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Bonus Final Exam 3
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1 Calculate the heat of reaction,ΔH 0rxn , for the following reaction as written at 298 K:
CH 4 g  2F 2 g → CF 4 g  2H 2 g
(A) ΔH 0rxn
(B) ΔH 0rxn
(C) ΔH 0rxn
(D) ΔH 0rxn
(E) ΔH 0rxn





substance
CH 4 g CF 4 g
ΔH 0f kJ/mol
−75
−680
203 kJ
−914 kJ
−755 kJ
−605 kJ
302 kJ
2 Consider the combustion of propane:
C 3 H 8 g  5O 2 g → 3CO 2 g  4H 2 Ol
ΔH 0  −2220 kJ
How much heat is liberated when 10.0 g of C 3 H 8 g is burned to produce products at 1
atm pressure?
(A) 23.1 kJ
(B) 503 kJ
(C) 2.2210 4 kJ
(D) 2.22 10 3 kJ
(E) 13.9 kJ
3 What is the P H when 50 mL of 0.10 M HC 2 H 3 O 2 is titrated with 50mL of 0.10 M NaOH?
The K a of HC 2 H 3 O 2 is 1. 8  10 −5 .
(A) P H  9. 26
(B) P H  2. 60
(C) P H  4. 74
(D) P H  1. 48
(E) P H  8. 72
4 Consider the calculated value of K P for the following equilibrium at 249 ∘ C:
2NOg  Cl 2 g  2NOClg;
K P  30. 9
Which of the choices is TRUE for the gas mixture with the partial pressures
P NO  8. 13 atm, P Cl 2  1. 36 atm, and P NOCl  6. 99
atm?
(A) Q  K P and some product will be converted to reactants in order to achieve
equilibrium.
(B) Q  K P and some reactants will be converted to product in order to achieve
equilibrium.
(C) Q  K P and some product will be converted to reactants in order to achieve
equilibrium.
(D) Q  K P and the reaction mixture is at equilibrium.
(E) Q  K P and some reactants will be converted to product in order to achieve
equilibrium.
5 Based on the K a values given which of the acids listed below is the STRONGEST acid?
(A) propionic acid
K a  1. 3  10 −5
(B) benzoic acid
K a  6. 3  10 −5
(C) butanoic acid
K a  1. 5  10 −5
(D) hydrofluoric acid
K a  6. 8  10 −4
(E) lactic acid
K a  1. 4  10 −4
6 The decomposition of CH 3 N 2 CH 3 , shown below, is a first-order reaction with a half life
of 32.1 min at 327 ∘ C. Initially the concentration of CH 3 N 2 CH 3 is 8.9210 −2 M. What is
the concentration after 26.1 min?
CH 3 N 2 CH 3 g → C 2 H 6 g  N 2 g
(A) 5.0810 −2 M
(B) 8.4610 −3 M
(C) 7.2510 −2 M
(D) 1.5710 −1 M
(E) 1.2110 −2 M
7 ΔH 0rxn  −802. 3 kJ for the following reaction, as written, at 298 K:
CH 4 g  2O 2 g → CO 2 g  2H 2 Ol
Which of the following statements is TRUE?
(A) At constant volume, w  -802.3 kJ.
(B) q  - w
(C) At constant volume, q  -802.3 kJ.
(D) Heat flows into the surroundings.
(E) When 2 mol of H 2 Ol is produced ΔH 0rxn  802. 3 kJ.
8 Which of the following compounds, when added to water, will make an acidic solution?
NaCl
NaF
NaC 2 H 3 O 2
NH 4 Cl
(A) Only NaC 2 H 3 O 2 will make an acidic solution.
(B) NaCl and NaF will make acidic solutions.
(C) NH 3 and NaC 2 H 3 O 2 will make acidic solutions.
(D) NaC 2 H 3 O 2 and NH 4 Cl will make acidic solutions.
(E) Only NH 4 Cl will make an acidic solutions.
9 Choose the selection which lists the following acids in order of INCREASING acid
strength (weakest acid first).
HClO 2
HClO 3
HClO 4
HIO 2
HBrO 2
(A) HClO 2  HClO 3  HClO 4  HBrO 2  HIO 2
(B) HClO 4  HClO 3  HClO 2  HBrO 2  HIO 2
(C) HClO 2  HClO 3  HClO 4  HIO 2  HBrO 2
(D) HClO 2  HBrO 2  HIO 2  HClO 3  HClO 4
(E) HIO 2  HBrO 2  HClO 2  HClO 3  HClO 4
10 Consider the following equilibrium for which ΔH 0rxn  180. 74 kJ
N 2 g  O 2 g  2NOg
Which of the following shifts the equilibrium toward products?
(A) adding a catalyst
(B) decreasing volume
(C) raising the temperature
(D) adding nitrogen monoxide
(E) removing nitrogen
11 How many milliliters of 0.235 M HIO 4 are needed to titrate 64.5 mL of 0.212 M NaOH to
the equivalence point?
(A) 58.2 mL
(B) 17.2 mL
(C) 71.5 mL
(D) 3.2 mL
(E) 1.3 mL
12 Give the following reactions:
N 2 g  2O 2 g → 2NO 2 g
2NOg  O 2 g → 2NO 2 g
ΔH 0rxn  66. 4 kJ
ΔH 0rxn  −114. 2 kJ
Calculate the standard enthalpy of reaction for the reaction: N 2 g O 2 g →2NOg.
(A) ΔH 0rxn  −47. 8 kJ
(B) ΔH 0rxn  47. 8 kJ
(C) ΔH 0rxn  −180. 6 kJ
(D) ΔH 0rxn  180. 6 kJ
(E) ΔH 0rxn  90. 3 kJ
13 Arrange the following species in order of DECREASING OXIDIZING strength
(strongest oxidizing agent first):
F 2 g
(A) O 2
(B) F 2
(C) F 2
(D) H 
(E) MnO −4
MnO −4
MnO −4
O2
Fe 2
O2
O 2 g
F2
O2
Fe 2
Fe 2
F2
2
Fe aq
H
H
MnO −4
O2
H
−
MnO 4 aq

H aq
Fe 2
Fe 2
H
MnO −4
Fe 2
14 When a hot lava rock is dropped into 100 g of water at 25.0 ∘ C the rock releases 4.97 kJ of
heat to the water. What is the final temperature of the water?
The specific heat of water is 4.18 J/(g 0 C).
(A) 27.4 ∘ C
(B) 59.0 ∘ C
(C) 36.9 ∘ C
(D) 11.9 ∘ C
(E) 29.8 ∘ C
15 Consider the following reaction: 2NOg 2H 2 g →N 2 g 2H 2 Og.
Use the following data to determine the rate law for this reaction.
(A) Rate  k NO
2
(B) Rate  k NO
1/2
(C) Rate  k NO
2
Exp
NO
1
0.0126
0.0125
0.24
2
0.0252
0.0250
1.90
3
0.0252
0.0125
0.96
H2
0
H2
0
Initial Rate M/s
2
H2
H2
(D) Rate  k NO
H2
(E) Rate  k NO
H2
2
16 A mixture consisting of 100g of solid sodium hydroxide, 100g of solid sodium hydrogen
carbonate, and 2.5 atm of carbon dioxide is placed
into a sealed 1.00-L steel reaction vessel. This mixture is heated to 700 K and allowed to
come to equilibrium according to the following
reaction:
NaOHs  CO 2 g  NaHCO 3 s;
K p  2. 5
What is the equilibrium partial pressure of carbon dioxide?
(A) 3.010 −1 atm
(B) 1.910 −1 atm
(C) 4.010 −1 atm
(D) 3.7 atm
(E) 2.5 atm
17 The overall cell reaction for the ELECTROLYSIS shown below is:
Cd 2 aq Cus →Cdg Cu 2 aq
Which of the following statements is FALSE?
(A) The mass of the Cds electrode will increase during the electrolysis.
(B) The mass of the Cus electrode will decrease during the electrolysis.
(C) The copper electrode is the anode and the cadmium electrode is the cathode.
(D) Cations migrate from the salt bridge into the 1.0 M Cu 2 solution.
(E) Electrons flow from the copper electrode to the cadmium electrode.
18 Consider the redox reaction shown below. Which element is REDUCED during the course
of the reaction?
2KMnO 4 aq 10KIaq 16HClaq →2MnCl 2 aq 5I 2 s 12KClaq 10H 2 Ol
(A) Mn
(B) O
(C) I
(D) Cl
(E) H
19 Using data in the standard reduction potentials table at the front of this exam calculate the
value of ΔG 0rxn for the reaction shown below.
−

2
2MnO 4 − aq  10I aq  16H aq → 2Mn aq  5I 2 s  8H 2 Ol
(A) ΔG 0rxn
(B) ΔG 0rxn
(C) ΔG 0rxn
(D) ΔG 0rxn
(E) ΔG 0rxn





−93. 6 kJ
936 kJ
1978 kJ
−1978 kJ
−936 kJ
20 Calculate the P H of a solution prepared by dissolving 0.37 mol of hypochlorous acid
HClO and 0.23 mol of sodium hypochlorite NaOCl
in water with a total volume of 1.00 L of solution.
The K a of hypochlorous acid is 3.010 −8 .
(A) P H  6. 48
(B) P H  4. 19
(C) P H  8. 38
(D) P H  7. 32
(E) P H  7. 73
21 Calculate ΔG 0rxn for the reaction shown below at 1000 K given the following data.
(Assume that ΔH 0rxn and ΔS 0rxn do not depend on temperature.)
2NO 2 g → N 2 O 4 g
NO 2 g N 2 O 4 g
ΔH 0f
kJ/mol
S 0 J/mol  K
33.9
9.66
240.5
304.3
Which of the following statements is CORRECT if all gases are present at 1 atm of
pressure?
(A) ΔG 0rxn  118. 6 kJ; this reaction favors reactants.
(B) ΔG 0rxn  −1. 77  10 5 ; this reaction favors reactants.
(C) ΔG 0rxn  0; this reaction is at equilibrium.
(D) ΔG 0rxn  −118. 6 kJ; this reaction favors products.
(E) ΔG 0rxn  1. 77  10 5 kJ; this reaction favors products.
22 Using the energy diagram below calculate the activation energy for the REVERSE
reaction.
(A) E a rev
(B) E a rev
(C) E a rev
(D) E a rev
(E) E a rev





54 kJ/mol
24 kJ/mol
30 kJ/mol
74 kJ/mol
94 kJ/mol
23 A layer of chromium is electroplated onto an automobile bumper by passing a constant
current of 200.0 A through a cell that contains Cr NO 3 3 aq. How many minutes are
required to deposit 125g of chromium?
(A) 129 min
(B) 3480 min
(C) 6.44 min
(D) 58.0 min
(E) 19.3 min
24 For a process to be spontaneous it MUST be true that...
(A) heat is transferred from the system to the surroundings.
(B) both the enthalpy and the entropy of the system decrease.
(C) the Gibbs free energy of the system decreases and S univ increases.
(D) the entropy change of the system is zero.
(E) the entropy change of the system is positive.
25 Consider the following equilibrium, for which K p  1. 49  10 8 at 373 K
COg  Cl 2 g  COCl 2 g
In an equilibrium mixture of the three gages, P CO P Cl2  8. 60  10 −4 atm. The partial
pressure of the product COCl 2 is
atm.
(A) 4. 96  10 −15 atm
(B) 1. 10  10 2 atm
(C) 2. 01  10 14 atm
(D) 1. 72  10 11 atm
(E) 1. 28  10 5 atm
26 Calculate the P H of a 2.16 M solution of NaF.
The K a for HF is 6. 8  10 −4 .
(A) P H  2. 16
(B) P H  5. 24
(C) P H  10. 83
(D) P H  8. 75
(E) P H  0. 33
27 Calculate the OH − aqconcentration of a solution with a P H of 9.30.
−
(A) OH  5. 0  10 −10 M
(B)
(C)
(D)
(E)
−
OH  5. 0  10 4 M
−
OH  6. 7  10 −1 M
−
OH  2. 0  10 −5 M
−
OH  9. 3  10 −1 M
28 What is the P H of a solution made by dissolving 15.1 g of acetic acid, HC 2 H 3 O 2 , in
enough water to make 100 mL of solution? The K a of HC 2 H 3 O 2 is 1. 8  10 −5 .
(A) P H  0. 61
(B) P H  2. 17
(C) P H  4. 72
(D) P H  2. 71
(E) P H  3. 70
29 Balance the following redox reaction in ACIDIC solution with the smallest possible
whole-number coefficients:
−
2
ClO 4 aq  Mn aq → Cl 2 g  MnO 2 s
What is the coefficient in front of H  aq when this reaction is balanced?
(A) 2
(B) 4
(C) 6
(D) 8
(E) 12
30 K p  6. 64  10 −58 for the following reaction:
3O 2 g  2O 3 g
Which of the following are TRUE?
(i) At equilibrium, P O 2 P O 3 .
(ii) At equilibrium, P O 2 P O 3 .
(iii) At equilibrium, DECREASING the volume will shift the equilibrium toward
REACTANT.
(iv) At equilibrium, INCREASING the volume will shift the equilibrium toward
REACTANT.
(A) (ii) and (iv) are true.
(B) (ii) and (iii) are true.
(C) (i) and (iv) are true.
(D) Only (i) is true.
(E) (i) and (iii) are true.
31 Consider the following reaction:
4NH 3 g  O 2 g → 2N 2 H 4 g  2H 2 Og
At 298 K, ΔH 0rxn  −108. 08 kJ and ΔS 0rxn  −120. 34 J/K. Calculate the value of K P for
this reaction at 436 K. Assume that ΔH 0rxn and ΔS 0rxn do not depend on temperature.
(A) K P  1. 02
(B) K P  2. 17  10 −7
(C) K P  4. 60  10 6
(D) K P  5. 33  10 −7
(E) K P  4. 56  10 12
32 Consider the combustion of propylene:
2C 3 H 6 g  9O 2 g → 6CO 2 g  6H 2 Og
If oxygen is consumed at the rate of 0.11 M/s by this reaction, what is the rate of
production of carbon dioxide?
(A) 5.9 M/s.
(B) 0.66 M/s.
(C) 0.073 M/s.
(D) 0.038 M/s.
(E) 0.17 M/s.
33 Calculate the concentration of iodide ions in a saturated solution of lead II iodide. The
solubility product constant of PbI 2 is K sp  1. 4  10 −8 .
(A) 3. 8  10 −4 M
(B) 1. 5  10 −3 M
(C) 3. 5  10 −9 M
(D) 3. 0  10 −3 M
(E) 1. 4  10 −8 M
34 Which of the following statements about collision theory in kinetics is FALSE for the
following elementary reaction?
Ag  Bg → Productsg
(A) High temperatures do not speed up reaction rates.
(B) Not every collision results in reaction.
(C) Molecules with E much less than E a have a low probability of reaction.
(D) The orientation of the collision affects the probability of reaction.
(E) The more frequently molecules collide with one another during a chemical reaction,
the greater the reaction rate.
35 Which CORRECTLY indicates the signs of the enthalpy change and the entropy change
for the process shown below?
Nas → Nal
(A) ΔH 0
(B) ΔH 0
(C) ΔH 0
(D) ΔH 0
(E) ΔH 0





0 and ΔS 0
0 and ΔS 0
0 and ΔS 0
0 and ΔS 0
0 and ΔS 0





0
0
0
0
0