Multiple Choice
Identify the
letter of the choice that best completes the statement or answers the question.
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1.
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According to the kinetic-molecular theory of matter, particles in a
liquid a. | are packed
closely together in a regular array. | b. | move slower as the temperature
increases. | c. | expand to fill their container. | d. | vibrate back and
forth about an average position. | e. | are packed closely together, but are not confined to specific
positions. | | |
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2.
|
A
pure substance composed of two or more different elements is a. | a homogeneous
mixture. | b. | a heterogeneous mixture. | c. | a
polyelement. | d. | an atom. | e. | a chemical
compound. | | |
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3.
|
What
is the correct symbol for lead?
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4.
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The
molecular model below depicts a molecule composed of carbon (black), oxygen (gray), and hydrogen
(white) atoms. What is the correct molecular formula?
a. | CHO | b. | C6H6O2 | c. | C6H7O | d. | C7H6O | e. | C7H6O2 | | |
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5.
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When
24 copper pennies are submerged in water, the pennies displace 8.26 cm3 of water. If the
combined mass of the pennies is 73.86 g, what is the density of copper? a. | 0.112
g/cm3 | b. | 1.34 g/cm3 | c. | 8.94
g/cm3 | d. | 32.8 g/cm3 | e. | 107
g/cm3 | | |
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6.
|
At 0
°C, a bottle
contains 325 mL of water in its liquid state. What is the volume of the water after it freezes (at 0
°C)? The
densities of liquid water and ice at 0 °C are 1.000 g/mL and 0.917 g/mL, respectively. a. | 27.0
mL | b. | 298
mL | c. | 325
mL | d. | 354
mL | e. | 391
mL | | |
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7.
|
All
of the following are examples of chemical change EXCEPT a. | the tarnishing
of silver. | b. | the rusting of iron. | c. | the combustion
of butane gas. | d. | the condensation of steam. | e. | the
decomposition of water to hydrogen gas and oxygen gas. | | |
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8.
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Which
of the following observations are examples of chemical changes to
aluminum?
1. | When aluminum reacts with hydrochloric acid, hydrogen gas is
evolved. | 2. | Aluminum melts
at 660 °C. | 3. | A cube of aluminum with a volume of 4.0 cm3 has a
mass of 10.8 g. | 4. | Aluminum is a good electrical
conductor. | | |
a. | 1
only | b. | 2
only | c. | 1 and
2 | d. | 3 and
4 | e. | 1, 2 and
4 | | |
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9.
|
Thermostats are often set to 68 °F. What is this temperature in Celsius? a. | 2.0 ´ 101
°C | b. | 25 °C | c. | 38 °C | d. | 56 °C | e. | 7.0 ´ 102 °C | | |
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10.
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The
boiling point of liquid helium is 4 K. What is this temperature in Celsius? a. | -294
°C | b. | -277 °C | c. | -269 °C | d. | -255 °C | e. | -169 °C | | |
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11.
|
What
is a correct method for converting Celsius to Kelvin?
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12.
|
Two
electronic balances are tested using a standard weight. The true mass of the standard is 1.3111 g.
The results of 5 individual measurements on each balance are recorded
below.
| Balance A | Balance
B | | 0.8888
g | 1.3110 g | | 0.9959
g | 1.3109 g | | 1.1182
g | 1.3111 g | | 1.0033
g | 1.3110 g | | 0.9938
g | 1.3110 g | average mass = | 1.0000 g | 1.3110
g | | | |
Which statement
best describes the results? a. | A: good precision, good accuracy. B: good precision, good
accuracy. | b. | A: good precision, good accuracy. B: poor precision, poor
accuracy. | c. | A: poor precision, good accuracy. B: good precision, good
accuracy. | d. | A: poor precision, poor accuracy. B: good precision, good
accuracy. | e. | A: poor precision, poor accuracy. B: good precision, poor
accuracy. | | |
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13.
|
Which
method is correct for determining the liters of gas required to fill an automobile's 15 gallon tank?
(1.000 L = 1.057 quarts, 4 quarts = 1 gallon) a. | 15 gallons  | b. | 15 gallons  | c. | 15 gallons  | d. | 15 gallons  | e. | none of the above | | |
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14.
|
The
wavelength of light emitted from a green laser pointer is 5.32 ´ 102
nm. What is the wavelength in meters? a. | 5.32 ´ 10-9 m | b. | 5.32
´ 10-7
m | c. | 5.32
´ 10-5
m | d. | 5.32
´ 10-3
m | e. | 5.32
´ 10-1
m | | |
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15.
|
How
many protons, neutrons, and electrons are in an oxygen-18 atom? a. | 6 protons, 8
neutrons, 4 electron | b. | 6 protons, 10 neutrons, 8 electrons | c. | 8 protons, 8
neutrons, 8 electrons | d. | 8 protons, 10 neutrons, 8 electrons | e. | 8 protons, 10
neutrons, 18 electrons | | |
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16.
|
What
is the atomic symbol for an element that has 30 neutrons and a mass number of 55?
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17.
|
How
many elements are in the first period of the periodic table?
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18.
|
What
alkali metal is in the fourth period?
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19.
|
A
nitride ion has ____ electrons.
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20.
|
For a
nonmetal in Group 5A of the periodic table, the most common monatomic ion will have a charge of
____.
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21.
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Sodium sulfate has the chemical formula Na2SO4. Based on this
information, the formula for chromium(III) sulfate is ____. a. | Cr3(SO4)2 | b. | Cr2(SO4)3 | c. | Cr(SO4)2 | d. | Cr2SO4 | e. | CrSO4 | | |
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22.
|
What
is the charge on the copper ion in Cu2O?
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23.
|
What
is the correct formula for potassium dihydrogen phosphate? a. | K2H2PO4 | b. | KH2PO4 | c. | KH2PO3 | d. | K2H2P | e. | KH2P | | |
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24.
|
All
of the following are named correctly EXCEPT a. | LiClO4; lithium
perchlorate. | b. | CaHPO4; calcium hydrogen
phosphide. | c. | NaCN; sodium cyanide. | d. | Mg(OH)2; magnesium hydroxide. | e. | CaSO3; calcium sulfite. | | |
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25.
|
What
is the molar mass of ammonium sulfate? a. | 110.0 g/mol | b. | 114.1
g/mol | c. | 132.1 g/mol | d. | 144.6
g/mol | e. | 168.9 g/mol | | |
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26.
|
What
is the mass percent of each element in dichloromethane,
CH2Cl2? a. | 10.06% C, 60.24% H, 29.70% Cl | b. | 20.00% C, 20.00%
H, 60.00% Cl | c. | 24.10% C, 3.11% H, 72.79% Cl | d. | 33.87% C, 0.22%
H, 65.91% Cl | e. | 14.14% C, 2.37% H, 83.48% Cl | | |
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27.
|
Nitrogen and oxygen form an extensive series of oxides with the general formula
NxOy. What is the empirical formula for an oxide that contains 46.68%
nitrogen? a. | N2O | b. | NO | c. | NO2 | d. | N2O3 | e. | N2O5 | | |
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28.
|
The
combustion of propane produces carbon dioxide and steam.
C3H8(g) + 5 O2(g) ® 3
CO2(g) + 4 H2O(g)
All of the following statements concerning this reaction are correct
EXCEPT a. | three molecule
of carbon dioxide are formed per one molecule of propane consumed. | b. | five molecules
of oxygen are consumed per one molecule of propane consumed. | c. | four moles of
steam are formed per five moles of oxygen consumed. | d. | the combined
mass of reactants consumed equals the mass of products formed. | e. | three grams of
carbon dioxide are formed per five grams of oxygen consumed. | | |
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29.
|
Ammonia is prepared by reacting nitrogen and hydrogen gases at high temperature
according to the unbalanced chemical equation below.
__ N2(g) + __ H2(g) ® __
NH3(g)
What are the respective coefficients when the equation
is balanced with the smallest whole numbers? a. | 1, 1, 1 | b. | 1, 3,
1 | c. | 1, 3,
2 | d. | 2, 1,
2 | e. | 2, 3,
2 | | |
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30.
|
The
products of the complete combustion of a hydrocarbon are carbon dioxide and water. Write a balanced
chemical equation for the combustion of pentane, C5H12. a. | C5H12(g) + 8 O2(g) ® 5
CO2(g) + 6 H2O(g) | b. | C5H12(g) ® 5 C(s) + 6
H2(g) | c. | C5H12(g) + 9 O2(g)
® 4
CO2(g) + 5 H2O(g) | d. | C5H12(g) + 11 O2(g)
®
C5O10(g) + 6 H2O(g) | e. | C5H12(g) + 11 O2(g) ® 5
CO2(g) + 12 H2O(g) | | |
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31.
|
The
complete combustion of 0.40 moles of butane gas, C4H10, will a. | consume 0.40 mol
O2 and produce 0.20 mol CO2. | b. | consume 0.80 mol
O2 and produce 0.40 mol CO2. | c. | consume 1.3 mol
O2 and produce 0.80 mol CO2. | d. | consume 2.6 mol
O2 and produce 1.6 mol CO2. | e. | consume 5.2 mol
O2 and produce 3.2 mol CO2. | | |
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32.
|
The
compound P4S3 is used in matches. It reacts with oxygen to produce
P4O10 and SO2. The unbalanced chemical equation is shown
below.
P4S3(s) + O2(g)
®
P4O10(s) + SO2(g)
What mass of O2 will react with 0.641 grams of
P4S3? a. | 0.0466 g | b. | 0.0932
g | c. | 0.186
g | d. | 0.372
g | e. | 0.746
g | | |
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33.
|
What
is a correct method for determining how many grams of oxygen react with 1.00 gram of
pentane?
C5H12(g) + 8 O2(g)
® 5
CO2(g) + 6 H2O(g)
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34.
|
Sulfur trioxide is made from the reaction of sulfur dioxide and oxygen. How many grams
of SO3 can be made from the reaction of 3.00 g SO2 with 2.02 g
O2?
2 SO2(g) + O2(g) ® 2
SO3(g)
a. | 2.53 g | b. | 3.75
g | c. | 5.02
g | d. | 5.05
g | e. | 10.1
g | | |
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35.
|
Under
certain conditions the reaction of ammonia with excess oxygen will produce a 38.2% yield of NO. How
many grams of NH3 must be reacted with excess oxygen to yield 17.5 g of
NO?
4 NH3(g) + 5 O2(g) ® 4 NO(g) + 6
H2O(g)
a. | 3.79 g | b. | 9.93
g | c. | 26.0
g | d. | 32.2
g | e. | 45.8
g | | |
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36.
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A
2.000 g mixture of CaCO3 and CaO is heated. The CaCO3 decomposes to CaO and
CO2. What was the mass percentage of CaCO3 in the mixture if the mass after
heating is 1.809 g? a. | 17.8% | b. | 21.7% | c. | 43.4% | d. | 78.3% | e. | 95.5% | | |
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37.
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If
0.10 mole of each of the following compounds is dissolved to a volume of 1.0 L in water, which one
will have the highest concentration of dissolved ions? a. | HF | b. | NaOH | c. | MgSO4 | d. | Al(NO3)3 | e. | CaI2 | | |
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38.
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Which
of the following compounds is a weak acid? a. | H3PO4 | b. | HI | c. | HBr | d. | HClO4 | e. | H2SO4 | | |
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39.
|
What
are the spectator ions in the reaction between aqueous perchloric acid and aqueous potassium
hydroxide? a. | H+,
ClO4-, K+, and OH- | b. | H+
and OH- | c. | K+ and
ClO4- | d. | H+ and
ClO4- | e. | K+ and OH- | | |
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40.
|
Write
a net ionic equation for the reaction of aqueous acetic acid and aqueous potassium
hydroxide. a. | CH3CO2H(aq) + KOH(aq) ® K+(aq) +
CH3CO2-(aq) + H2O(l) | b. | CH3CO2H(aq) + KOH(aq) ®
KCH3CO2(aq) + H2O(l) | c. | H+(aq) + OH-(aq) ®
H2O(l) | d. | CH3CO2H(aq) + OH-(aq)
®
CH3CO3H2-(aq) | e. | CH3CO2H(aq) + OH-(aq) ®
CH3CO2-(aq) + H2O(l) | | |
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41.
|
Write
a balanced equation for the reaction of aqueous solutions of baking soda and acetic
acid. a. | NaHCO3(aq) + CH3CO2H(aq) ®
NaCH3CO2(aq) + H2O( l) + CO2(g) | b. | 2
NaHCO3(aq) + CH3CO2H(aq) ® 2 Na2CO3(aq) + CH4(aq) +
2H2O(
l)
+ CO2(g) | c. | NaHCO3(aq) + CH3CO2H(aq)
®
H2CO3(s) + NaCH3CO2(aq) | d. | NaHCO3(aq) + CH3CO2H(aq) ® NaOH(aq) +
CH3CO2H(aq) + CO2(g) | e. | NaHCO3(aq) + CH3CO2H(aq) ®
CH4(aq) + 2 CO2(g) + O2(g) + NaOH(aq) | | |
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42.
|
Which
of the following are oxidation-reduction reactions?
1. | Zn(s) + CuSO4(aq) ®
ZnSO4(aq) + Cu(s) | 2. | Pb(ClO4)2(aq) + 2 KI(aq) ®
PbI2(s) + 2 NaClO4(aq) | 3. | CaCO3(s) ® CO2(g) + CaO(s) | | |
a. | 1 only | b. | 2
only | c. | 1 and
2 | d. | 1 and
3 | e. | 2 and
3 | | |
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43.
|
If
5.00 mL of 0.314 M KOH is diluted to exactly 125 mL with water, what is the concentration of the
resulting solution? a. | 5.02 ´ 10-4 M | b. | 1.26
´ 10-2
M | c. | 0.127
M | d. | 0.281
M | e. | 7.85
M | | |
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44.
|
What
is the pH of 0.27 M HNO3? a. | 0.57 | b. | 1.31 | c. | 1.86 | d. | 2.70 | e. | 13.43 | | |
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45.
|
A
25.00 mL sample of NaOH is titrated with 17.13 mL of 0.3150 M HCl. What is the concentration of the
NaOH solution? a. | 0.001360
M | b. | 0.1233
M | c. | 0.2158
M | d. | 0.4597
M | e. | 0.7356
M | | |
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46.
|
Assuming the following reaction proceeds in the forward
direction,
Ni2+(aq) + Cr(s) ® Ni(s) +
Cr2+(aq)
a. | Ni2+(aq) is oxidized and Cr(s) is
reduced. | b. | Ni2+(aq) is oxidized and Ni(s) is
reduced. | c. | Ni(s) is oxidized and Ni2+(aq) is
reduced. | d. | Cr(s) is oxidized and Cr2+(aq) is
reduced. | e. | Cr(s) is oxidized and Ni2+(aq) is
reduced. | | |
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47.
|
The
following reaction occurs spontaneously.
3 Cu2+(aq) + 2 Fe(s) ® 2
Fe3+(aq) + 3 Cu(s)
Write the
balanced oxidation half-reaction. a. | 2 Fe(s) ® 2 Fe3+(aq) + 6
e- | b. | 2 Fe(s) + 6 e- ® 2
Fe3+(aq) | c. | 3 Cu2+(aq) + 6 e- ® 3
Cu(s) | d. | 3 Cu2+(aq) ® 3 Cu(s) + 6 e- | e. | 3 Cu(s)
® 3
Cu2+(aq) + 6 e- | | |
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48.
|
Write
a balanced half-reaction for the reduction of ClO3-(aq) to Cl2(g) in
an acidic solution. a. | 2 ClO3-(aq) + 6 H+(aq) + 10
e- ® Cl2(g) + 6 OH-(aq) | b. | 2
ClO3-(aq) + 12 H+(aq) + 5 e- ®
Cl2(g) + 6 H2O(l) | c. | 2 ClO3-(aq) + 10 e-
®
Cl2(g) + 6 H2O(l) + 3 O2(g) | d. | 2 ClO3-(aq) + 12 H+(aq) + 10
e- ® Cl2(g) + 6 H2O(l) | e. | 2 ClO3-(aq) + 18 H+(aq)
®
Cl2(g) + 6 H3O+(aq) | | |
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49.
|
Write
a balanced half-reaction for the reduction of permanganate ion, MnO4-, to
MnO2 in a basic solution. a. | MnO4-(aq) + 4 OH-(aq) + 3
e- ® MnO2(s) + 2 H2O(l) + 2
O2(g) | b. | MnO4-(aq) + 2 OH-(aq) + 3
e- ® MnO2(s) + 2 HO2(aq) | c. | MnO4-(aq) + 3 e- ®
MnO2(s) + O2(g) | d. | MnO4-(aq) + 2 H+(aq) + 3
e- ® MnO2(s) + 2 OH-(aq) | e. | MnO4-(aq) + 2 H2O(l) + 3
e- ® MnO2(s) + 4 OH-(aq) | | |
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50.
|
Write
a balanced chemical equation for the following reaction in an acidic
solution.
Cr2O72-(aq) +
Br-(aq) ® Cr3+(aq) + Br2(aq)
a. | Cr2O72-(aq) + 2 Br-(aq) ® 2
Cr3+(aq) + Br2(aq) | b. | Cr2O72-(aq) + 6
Br-(aq) + 14 H+(aq) ® 3 Br2(aq) + 2 Cr3+(aq) + 7
H2O(l) | c. | Cr2O72-(aq) + 2
Br-(aq) + 14 H+(aq) ® 2 Cr3+(aq) + Br2(aq) + 7
H2O(l) | d. | Cr2O72-(aq) + 2
Br-(aq) + 7 H+(aq) ® 2 Cr3+(aq) + Br2(aq) + 7
OH-(aq) | e. | Cr2O72-(aq) + 6
Br-(aq) + 7 H+(aq) ® 2 Cr3+(aq) + 3 Br2(aq) + 7
OH-(aq) | | |
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51.
|
Of
the following types of energy, which are classified as kinetic energy?
1. | thermal energy | 2. | mechanical energy | 3. | electrical energy | | |
a. | 1 only | b. | 2
only | c. | 3
only | d. | 2 and
3 | e. | 1, 2, and
3 | | |
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52.
|
Specific heat capacity is a. | the quantity of heat needed to change 1.00 g of a substance by
1.00 K. | b. | the mass of a substance that 1.00 J of energy will heat by 1.00
K. | c. | the mass of a
substance that 1.00 cal of energy will heat by 1.00 K. | d. | the temperature
change undergone when 1.00 g of a substance absorbs 4.184 J. | e. | the quantity of
heat required to melt 4.184 g of a substance. | | |
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53.
|
If
the same amount of heat is added to 5.00 g samples of each of the metals below, which metal will
experience the smallest temperature change?
Metal | Specific Heat
Capacity (J/g·K) | Al | 0.897 | Au | 0.129 | Cu | 0.385 | Fe | 0.449 | K | 0.753 | | |
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54.
|
How
much energy is required to change the temperature of 21.5 g Cu from 27.0 °C to 88.1
°C? The specific
heat capacity of copper is 0.385 J/g·K. a. | 223 J | b. | 506
J | c. | 641
J | d. | 729
J | e. | 3.41
´ 103
J | | |
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55.
|
If
50.0 g H2O at 13.6 °C is combined with 85.0 g H2O at 93.7 °C, what is the
final temperature of the mixture? The specific heat capacity of water is 4.184
J/g·K. a. | 26.1
°C | b. | 40.0 °C | c. | 56.1 °C | d. | 64.0 °C | e. | 80.1 °C | | |
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56.
|
Calculate the amount of heat required to change 50.0 g ice at -20.0 °C to steam at
135 °C. (Heat of
fusion = 333 J/g; heat of vaporization = 2260 J/g; specific heat capacities: ice = 2.09 J/g·K,
liquid water = 4.18 J/g·K, steam = 1.84 J/g·K) a. | 4.18
kJ | b. | 32.4
kJ | c. | 78.8
kJ | d. | 135
kJ | e. | 156
kJ | | |
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57.
|
45.0
g of ice at -12.0 °C is mixed with 256 g of water at 31.4 °C. What is the
final temperature of the mixture? (Heat of fusion = 333 J/g; specific heat capacities: ice = 2.09
J/g·K, liquid water = 4.184 J/g·K) a. | -1.6 °C | b. | 0.0 °C | c. | 13.9 °C | d. | 21.0 °C | e. | 25.8 °C | | |
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58.
|
The
heat of vaporization of benzene, C6H6, is 30.8 kJ/mol at its boiling point of
80.1 °C. How much heat
is required to vaporize 128 g benzene at its boiling point? a. | 4.04
kJ | b. | 18.8
kJ | c. | 19.3
kJ | d. | 50.5
kJ | e. | 4.04
´ 103
kJ | | |
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59.
|
Calculate DE for the system in which a gas absorbs 31 J of heat and does 18 J of work on
the surroundings? a. | -49
J | b. | -13
J | c. | +13
J | d. | +31
J | e. | +49
J | | |
|
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60.
|
Determine DH for the following reaction,
N2(g) + 3 H2(g) ® 2
NH3(g)
given the thermochemical equations
below.
N2(g) + O2(g) ® 2 NO(g)
DH =
+180.8 kJ
4 NH3(g) + 5 O2(g) ® 4 NO(g) + 6
H2O(g) DH = -906.2 kJ
2 H2(g) + O2(g) ® 2
H2O(g) DH = -483.6 kJ
a. | -1209.0 kJ | b. | -1189.0
kJ | c. | -756.5
kJ | d. | -241.8
kJ | e. | -91.5
kJ | | |
|
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61.
|
Calculate for
sulfur dioxide,
S(s) + O2(g) ®
SO2(g)
given the thermochemical equations
below.
2 S(s) + 3 O2(g) ® 2
SO3(g) DH° = -791.5 kJ
2
SO2(g) + O2(g) ® 2 SO3(g) DH° = -197.9 kJ
a. | -296.8 kJ/mol | b. | -395.7
kJ/mol | c. | -494.7 kJ/mol | d. | -593.6
kJ/mol | e. | -989.4 kJ/mol | | |
|
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62.
|
Which
of the following chemical equations corresponds to the standard molar enthalpy of formation of
N2O? a. | NO(g) + 1/2
N2(g) ® N2O(g) | b. | N2(g)
+ 1/2 O2(g) ® N2O(g) | c. | 2N(g) + O(g)
®
N2O(g) | d. | N2(g) + O(g) ®
N2O(g) | e. | 2 N2(g) + O2(g) ® 2
N2O(g) | | |
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63.
|
The
standard enthalpy change for the combustion of 1 mole of benzene is -3267.4
kJ.
C6H6(l) + 15/2 O2(g) ® 6 CO2(g) + 3 H2O(l)
Calculate for benzene based on the following standard molar enthalpies of
formation.
molecule | (kJ/mol) | CO2(g) | -393.5 | H2O(l) | -285.8 | | |
a. | -6485.8
kJ | b. | -3946.7
kJ | c. | -3218.4
kJ | d. | +49.0
kJ | e. | +2588.1
kJ | | |
|
|
64.
|
The
standard molar enthalpy of formation of ClF3 is -405 kJ.
1/2 Cl2(g) + 3/2 F2(g) ®
ClF3(g)
The bond energies of Cl2 and F2
are 242 kJ and 155 kJ/mol, respectively. Calculate the energy of an Cl-F bond. a. | 8
kJ/mol | b. | 87 kJ/mol | c. | 207
kJ/mol | d. | 253 kJ/mol | e. | 802
kJ/mol | | |
|
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65.
|
When
heated, azomethane decomposes into nitrogen gas and ethane gas.
CH3N=NCH3(g) ®
N2(g) + C2H6(g)
Bond | Bond Energy
(kJ/mol) | Bond | Bond Energy
(kJ/mol) | C-H | 413 | N-N | 163 | C-N | 305 | N=N | 418 | C-C | 346 | N N | 945 | | | | |
Using average bond energies, calculate the enthalpy of
reaction. a. | -611
kJ | b. | -527
kJ | c. | -429
kJ | d. | -313
kJ | e. | -263
kJ | | |
|
|
66.
|
What
shell contains a total of 9 orbitals? a. | n = 1 | b. | n =
2 | c. | n =
3 | d. | n =
4 | e. | n =
5 | | |
|
|
67.
|
How
many nodal planes exist for a 2p orbital?
|
|
68.
|
Which
of the following diagrams represent d-orbitals?
a. | (I)
only | b. | (II)
only | c. | (III)
only | d. | (IV)
only | e. | (I) and
(IV) | | |
|
|
69.
|
How
many electrons can be described by the following quantum numbers: n = 4, l = 3,
ml = -2, ms = +1/2?
|
|
70.
|
Which
element has the electron configuration
[Ar]3d104s1?
|
|
71.
|
What
is the electron configuration for a lead atom? a. | [Xe]6s26p2 | b. | [Kr]5d106s26p2 | c. | [Xe]4f145d106s26p2 | d. | [Xe]5d106s26p2 | e. | [Kr]4d104f145d2 | | |
|
|
72.
|
Which
element has the following electron configuration?
|
|
73.
|
What
3- ion has the following ground state electron configuration?
a. | oxide
ion | b. | nitride
ion | c. | sodium
ion | d. | aluminum
ion | e. | phosphide
ion | | |
|
|
74.
|
What
2+ ion has the following ground state electron configuration?
a. | Ni2+ | b. | Co2+ | c. | Ca2+ | d. | Cu2+ | e. | Mn2+ | | |
|
|
75.
|
Which
group of the periodic table of elements forms only 2+ ions? a. | group
1A | b. | group
2A | c. | group
7B | d. | group
7A | e. | group
8A | | |
|
|
76.
|
For
an atom of a main group element, the number of valence electrons is equal to a. | its number of
core electrons. | b. | the principle quantum number of its outer
shell. | c. | its period number. | d. | its group
number. | e. | eight minus its group number. | | |
|
|
77.
|
A
silicon atom has ____ valence electrons.
|
|
78.
|
Which
of the following statements are CORRECT?
1. | Ionic bonds form when one or more valence electrons are
transferred from one atom to another. | 2. | Covalent bonds involve sharing of electrons between
atoms. | 3. | Ionic bond
formation is always exothermic; covalent bond formation is always
endothermic. | | |
a. | 1
only | b. | 2
only | c. | 3
only | d. | 1 and
2 | e. | 1, 2, and
3 | | |
|
|
79.
|
How
many lone-pair electrons are on the carbon atom in CO2?
|
|
80.
|
Use
VSEPR theory to predict the molecular geometry of H3O+. a. | trigonal-pyramidal | b. | trigonal-planar | c. | bent | d. | T-shaped | e. | linear | | |
|
|
81.
|
Use
VSEPR theory to predict the electron-pair geometry and the molecular geometry of the nitrite ion,
NO2-. a. | The electron-pair geometry is linear, the molecular geometry is
linear. | b. | The electron-pair geometry is trigonal-planar, the molecular
geometry is bent. | c. | The electron-pair geometry is trigonal-planar, the molecular
geometry is linear. | d. | The electron-pair geometry is tetrahedral, the molecular
geometry is bent. | e. | The electron-pair geometry is tetrahedral, the molecular
geometry is linear. | | |
|
|
82.
|
Which
of the following is a correct Lewis structure for ozone, O3?
|
|
83.
|
Which
of the following is a correct Lewis structure for N2O?
|
|
84.
|
Which
of the following are possible Lewis structures for
C2H6O?
a. | 1 | b. | 2 | c. | 3 | d. | 2 and 3 | e. | 1, 2, and
3 | | |
|
|
85.
|
Which
of the following is a correct Lewis structure for the phosphate ion?
|
|
86.
|
What
is the bond angle in N2O? a. | 90° | b. | 107° | c. | 109.5° | d. | 120° | e. | 180° | | |
|
|
87.
|
How
many sigma (s) bonds and pi
(p) bonds are in
acetic acid?
a. | six s and one
p | b. | six s and two
p | c. | seven
s and one
p | d. | eight
s and zero
p | e. | eight
s and one
p | | |
|
|
88.
|
How
many sigma (s) bonds and pi
(p) bonds are in
formaldehyde, H2CO? a. | one s, one p | b. | two s, two p | c. | three s, one p | d. | three s, two p | e. | four s, one p | | |
|
|
89.
|
What
is the hybridization of the central oxygen atom in ozone, O3? a. | sp | b. | sp2 | c. | sp3 | d. | sp3d | e. | sp3d2 | | |
|
|
90.
|
What
is the hybridization of the central atom in a molecule with a trigonal-planar
geometry? a. | sp | b. | sp2 | c. | sp3 | d. | sp3d | e. | sp3d2 | | |
|
|
91.
|
What
is the molecular geometry around a central atom that is sp3 hybridized and has one
lone electron-pair? a. | bent | b. | linear | c. | trigonal-planar | d. | trigonal-pyramidal | e. | trigonal-bipyramidal | | |
|
|
92.
|
Which
of the underlined atoms (C1, C2, N, and O) are sp2
hybridized?
a. | C1
and C2 | b. | C1, N, and O | c. | N and
O | d. | O and
C2 | e. | O only | | |
|
|
93.
|
If
the volume of a confined gas is quadrupled while its temperature remains constant, what change will
be observed? a. | The pressure of
the gas will decrease to 1/4 its original value. | b. | The pressure of
the gas will quadruple. | c. | The density of the gas will decrease to 1/2 its original
value. | d. | The average velocity of the molecules will
quadruple. | e. | The average velocity of the molecules will
double. | | |
|
|
94.
|
Avogadro's hypothesis states that equal volumes of gases under the same conditions of
temperature and pressure have equal ____. a. | densities | b. | particle
velocities | c. | molar masses | d. | numbers of
particles | e. | masses | | |
|
|
95.
|
Which
of the following relationships are true for gases?
1. | The number of moles of a gas is directly proportional to its
volume (at constant pressure). | 2. | The pressure of a gas is inversely proportional to its
temperature in Kelvins (at constant volume). | 3. | The volume of a gas is directly proportional to its pressure
(at constant temperature). | | |
a. | 1
only | b. | 2
only | c. | 3
only | d. | 1 and
2 | e. | 2 and
3 | | |
|
|
96.
|
The
pressure in a 20.0 L flask is 0.512 atm at 72 °C. How many moles of gas are in the flask? (R = 0.08206
L·atm/mol·K) a. | 0.0297 mol | b. | 0.142
mol | c. | 0.276
mol | d. | 0.362
mol | e. | 1.73
mol | | |
|
|
97.
|
At
453 K and 755 mm Hg, what volume of N2 will react completely with 22.2 L H2 to
produce NH3?
N2(g)
+ 3 H2(g) ® 2 NH3(g)
a. | 7.40
L | b. | 14.8
L | c. | 22.2
L | d. | 44.4
L | e. | 66.6
L | | |
|
|
98.
|
Which
of the following are postulates of kinetic-molecular theory of gases?
1. | The distance between gas molecules is large in comparison to
their size. | 2. | Gas molecules are in constant, random
motion. | 3. | The kinetic
energy of gas particles is proportional to the Kelvin temperature. | | |
a. | 1 only | b. | 2
only | c. | 3
only | d. | 1 and
2 | e. | 1, 2, and
3 | | |
|
|
99.
|
If a
gas effuses 1.618 times faster than Kr, what is its molar mass? a. | 18.02
g/mol | b. | 28.01 g/mol | c. | 32.01
g/mol | d. | 51.79 g/mol | e. | 65.88
g/mol | | |
|
|
100.
|
Non-ideal behavior for a gas is most likely to be observed under conditions
of a. | high temperature
and low pressure. | b. | high temperature and high pressure. | c. | low temperature
and low pressure. | d. | standard temperature and pressure. | e. | low temperature
and high pressure. | | |
|