1413.001 CHEM - Final Exam Dec. 14, 2011
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CHEM 1413.001 - Final Exam December 14, 2011
Constants:
R = 0.082 L-atm/mol-K
R = 8.31 J/mol-K
NA = 6.02x1023 mol-1
c = 3.00x108 m/s
h = 6.63x10-34 J-s
1 amu = 1.66x10-24 g
Conversion Factors: 1 atm. = 760 torr
1 = 1x10-8 cm
Molar Masses: H - 1.
1 L = 1.06 Qt.
C - 12.
N - 14.
Mg(NO3)2 - 148.3
Al - 27.
O - 16.
Al2O3 - 102.
HCl - 36.5
AlCl3 - 133.5
KBr - 119.
C4H10 - 58.
Na - 23.
H2O - 18.
CH3OH - 32.
CH3OCH3 - 46.
CH3CH2CH2CH3 - 58. CH3CH2CH3 - 44.
Ni(CO)4 - 170.7
SO2 - 64.1
C2H6 - 30.
FeS2 - 120.
Clausius-Clapeyron Equation:
H vap
P
ln vap ,2
Pvap ,1
R
C3H8 - 44.
1 1
T2 T1
CHEM 1413.001 - Final Exam Dec. 14, 2011
(65)
MULTIPLE CHOICE (Circle the ONE correct answer)
1. A density of 25 g/m3 = ____ mg/cm3 ?
(A) 2.5x10-10
(B) 2.5x10-2
(C) 2.5x102
(D) 2.5x104
2. The density of potassium is 0.86 g/mL. What is the volume, in Quarts (Qt.) of
0.50 kg of potassium?
(A) 0.62 Qt.
3. A
(B) 0.55 Qt.
(D) 6.1x10-4 Qt.
(C) 0.45 Qt.
227
Ra2+ ion contains how many neutrons (n) and electrons (e)?
(A) 227 n & 86 e (B) 139 n & 90 e (C) 86 n & 139 e (D) 139 n & 86 e
4. What is the formula of copper(I) nitrite?
(A) CuNO2
(B) Cu(NO2)2
(C) CuNO3
(D) Cu2NO2
5. Which one of the following formulas is incorrect?
(A) MgSO3
(B) Ga3(PO4)2
(C) LiCO3
(D) (NH4)2S
6. The half-life for the decay of 14C is 5730 years. A piece of clothing from an
archaeological dig is 18% as much 14C as a piece of modern clothing.
Therefore, the age of this piece of clothing is approximately:
(A) 8,600 years (B) 10,300 years
(C) 14,200 years
(D) 19,400 years
H
H
structural formula to the right is:
(A) 2-hexanol
(B) 2-heptanol
H
H
H
O
H
C
C
C
C
C
C
H
7. The name of the compound with the
H
H
H
H
H
H
(C) 5-hexanol
H
(D) 5-hexanone
8. The name of the compound with the condensed structural formula,
CHCCHFCH2F , is
(A) 3,4-fluoro-1-butene
(B) 3,4-difluoro-1-butyne
(C) 1,2-difluoro-3-butyne
(D) 3,4-difluoro-1-butene
9. How many grams of Mg(NO3)2 contain a total of 3x1024 atoms?
(A) 740 g
(B) 6650 g
(C) 494 g
(D) 82 g
10. When 50. grams of a compound containing Aluminum (Al) (and other elements)
is burned completely in O2(g), 19.0 grams of Al2O3(s) is produced. Therefore, the
percent (by mass) of Aluminum in this compound is approximately:
(A) 8.4%
(B) 10%
(C) 20%
(D) 38%
11. A compound contains 25.9% Nitrogen (N) and 74.1% Oxygen (O) by mass.
What is the empirical formula of this compound?
(A) N2O5
(B) NO2
(C) NO3
(D) N3O7
For #12-#15: Consider the reaction: 2 Al + 6 HCl 2 AlCl3 + 3 H2.
12. What is the theoretical yield of AlCl3 when 146 grams of HCl are reacted with an
excess of Al ?
(A) 49 g
(B) 178 g
(C) 534 g
(D) 1602 g
13. When 135 grams of Al are reacted with 219 grams of HCl, what is the theoretical
yield of AlCl3 ?
(A) 148 g
(B) 186 g
(C) 668 g
(D) 267 g
14. When 135 grams of Al are reacted with 219 grams of HCl, ____ grams of
___ remain when the reaction is complete.
(A) 81 g , Al
(B) 32 g , HCl
(C) 54 g, Al
(D) 81 g , HCl
15. When 292 grams of HCl reacts with an excess of Al, 125 grams of AlCl3 are
formed. The percent yield is:
(A) 16%
(B) 35%
(C) 43%
(D) 71%
16 For the reaction, 4 Al + 3 O2 2 Al2O3, the percent yield is 60%. How many
moles of O2 (reacted with an excess of Al) are required to produce 9 moles of
Al2O3?
(A) 13.5 mol
(B) 15.0 mol
(C) 22.5 mol
(D) 10.0 mol
17. Consider the reaction, ___ P(s) + __ Br2(g) ___ PBr3(s). When 12 moles of
P(s) are reacted with 9 moles of Br2(g), it is found that 3 moles of PBr3(s) are
produced. Therefore, the percent yield for this reaction is:
(A) 25%
(B) 33%
(C) 50%
(D) 67%
18. The oxidation number of chromium (Cr) in MgCr2O7 is
(A) +6
(B) +7
(C) +12
(D) +14
19. Regarding the reaction, I2O5(s) + 5 CO(g) I2(s) + 5 CO2(g), which of the
following statements is/are true?
(1) I2O5 is the oxidizing agent
(3) CO is oxidized
(A) 1 & 2
(B) 1 & 3 & 4
(2) I2 is oxidized
(4) I2O5 is reduced
(C) 1 & 4
(D) All four statements
20. How many grams of KBr are contained in 300 mL of 0.85 M KBr?
(A) 18.7 g
(B) 340 g
(C) 42.0 g
(D) 30.3 g
21. What is the Molarity of a solution prepared by mixing 200 mL of 0.60 M KCl to
500 mL of 0.20 M KCl?
(A) 0.42 M
(B) 0.31 M
(C) 0.24 M
(D) 0.16 M
22. What volume of 0.60 M H2SO4 is needed to completely neutralize 300 mL of
0.80 M NaOH?
(A) 200 mL
(B) 400 mL
(C) 225 mL
(D) 800 mL
23. Consider the reaction:
____K3PO4(aq) + ____Mg(NO3)2 ____Mg3(PO4)2(s) + ____KNO3(aq)
When 2.0 L of 0.50 M K3PO4(aq) is mixed with 2.0 L of 0.50 M Mg(NO3)2(aq),
how many moles of Mg3(PO4)2(s) will precipitate?
(A) 0.40 mol
(B) 0.50 mol
(C) 0.33 mol
(D) 0.60 mol
24. For butane, C4H10, the enthalpy of vaporization is 22.4 kJ/mol and the specific
heat capacity is 1.9 J/g-oC. How much heat is required to vaporize 29 g of liquid
C4H10 at its boiling point (Tb = 0 oC) and heat the gas to 75 oC?
(A) 15.3 kJ
(B) 4.14 kJ
(C) 7.1 kJ
(D) 4140 kJ
25. Consider the reaction of sodium with water:
2 Na(s) + 2 H2O(l) 2 NaOH(aq) + H2(g)
Ho = -240 kJ
The enthalpy of fusion of H2O(s) is 6.0 kJ/mol
When 92 grams of Na is dropped into a container of ice water at 0 oC, how many
grams of ice will melt?
(A) 720 g
(B) 2880 g
(C) 80 g
(D) 1440 g
26. Consider the reaction:
2 CH3OH(l) + 3 O2(g) 2 CO2(g) + 4 H2O(l)
H = -1450 kJ
What is H for the production of 16. g of CH3OH from CO2 and H2O
(A) -363 kJ
(B) -725 kJ
(C) +363 kJ
(D) +725 kJ
27. Consider the combustion of 3 moles of liquid benzene:
3 C6H6(l) + 22 O2(g) 18 CO2(g) + 9 H2O(l) Ho = -9813 kJ
From this value plus the Enthalpies of Formation of CO2(g) [-394 kJ/mol] and
H2O(l) [-286 kJ/mol], one can determine that the Enthalpy of Formation of liquid
benzene is:
(A) -147 kJ/mol
(B) +49 kJ/mol
(C) +147 kJ/mol
(D) -294 kJ/mol
28. From the following thermochemical equations,
2 H2O(g) 2 H2(g) + O2(g)
H= +484 kJ
H= +286 kJ
2 O3(g) 3 O2(g)
H for the reaction, 3 H2(g) + O3(g) 3 H2O(g), is
(A) -583 kJ
(B) -341 kJ
(C) +583 kJ
(D) +869 kJ
29. The energy of the H-H bond in H2 is 436 kJ/mol. What is the maximum
wavelength (in nm) of radiation that can be absorbed by H2 ?
(A) 2.75x10-7 nm
(B) 110 nm
(C) 242 nm
(D) 275 nm
30. A stellar object is emitting photons with a wavelength of 130 nm. In a given
period of time, a detector has captured photons with a total energy of 0.015 J.
How many photons have been captured?
(A) 9.8x106
(B) 9.8x1015
(C) 9.8x1024
(D) 5.8x1020
31. The condensed electron configuration of Sn (Z=50) is
(A) [Kr]5s24d105p2
(B) [Kr]5s25p2
(C) [Kr]5s25d105p2
(D) [Kr]4d104p4
32. Of the four atoms, Na, Mg, P and S, ___ has the most unpaired electrons and
____ has the least unpaired electrons.
(A) S , Na
(B) P , Na
(C) S , Mg
(D) P , Mg
33. Of the four Ge, atoms, Ca, S, Si, ____ has the smallest radius and ____ has the
lowest first ionization energy.
(A) Ca , S
(B) S , Ge
(C) S , Ca
(D) Si , Ca
34. Rank the following atoms in order of decreasing First Ionization Energy?
Ca , Sr , Rb , Ge
(A) Rb>Sr>Ca>Ge
(B) Ge>Ca>Sr>Rb
(C) Rb>Ge>Ca>Sr
(D) Ge>Ca>Rb>Sr
35. Arrange the following in order of increasing phosphorus-sulfur Bond Lengths:
PS2-1 , PS+1 , PS-1
(A) PS -1 < PS-1 < PS+1
2
(B) PS+1 < PS-1 < PS2-1
(C) PS-1 < PS+1 < PS2-1
(D) PS+1 < PS2-1 < PS-1
36. In the molecular ion, SF3-1, the molecular geometry is _______ and the ion is
_______:
(A) SeeSaw , Polar
(B) Trigonal Pyramidal , Polar
(C) T-Shaped , Polar
(D) Trigonal Planar , Non-Polar
37. In the molecular ion TeCl42- , the hybridization of the central atom is ____ and the
molecular geometry is ______.
(A) sp3 , tetrahedral
(C) sp3d2 , octahedral
(B) sp3d , see-saw
(D) sp3d2 , square planar
38. In the molecular ion, XeF5+1, the molecular geometry is _______ and the ion is:
(A) SeeSaw , Polar
(B) Trigonal Bipyramidal , Non-Polar
(C) Square Pyramidal , Polar
(D) Octahedral , Polar
39. In the molecule, TeBr2 , the hybridization of the central atom is ______ and the
Br-Te-Br bond angle is _______.
(A) sp2 , 120o
(B) sp3d , 180o
(C) sp3 , 109.5o
(D) sp , 180o
-1
40. In the molecular ion, PS3 , the hybridization of the central atom is _____ and the
molecular geometry is:
(A) sp2 , Trigonal Planar
(B) sp2 , Trigonal Pyramidal
(C) sp3d , Trigonal Bipyramidal
(D) sp3 , Tetrahedral
41. In the molecular ion NS2-1, the hybridization of the central atom is ____ and the
electron pair geometry is ____.
(A) sp3 , tetrahedral
(C) sp2 , bent
(B) sp2 , trigonal planar
(D) sp , linear
42. In the molecule CH2CHNH2 the hybridization of the second carbon (closer to
right) is ____ and the C-C-N angle is:
(A) sp2 , 109.5o (B) sp , 180o (C) sp2 , 120o (D) sp3 , 109.5
43. Which of the following substances has the highest vapor pressure (at 25 oC)?
(A) CH3OCH3
(B) CH3OH
(C) CH3CH2CH2CH3
(D) CH3CH2CH3
44. A sample of air in a 20 L container at 200 oC contains 3x1022 molecules. What is
the pressure of the air, in torr?
(A) 73 torr
(B) 31 torr
(C) 0.10 torr
(D) 7450 torr
45. The pressure of a gas is 25 lb/in2 in an 800 mL container at 30 oC. What is the
pressure, in lb/in2, if the volume is decreased to 500 mL and the temperature is
increased to 130 oC?
(A) 12 lb/in2
(B) 21 lb/in2
(C) 53 lb/in2
(D) 173 lb/in2
46. For the reaction, 4 Al(s) + 3 O2(g) 2 Al2O3(s), how many Liters of O2(g) at
40 oC and 0.70 atm. (reacting with excess Al) are required to produce 150 grams
of Al2O3?
(A) 12.4 L
(B) 36 L
(C) 54 L
(D) 81 L
47. Consider the reaction, 2 H2(g) + O2(g) 2 H2O(l). Approximately how many
moles of H2O(l) can be produced by the reaction of 30 L of H2(g) at 300 K and
1. atm. with 20 L of O2(g) at 300 K and 1. atm?
(A) 0.81 mol
(B) 1.22 mol
(C) 1.62
(D) 2.44 mol
48. Nickel carbonyl, Ni(CO)4, can be decomposed to Ni(s) and CO(g) by heating. If
one starts with 120 g of Ni(CO)4(s), approximately how many Liters of CO(g) will
be produced at a temperature of 250 oC and a pressure of 400 torr from the
decomposition of the sample?
(A) 14 L
(B) 109 L
(C) 230 L
(D) 57 L
49. The fraction of CO(g) in air is 12 ppm (parts per million). Approximately how
many moles of CO(g) are in a 1500. L tank at 150 oC filled with air at a pressure
of 700 torr?
(A) 4.8x10-4 mol
(B) 0.013 mol
(C) 1.3x10-3 mol
(D) 4.8x108 mol
50. A mixture contains 0.60 mol of CH4(g) and 0.20 mol of CO2(g). The partial
pressure of CO2 is 1.40 atm. Therefore, the partial pressure of CH4 is ____ atm.
and the total pressure is ____ atm.
(A) 4.20 , 2.80
(B) 4.20 , 5.60
(C) 5.60 , 4.20
(D) cannot be determined without the volume and temperature of the mixture
51 Consider the following 3 gases: (i) SO2(g) at 200 oC, (ii) C3H8(g) at 170 oC,
(iii) C2H6(g) at 200 oC. _____ has the highest RMS speed and ____ has the
lowest Kinetic Energy.
(A) C2H6 , SO2
(B) C3H8 , SO2
(C) C2H6 , C3H8
(D) SO2 , C3H8
52. The RMS average speed of SO2(g) molecules at 25 oC is 340 m/s. What is the
RMS average speed of SO2(g) molecules at 800 oC?
(A) 645 m/s
(B) 180 m/s
(C) 1220 m/s
(D) 1920 m/s
53. The RMS average speed of SO2(g) molecules at 25 oC is 340 m/s. What is the
RMS average speed of C3H8(g) molecules at 25 oC?
(A) 280 m/s
(B) 410 m/s
(C) 495 m/s
(D) 720 m/s
54. The rate of effusion of SO2(g) through a pinhole is 0.35 mol/min. Under the
same conditions, the rate of effusion of an unknown gas through the pinhole is
0.50 mol/min. Therefore, the Molar Mass of the unknown gas is approximately:
(A) 45 g/mol
(B) 130 g/mol
(C) 54 g/mol
(D) 31 g/mol
55. The van der Waals equation for a real gas is: [P+a(n/V)2][V-nb] = nRT. The
purpose of the a(n/V)2 term is to correct for the fact that the pressure of a real
gas is ______ than the pressure of an ideal gas because of ______
intermolecular forces.
(A) greater, repulsive
(B) less, repulsive
(C) greater, attractive
(D) less, attractive
56. CFCs (chlorofluorocarbons) are very _______ compounds and cause depletion
of ozone in the ______.
(A) stable, troposphere
(C) unstable , troposphere
(B) stable , stratosphere
(D) unstable , stratosphere
57. FeS2(s) in coal is burned to form SO2(g) according to the reaction:
4 FeS2(s) + 11 O2(g) 2 Fe2O3(s) + 8 SO2(g).
The coal in a power plant contains 6% FeS2 by weight, and produces 4.5x109
grams of SO2(g) in one day. How many grams of coal were burned in the day?
(A) 2.5x108 g
(B) 1.4x1011 g
(C) 7.0x1010 g
(D) 4.2x109 g
58. The functions of an automobile catalytic converter include:
(i)
(ii)
(iii)
(iv)
lower concentration of NO in exhaust
lower concentration of CO2 in exhaust
adjust fuel/air ratio in the fuel injector
lower concentration of VOCs in exhaust
(A) i , iii , iv
(B) i , ii , iv
(C) i , ii , iii
(D) i , iv
59. When the pressure over a solid is increased, the sublimation temperature will
(A) always decrease
(B) increase or decrease (C) always increase
(D) not be changed
B
For #60-#62: Consider a substance
C
with the phase diagram to the right.
P
D
A
T
60. The Critical Point in the diagram is:
(A) Point A
(B) Point B
(C) Point C
(D) Point D
61. If the pressure on the substance is decreased from 500 atm. to 1 atm.,
(A) the melting point will increase and the boiling point will decrease.
(B) the melting point will decrease and the boiling point will decrease.
(C) the melting point will increase and the boiling point will increase.
(D) the melting point will decrease and the boiling point will increase.
62. At pressures below the triple point pressure, the substance can exist as
(A) solid or liquid or vapor
(B) solid only
(C) vapor only
(D) solid or vapor
63. The normal boiling point of anthracene is 340 oC (this is the temperature at which
the vapor pressure is 1 atm. = 760 torr). The enthalpy of vaporization of
napthalene is 52 kJ/mol.
What is the vapor pressure of anthracene at 310 oC (in torr)?
(A) 1290 torr
(B) 450 torr
(C) 5.8x10-21 torr
(D) 130 torr
For #64 - #65: Consider crystalline KCl, which
has the same crystal structure as NaCl
(face-centered cubic)
There are K+ ions () at each corner and on each face.
There are Cl- ions ()on each edge and in the center.
The length of the KCl unit cell is 6.28 (1 = 1x10-8 cm).
64. How many K+ and Cl- ions are there in one unit cell?
(A) 1 K+ , 1 Cl-
(B) 2 K+ , 2 Cl-
(C) 3 K+ , 3 Cl-
(D) 4 K+ , 4 Cl-
65. The total mass of ions in the unit cell is 4.9x10-22 g.
The density of KCl, in g/cm3, is
(A) 2.0 g/cm3
(B) 7.8x10-15 g/cm3
(C) 0.5 g/cm3
(D) 7.8 g/m3