2(s) + 4H+ + 2e– → Pb2+ + 2H2O(l)
Au3+ + 3e– → Au(s)
0.153
0.222
0.337
0.357
0.450
0.536
0.564
0.68
0.682
0.771
Hg2+ + 2e– → Hg(l)
0.788
Ag+ + e– → Ag(s)
2NO3– + 4H+ + 2e– → N2O4(g) + 2H2O(l)
2Hg2+ + 2e– → Hg22+
NO3– + 4H+ + 3e– → NO(g) + 2H2O(l)
Pd2+ + 2e– → Pd(s)
Br2(l) + 2e– → 2Br–
Br2(aq) + 2e– → 2Br–
ClO4– + 2H+ + 2e– → ClO3– + H2O(l)
2IO3– + 12H+ + 10e– → I2(s) + 6H2O(l)
0.799
0.803
0.920
0.96
0.987
1.065
1.087
1.19
1.195
Eo(V)
B. Alkaline Solution
Mg(OH)2(s) + 2e– → Mg(s) + 2OH–
Al(OH)3(s) + 3e– → Al(s) + 3OH–
Zn(OH)2(s) + 2e– → Zn(s) + 2OH–
Fe(OH)2(s) + 2e– → Fe(s) + 2OH–
2H2O(l) + 2e– → H2(g) + 2OH–
2H2O(l) + 2e– → H2(g) + 2OH–(pH = 7)
Cd(OH)2(s) + 2e– → Cd(s) + 2OH–
Ni(OH)2(s) + 2e– → Ni(s) + 2OH–
Fe(OH)3(s) + e– → Fe(OH)2(s) + OH–
2S(s) + 2e– → S22Cu2O(s) + H2O(l) + 2e– → 2Cu(s) + 2OH–
CrO42– + 4H2O(l) + 3e– → Cr(OH)3(s) + 5OH–
MnO2(s) + 2H2O(l) + 2e– → Mn(OH)2(s) + 2OH–
NO3– + H2O(l) + 2e– → NO2– + 2OH–
HgO(s) + H2O(l) + 2e– → Hg(l) + 2OH–
PbO2(s) + H2O(l) + 2e– → PbO(s) + 2OH–
ClO3– + H2O(l) + 2e– → ClO2– + 2OH–
ClO4– + H2O(l) + 2e– → ClO3– + 2OH–
O2(g) + 2H2O(l) + 4e– → 4OH–
NiO2(s) + 2H2O(l) + 2e– → Ni(OH)2(s) + 2OH–
MnO4– + 2H2O(l) + 3e– → MnO2(s) + 4OH–
BrO3– + 3H2O(l) + 6e– → Br– + 6OH–
ClO– + H2O(l) + 2e– → Cl– + 2OH–
O ( )
H O(l)
2
O ( )
2OH
–2.690
–2.30
–1.245
–0.877
–0.828
–0.43
–0.809
–0.72
–0.56
–0.447
–0.358
–0.13
–0.05
0.01
0.098
0.247
0.33
0.36
0.401
0.490
0.588
0.61
0.89
1 24
CHEM 1515 Exam V – F93
Page 16
CHEM 1515 Exam V – F93
Page 17
Thermodynamic Values (25 ˚C)
o
o
Substance
∆H f
and State
kJ
 mol

∆G f
kJ
 mol

Carb o n
C(s) (graphite)
C(s) (diamond)
CO(g)
CO2(g)
CH4(g)
CH3OH(g)
CH3OH(l)
H2CO(g)
HCOOH(g)
HCN(g)
C2H2(g)
C2H4(g)
CH3CHO(g)
C2H5OH(l)
C2H6(g)
C3H6(g)
C3H8(g)
0
2
-110.5
-393.5
?
-201
-239
-116
-363
135.1
227
52
-166
-278
-84.7
20.9
-104
0
3
-137
-394
-51
-163
-166
-110
-351
125
209
68
-129
-175
-32.9
62.7
-24
Bromine
Br2(l)
BrCl(g)
0
14.64
0
-0.96
∆H f
 . J 
K mol
and State
kJ
 mol

∆G f
kJ
 mol

6
2
198
214
186
240
127
219
249
202
201
219
250
161
229.5
266.9
270
Nitrogen
N2(g)
NCl3(g)
NF3(g)
NH3(g)
NH3(aq)
NH2CONH2(aq)
NO(g)
NO2(g)
N2O(g)
N2O4(g)
N2O5(g)
N2H3CH3(l)
HNO3(aq)
HNO3(l)
NH4Cl(s)
NH4ClO4(s)
0
230
-125
?
?
?
90
32
82
10
-42
54
-207
-174
-314
-295
0
271
-83.6
-17
-27
?
87
52
104
98
134
180
-111
-81
-201
-89
Silver
Ag(s)
Ag+(aq)
Ag(S2O3)3-(aq)
AgBr(s)
AgCl(s)
0
105.6
-1285.7
-100.4
-127.1
0
77.1
--96.9
-109.8
42.6
72.7
-107.1
96.2
152.
240
0
-23
0
7
223
121
-167
-92
-131
-95
57
187
Fluorine
F2(g)
F-(aq)
HF(g)
0
-333
-271
0
-279
-273
203
-14
174
Magnesium
Mg(s)
Mg(aq)
MgO(s)
Oxygen
O2(g)
O(g) 249
O3(g)
0
203
0
-230
-286
-242
0
115
0
-157
-237
-229
o
Substance
Chlorine
Cl 2 (g)
Cl2(aq)
Cl-(aq)
HCl(g)
Hydrogen
H2(g)
H(g) 217
H+(aq)
OH-(aq)
H2O(l)
H2O(g)
o
So
131
0
-11
70
189
0
-492
-601
0
-456
-569
33
-118
26.9
0
232
143
0
161
163
205
239
So
 . J 
K mol
192
-137
-139
193
111
174
211
240
220
304
178
166
146
156
95
186
Sulfur
S(rhombic)
SO2(g)
SO3(g)
H2S(g)
0
-296.8
-395.7
-20.17
0
-300.2
-371.1
-33.0
31.8
248.8
256.3
205.6
Titanium
TiCl4(g)
TiO2(s)
-763
-945
-727
-890
355
50
Aluminum
AlCl3(s)
-526
-505
184
Barium
BaCl2(aq)
-872
Ba(OH)2·8H2O(s) -3342
-823
-2793
123
427
Iodine
I2(s)
HI(g)
0
25.94
0
1.30
116.7
206.3