Chem 1100 Pre-Test 3
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1.
An open-tube manometer is used to measure the pressure in a flask. The atmospheric pressure is 756
torr and the Hg column is 8.5 cm higher on the open end. What is the pressure in the flask?
a. 764.5 mmHg
b. 841 cm Hg
c. 841 torr
d. 671 torr
e. 747.5 mm Hg
____
2.
A sample of gas occupies a volume of 1.60 L at a pressure of 720. torr. What would be the pressure of
this gas if it were compressed to 1.20 L at the same temperature?
a. 540. torr
b. 360. torr
c. 180. torr
d. 960. torr
e. 1440 torr
____
3.
a.
b.
c.
d.
e.
____
4.
A sample of neon occupies 4.50 liters at 30.0C and 2.50 atmospheres. What volume will it occupy at
1000. torr and 300.C?
a. 4.52 L
b. 4.48 L
c. 16.2 L
d. 8.96 L
e. 1.25 L
____
5.
a.
b.
c.
d.
e.
What is the volume occupied by 10.0 grams of NH3 at STP, if it behaves ideally?
10.6 L
13.2 L
14.3 L
14.9 L
15.8 L
____
6.
a.
b.
c.
d.
e.
What is the molecular weight of a gas if 0.104 gram of the gas occupies 48.7 mL at STP?
5.06 g/mol
28.2 g/mol
34.5 g/mol
40.0 g/mol
47.8 g/mol
____
7.
A gas sample occupies 1.00 L at 120.C and 1.00 atm. What volume will it occupy at STP?
1.14 L
1.44 L
0.846 L
0.782 L
0.695 L
How many moles of Argon would occupy 75 mL at 33C and 1.07 atm?
a.
b.
c.
d.
e.
3.19
2.96  102
3.19  103
3.15  105
0.313
____
8.
a.
b.
c.
d.
e.
Calculate the density of O2 gas (in g/L) at 1.22 atm and 25C.
1.74 g/L
1.60 g/L
0.871 g/L
19.0 g/L
0.798 g/L
____
9.
A mixture of gases containing 21.0 g of N2, 106.5 g of Cl2 and 12.0 g of He at 14C is in a 50.0-L
container. What is the total pressure in the vessel?
a. 1.8 atm
b. 2.2 atm
c. 2.5 atm
d. 2.7 atm
e. 3.2 atm
____
10.
A mixture of gas contains 0.251 g Ar and 1.95 g Xe and has a total pressure of 2.33 atm. What are the
partial pressures of each gas?
a.
b.
c.
d.
e.
PAr (atm)
1.61
0.72
1.17
0.27
0.30
PXe (atm)
0.72
1.61
1.16
2.06
2.03
____
11.
a.
b.
c.
d.
e.
What is the mole fraction of O2 in a mixture of 2.00 g He, 12.0 g O2, and 17.0 g N2?
0.608
0.253
0.410
0.200
0.267
____
12.
A 300.-mL sample of hydrogen, H2, was collected over water at 21C on a day when the barometric
pressure was 748 torr. What mass of hydrogen is present? The vapor pressure of water is 19 torr at 21C.
a. 0.0186 g
b. 0.0241 g
c. 0.0213 g
d. 0.0269 g
e. 0.0281 g
____
13.
What total volume of gas (at STP) is produced by the electrolysis of 4 moles of H 2O?
2H2O(g)  2H2(g) + O2(g)
a. 67.2 L
b. 134.4 L
c. 3.0 L
d. 112 L
e. 5.0 L
____
14.
Calculate the weight of KClO3 that would be required to produce 29.52 liters of oxygen measured at
127C and 760. torr.
2KClO3(s)
a.
b.
c.
d.
e.
____
15.
a.
b.
c.
d.
e.
____
2KCl(s) + 3O2(g)
7.82 g
12.2 g
14.64 g
24.4 g
73.5 g
What is the order of increasing rate of effusion for the following gases?
Ar, CO2, He, N2
N2 < Ar < CO2 < He
Ar < CO2 < He < N2
Ar < He < CO2 < N2
CO2 < N2 < Ar < He
CO2 < Ar < N2 < He
16.
for
a.
b.
c.
d.
e.
The van der Waals constant, b, in the relationship
is a factor that corrects
deviations in the gas constant, R.
the attractive forces between gas molecules.
the tendency of the gas molecules to ionize.
the average velocities of the gas molecules.
the volume occupied by the gas molecules.
____
17.
a.
b.
c.
d.
e.
Which of the following statements is false? An increase in temperature will
increase the molecular weight of the gas.
increase the velocity of the gas molecules.
increase the number of collisions per second.
increase the average kinetic energy of the molecules.
increase the root-mean-square velocity of the molecules.
____
18.
a.
b.
c.
d.
e.
Which of the following gases is expected to have the largest value for its van der Waals constant "b"?
Ne
O2
H2
CO
CO2
____
19.
Calculate the pressure of 1000. grams of ethylene gas (C 2H4) in a 10.0 L container at 30.0C. Do not
assume ideal gas behavior. a = 4.471 L2-atm/mol2, b = 0.05714 L/mol.
a. 35.7 atm
b. 168 atm
c. 54.6 atm
d. 68.0 atm
e. 88.8 atm
____
20.
a.
b.
c.
d.
e.
Which of the following interactions are the strongest?
hydrogen bonding force
ion-ion interactions
permanent dipole force
dispersion force
London force
____
21.
The boiling points of the halogens increase in the order F 2 < Cl2 < Br2 < I2 due to the resulting
increasing ____ interactions.
a. ion-dipole
b. hydrogen-bonding
c. ion-ion
d. dispersion forces
e. permanent dipole-dipole
____
22.
a.
b.
c.
d.
e.
The term used to describe resistance to flow of a liquid is ____.
surface tension
capillary action
viscosity
vapor pressure
vaporization
____
23.
a.
b.
c.
d.
e.
Which of these liquids would have the highest surface tension at 25C?
Br2
H2O
CCl4
C5H12
CH3OCH3
____
24.
a.
b.
c.
d.
e.
Which of the following boils at the highest temperature?
C2H6
C3H8
C4H10
C5H12
C6H14
____
25.
Calculate the amount of heat required to raise the temperature of 165 g of water from 12.0C to
88.0C. (Sp. heat of H2O
a. 52.4 kJ
b. 1.93 J
c. 60.7 kJ
d. 1.46 kJ
e. 15.6 J
____
26.
= 4.18 J/gC)
Calculate the amount of heat (in joules) required to convert 92.5 g of water at 25.0C to steam at
108.0C. (Sp. heat of H2O
kJ/g)
= 4.18 J/gC, Sp. heat of H2O(g) = 2.03 J/gC, heat of vap. of H2O
= 2.260
a.
b.
c.
d.
e.
____
27.
Using the Clausius-Clapeyron equation determine the vapor pressure of water at 50.0C. The molar
heat of vaporization of water is 40.7 kJ/mol.
a.
b.
c.
d.
e.
____
2.26  105 J
3.05  104 J
2.40  105 J
2.20  104 J
6.43  105 J
28.
700 torr
450 torr
100 torr
80 torr
55 torr
Which response has the following substances arranged in order of increasing boiling point?
Ar, NaClO3, H2O, H2Se
a.
b.
c.
d.
e.
NaClO3 < H2O < H2Se < Ar
NaClO3 < H2Se < H2O < Ar
Ar < NaClO3 < H2Se < H2O
Ar < H2O < H2Se < NaClO3
Ar < H2Se < H2O < NaClO3
____
29.
a.
b.
c.
d.
e.
In a body-centered cubic lattice, how many atoms are contained in a unit cell?
one
two
three
four
five
____
30.
a.
b.
c.
d.
e.
Which one of the following is an ionic solid?
graphite
nickel
ammonium chloride
silicon carbide, SiC
sucrose, C12H22O11
____
31.
a.
b.
c.
d.
e.
Which one of the following is a molecular solid?
NH4Cl
K
SiC
C6H6
KC2H3O2
____
32.
Which one of the following substances is incorrectly matched with the kind of solid it forms?
Substance / Kind of Solid
a. sulfur dioxide / molecular
b.
c.
d.
e.
graphite / covalent
calcium bromide / ionic
potassium / ionic
methane / molecular
____
33.
Metallic calcium crystallized in a face-centered cubic lattice, and the edge of the cube is 15.57Å.
Calculate the density of calcium.
a. 1.28 g/cm3
b. 1.42 g/cm3
c. 1.54 g/cm3
d. 1.84 g/cm3
e. 2.11 g/cm3
____
34.
a.
b.
c.
d.
e.
Which one of the following elements is considered a semiconductor?
Li
Fe
Cl
Ni
Si
____
35.
Elements that have their highest energy electrons in a filled valence band that is separated from the
conductance band by an energy difference much too large for electrons to jump between bands are called
____.
a. semiconductors
b. metals
c. conductors
d. insulators
e. isomorphs
____
36.
a.
b.
c.
d.
e.
____
37.
At 25C, 100 g of water will be saturated with 35.7 g of NaCl. Which word below describes the
solution of 1.55 mol of NaCl dissolved in 250 mL of water?
a. saturated
b. unsaturated
c. supersaturated
d. metasaturated
e. none of these apply
____
38.
a.
b.
c.
d.
e.
____
39.
What mass of water must be used to dissolve 20.0 grams of ethanol, C 2H5OH, to prepare a 0.0500
molal solution of ethanol?
Which of the following solutions would not be expected to exist?
MgCl2 in CCl4
NaCl in water
Pentane, C5H12, in CCl4
methanol, CH3OH, in water
Vegetable oil in mineral oil
Calculate the molality of a solution that contains 25 g of H2SO4 dissolved in 40. g of H2O.
3.2 m
4.4 m
6.4 m
13 m
14 m
a.
b.
c.
d.
e.
3.76 kg
4.00 kg
8.70 kg
6.35 kg
7.18 kg
____
40.
What is the mole fraction of ethanol, CH3CH2OH, in an aqueous solution that is 20.0% ethanol by
mass?
a. 0.150
b. 0.144
c. 0.0980
d. 0.0892
e. 0.208
____
41.
a.
b.
c.
d.
e.
Which of the following is not a colligative property?
osmotic pressure
vapor pressure raising
boiling point elevation
freezing point depression
All of these are colligative properties
____
42.
a.
b.
c.
d.
e.
Which aqueous solution would have the lowest vapor pressure at 25C?
1 M NaCl
1 M K3PO4
1 M sucrose, C12H10O11
1 M MgCl2
1 M glucose, C6H12O6
____
43.
At 40C, the vapor pressure of heptane is 92 torr. If a solution is made of naphthalene in heptane and
has a vapor pressure of 82 torr, what is the mole fraction of naphthalene? Assume ideal solution behavior.
a. 0.891
b. 0.435
c. 0.487
d. 0.109
e. 1.109
____
44.
a.
b.
c.
d.
e.
____
45.
The boiling point of pure water in Winter Park, CO ( elev. 9000 ft), is 94C. What is the boiling point
of a solution containing 11.3 g of glucose (180 g/mol) in 55 mL of water in Winter Park? Kb for water =
0.512C/m.
a. 94.6C
b. 95.1C
c. 98.6C
d. 100C
e. 93.4C
Which of these aqueous solutions would be expected to have the highest boiling point?
0.100 m KCl
0.100 m NaOH
0.075 m K2SO4
0.050 m Al2(SO4)3
0.200 m CH3OH
____
46.
Calculate the freezing point of a solution that contains 68.4 g of sucrose (table sugar) in 300. g of
water. One mole of sucrose is 342 g. Kf for H2O = 1.86C/m.
a. 0.186C
b. 0.372C
c. 0.558C
d. 0.744C
e. 1.24C
____
47.
Estimate the molecular weight of a biological macromolecule if a 0.100-gram sample dissolved in
50.0 mL of benzene has an osmotic pressure of 9.76 torr at 25.0C.
a. 3.8  103 g/mol
b. 4.2  104 g/mol
c. 5.6  104 g/mol
d. 6.7  104 g/mol
e. 8.3  103 g/mol
Chem 1100 Pre-Test 3
Answer Section
MULTIPLE CHOICE
1.
ANS:
C
PTS:
1
TOP:
Pressure
2.
ANS:
D
PTS:
1
TOP:
Boyle's Law: The Volume-Pressure
Relationship
3.
ANS:
E
PTS:
1
TOP: Charles's Law: The Volume-Temperature Relationship; The Absolute Temperature Scale
4.
ANS:
C
PTS:
1
TOP:
The Combined Gas Law Equation
5.
ANS:
B
PTS:
1
TOP:
Avogadro's Law and the Standard Molar
Volume
6.
ANS:
E
PTS:
1
TOP:
Avogadro's Law and the Standard Molar
Volume
7.
ANS:
C
PTS:
1
TOP:
Summary of Gas Laws: The Ideal Gas
Equation
8.
ANS:
B
PTS:
1
TOP:
Summary of Gas Laws: The Ideal Gas
Equation
9.
ANS:
C
PTS:
1
TOP:
Dalton's Law of Partial Pressures
10.
ANS:
B
PTS:
1
TOP:
Dalton's Law of Partial Pressures
11.
ANS:
B
PTS:
1
TOP:
Dalton's Law of Partial Pressures
12.
ANS:
B
PTS:
1
TOP:
Dalton's Law of Partial Pressures
13.
ANS:
B
PTS:
1
TOP:
Mass-Volume Relationships in Reactions
Involving Gases
14.
ANS:
E
PTS:
1
DIF:
Harder Question
TOP: Mass-Volume Relationships in Reactions Involving Gases
15.
ANS:
E
PTS:
1
TOP:
Diffusion and Effusion of Gases
16.
ANS:
E
PTS:
1
TOP:
Deviations from Ideal Gas Behavior
17.
ANS:
A
PTS:
1
TOP:
The Kinetic-Molecular Theory
18.
ANS:
E
PTS:
1
TOP:
Deviations from Ideal Gas Behavior
19.
ANS:
C
PTS:
1
DIF:
Harder Question
TOP: Deviations from Ideal Gas Behavior
20.
ANS:
B
PTS:
1
TOP:
Intermolecular Attractions and Phase
Changes
21.
ANS:
D
PTS:
1
TOP:
Intermolecular Attractions and Phase
Changes
22.
ANS:
C
PTS:
1
TOP:
Viscosity
23.
ANS:
B
PTS:
1
TOP:
Surface Tension
24.
ANS:
E
PTS:
1
TOP:
Boiling Points and Distillation
25.
ANS:
A
PTS:
1
TOP:
Heat Transfer Involving Liquids
26.
ANS:
C
PTS:
1
TOP:
Heat Transfer Involving Liquids
27.
ANS:
C
PTS:
1
DIF:
Harder Question
TOP: Heat Transfer Involving Liquids
28.
ANS:
E
PTS:
1
TOP:
Heat Transfer Involving Liquids
29.
ANS:
B
PTS:
1
TOP:
Structures of Crystals
30.
ANS:
C
PTS:
1
TOP:
Bonding in Solids
31.
ANS:
D
32.
ANS:
D
33.
ANS:
C
TOP: Bonding in Solids
34.
ANS:
E
35.
ANS:
D
36.
ANS:
A
(Miscibility)
37.
ANS:
C
38.
ANS:
C
39.
ANS:
C
40.
ANS:
D
41.
ANS:
B
42.
ANS:
B
Law
43.
ANS:
D
Law
44.
ANS:
C
45.
ANS:
A
46.
ANS:
E
47.
ANS:
A
PTS:
PTS:
PTS:
1
1
1
TOP:
TOP:
DIF:
Bonding in Solids
Bonding in Solids
Harder Question
PTS:
PTS:
PTS:
1
1
1
TOP:
TOP:
TOP:
Band Theory of Metals
Band Theory of Metals
Dissolution of Liquids in Liquids
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
1
1
1
1
1
1
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
Rates of Dissolution and Saturation
Molality and Mole Fraction
Molality and Mole Fraction
Molality and Mole Fraction
Colligative Properties of Solutions
Lowering of Vapor Pressure and Raoult's
PTS:
1
TOP:
Lowering of Vapor Pressure and Raoult's
PTS:
PTS:
PTS:
PTS:
1
1
1
1
TOP:
TOP:
TOP:
TOP:
Boiling Point Elevation
Boiling Point Elevation
Freezing Point Depression
Osmotic Pressure