Name: __________________________ Date: _____________
1. If a solute dissolves in an endothermic process,
A)
B)
C)
D)
E)
the entropy of the solution must be greater than that of its pure components.
H bonds must exist between solvent and solute.
strong ion-dipole forces must exist in the solution.
the solute must be a gas.
the solute must be a liquid.
2. Determine the boiling point of a solution prepared by dissolving 678 g of glucose
(C6H12O6) in 2.00 kg of water at 1 atm. For water, Kb = 0.52 °C/m.
A)
B)
C)
D)
E)
101 °C
103 °C
105 °C
106 °C
104 °C
3. What is the percent of CsCl by mass in a 0.711 M aqueous CsCl solution that has a
density of 1.091 g/mL?
A)
B)
C)
D)
E)
11.0 %
3.87  10–4 %
3.87  10–1 %
3.87 %
1.09 %
4. The solubility of nitrogen gas at 25.0 °C and a nitrogen pressure of 522 mmHg is 0.013
g/L. What is the value of the Henry's Law constant in mol/L∙ atm?
A)
B)
C)
D)
E)
6.8  10–4
4.7  10–4
3.2  10–4
9.0  10–7
1.5  103
Page 1
5. Diethyl ether has a vapor pressure of 400. torr at 18.0 °C. When a sample of benzoic
acid, which is a non-volatile, is dissolved in ether, the vapor pressure of the solution is
342 torr. What is the mole fraction of benzoic acid in the solution?
A)
B)
C)
D)
E)
0.145
0.0169
0.0197
0.855
0.455
6. A solution of 1.00 g of AlCl3 in 50.0 g of water freezes at -1.11 °C. Determine the van't
Hoff factor (i) for AlCl3. Given: Kf = 1.86 °C/m
A)
B)
C)
D)
E)
4
3
2
1
5
7. When water and ethanol (C2H5OH) are mixed, which of the following forces will take
place?
A)
B)
C)
D)
E)
I. dispersion forces
II.dipole-dipole interactions
III. ion-dipole interactions
IV. hydrogen bonding
I, II and IV only.
I, III and IV only.
I and IV only.
II and IV only.
All of them
Page 2
8. Consider the phase diagram below. If the dashed line at 1 atm of pressure is followed
from 100 to 500 °C, what phase changes will occur (in order of increasing temperature)?
A)
B)
C)
D)
E)
fusion, followed by vaporization
condensation, followed by vaporization
sublimation, followed by deposition
vaporization, followed by deposition
no phase change will occur under the conditions specified.
9. The molar enthalpy of vaporization of hexane (C6H14) is 28.9 kJ/mol, and its normal
boiling point is 68.73°C. What is the vapor pressure of hexane at 25°C?
A)
B)
C)
D)
E)
171 torr
225 torr
117 torr
3370 torr
759 torr
10. Which one of the following statements is true?
A) Liquids having strong intermolecular forces have higher viscosities than those that
have weaker intermolecular forces.
B) Liquid with high molecular weight is less viscous than liquid with low molecular
weight.
C) The higher the viscosity, the faster a liquid flows.
D) Benzene is more viscous than water because it is a polar compound.
E) A molecule would become less viscous if it has more -OH groups.
Page 3
11. What is the process where molecules go directly from the solid phase to the gas phase?
A)
B)
C)
D)
E)
Sublimation
Freezing
Condensation
Melting
Deposition
12. Vanadium (V) crystallizes in a body-centered cubic lattice, and the length of the edge of
its unit cell is 305 pm. What is the density of V?
A)
B)
C)
D)
E)
5.96 g/cm3
2.98 g/cm3
11.9 g/cm3
7.92 g/cm3
6.92 g/cm3
13. What volume of oxygen gas, at 720 torr and 37°C, would be consumed in the formation
of 22.0 g of P2O3 by the following reaction?
2 PH3(g) + 3 O2(g) → P2O3(s) + 3 H2O(g)
A)
B)
C)
D)
E)
16.1 L
12.5 L
11.2 L
8.05 L
1.92 L
14. A compound composed of carbon, hydrogen, and chlorine effuses through a pinhole
0.411 times as fast as neon (Ne).
Select the correct molecular formula for the compound.
A)
B)
C)
D)
E)
CHCl3
CH2Cl2
C2H2Cl3
C2H3Cl
C3H3Cl2
Page 4
15. The root-mean-square speed of H2S at 26.0°C is __________ m/sec.
A)
B)
C)
D)
E)
468
14.8
46.5
751
214
16. A pressure that will support a column of Hg to a height of 256 mm would support a
column of water to what height? The density of mercury is 13.6 g/cm3 ; the density of
water is 1.00 g/cm3.
A)
B)
C)
D)
E)
348 cm
18.8 cm
455 cm
214 cm
498 cm
17. A sample of a gas occupies 1.40  103 mL at 25.0°C and 760. mmHg. What volume
will it occupy at the same temperature and 380. mmHg?
A)
B)
C)
D)
E)
2.80 x 103 mL
1.40 x 103 mL
1.05 x 103 mL
2.11 x 103 mL
700. mL
18. If 0.50 mole H2(g) and 1.0 mole He(g) are compared at standard temperature and
pressure, the two gases will:
A)
B)
C)
D)
E)
have equal average molecular kinetic energies
occupy equal volumes
have equal weights
have equal effusion rates
have equal average molecular velocities
Page 5
19. What is the approximate bond angle between H-N-H bond in NH2– ion?
A)
B)
C)
D)
E)
109.5°
120°
180°
90°
135°
20. Which one of the following is NOT polar?
A) ICl2B) PCl3
C) CH3Br
D) SCl4
E) ICl5
21. What is the hybridization state of Sb in SbCl3 molecule?
A)
B)
C)
D)
E)
sp3
sp2
sp
sp3d
sp3d2
22. What is the molecular geometry of the IF2O2- ion?
A)
B)
C)
D)
E)
see-saw
tetrahedral
trigonal bipyramidal
square planar
square pyramidal
23. Identify the paramagnetic species from the following:
I. B2
A)
B)
C)
D)
E)
II. N2+
III. F 2
All of them
I only.
II only.
III only.
I and III only.
Page 6
24. Which of the following have resonance structures?
I. O3
A)
B)
C)
D)
E)
-
II. NO3
III. C2H2
IV. SO2
I, II and IV only
I and IV only
II and IV only
III and IV only
II, III and IV only
25. The boiling point of helium is 4.22 K. Express this in oF.
A)
B)
C)
D)
E)
−452.07 °F
−181.41 °F
−117.41 °F
−167.18 °F
−131.27 °F
26. What is the formula for calcium permanganate?
A)
B)
C)
D)
E)
Ca(MnO4)2
CaMnO4
Ca2MnO4
CaMn2O7
Ca(Mn2O7)2
27. Which one of the following is a wrong statement?
A)
B)
C)
D)
E)
Electrons and protons have about the same mass.
Alpha particles have + 2 charge.
Beta particles are attracted by alpha particles.
Beta particles are negatively charged.
The isotopes of a given element have different mass numbers.
Page 7
28. The percent composition by mass of fumaric acid (C4H4O4 ) is ________.
A)
B)
C)
D)
E)
C 41.39%
C 33.33%
C 39.80%
C 40.00%
C 0.25%
H 3.47%
H
33.33%
H
6.68%
H
6.67%
H
0.25%
O 55.14%
O 33.33%
O
53.52%
O
53.33%
O
0.50%
29. How many grams of calcium are required to react with 7.75 g water to produce calcium
hydroxide and hydrogen gas?
A)
B)
C)
D)
E)
8.62 g
34.5 g
4.31 g
3.48 g
17.2 g
30. Which of the following statements about a reducing agent are correct?
I. It is reduced during the reaction.
II. Its oxidation number increases.
III. It loses one or more electrons.
IV. It leads to the reduction of a substance it reacts with.
A)
B)
C)
D)
E)
II, III and IV only.
I, III and IV only.
III and IV only.
I and II only.
II and IV only.
31. What volume of a 0.452 M NaOH solution is needed to neutralize 85 mL of a 0.176 M
solution of H2SO4?
A)
B)
C)
D)
E)
66.2 mL
38.4 mL
436.6 mL
33.1 mL
218.3 mL
Page 8
32. What is the coefficient for O2 when the following combustion reaction of a hydrocarbon
is balanced with whole number coefficients?
___ C7H14 + ___ O2  ___ CO2 + ___ H2O
A)
B)
C)
D)
E)
21
11
35
7
15
33. Determine the enthalpy change when 5.00 g of Fe2 O3 react with aluminum metal
according to the following equation:
Fe2O3(s) + Al(s) → Al2O3(s) + Fe(l)
ΔHf° (kJ/mol): Fe2O3(s) = –825.5;
A)
B)
C)
D)
E)
Al2O3(s) = –1675.7; Fe(l) = 12.4
–25.8 kJ
–26.2 kJ
–52.4 kJ
–77.9 kJ
–165 kJ
34. A 0.1000-g sample of liquid benzene, C6H6, is burned in a calorimeter whose heat
capacity is 1602 J/oC.
C6H6(l) + 7.5 O2(g)

3 H2O(l) + 6 CO2(g)
The combustion of benzene causes a temperature rise of 2.609 oC. Calculate the heat of
combustion for one mole of benzene.
A)
B)
C)
D)
E)
3265. kJ/mol
479.6 kJ/mol
535.1 kJ/mol
786.1 kJ/mol
4.180 x 104 kJ/mol
Page 9
35. Which one of the following statements is true?
A) Ni has 2 unpaired electrons in its 3d orbitals.
B) The exact location of an electron can be determined if we know its energy.
C) An electron in a 2s orbital can have the same n, l, and ml quantum numbers as an
electron in a 3s orbital.
D) In the buildup of atoms, electrons occupy the 4f orbitals before the 6s orbitals.
E) Only three quantum numbers are needed to uniquely describe an electron.
36. Which of the following has the highest first ionization energy?
A)
B)
C)
D)
E)
Kr
Xe
Ca
Br
Sn
37. What is the maximum number of electrons in a atom that can have the following set of
quantum numbers? n = 4 l = 3 ml = –2 ms = +1/2
A)
B)
C)
D)
E)
1
0
6
2
10
38. Select the correct electron configuration for Cu+ ion.
A)
B)
C)
D)
E)
[Ar]3d10
[Ar]4s24p63d3
[Ar]4s13d9
[Ar]4s24d8
[Ar]5s24d9
Page 10
39. Select the Lewis structure for XeO2F2 which correctly minimizes formal charges.
A)
B)
C)
D)
E)
II
I
III
IV
V
40. Which of these pairs of elements would be most likely to form an ionic compound?
A)
B)
C)
D)
E)
Mg and Cl
Al and K
Br and I
C and S
Al and Cs
Page 11
Answer Key
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38.
39.
40.
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
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