Final Exam Review Chemistry
2 11-12
1. Liquid ethanol evaporates readily. Which of
the following statements about this process is wrong? (Ch.
a. Evaporation is a phase
change.
b. The molecules become
separated to relatively great distances during evaporation.
c. The molecules of vapor
have a different chemical composition from those in the liquid.
d. The density of the vapor
is less than that of the liquid.
e. The vapor is much more
compressible than the liquid.
C2H5OH + O2 ® CO2 + H2O + 327
kcal
2. How many moles of CO2 are produced
when 1.0 mole of ethanol burns? (Ch.
a. 0.50 d. 2.0
b. 1.0 e. impossible to determine
c. 1.5
3. When one mole of C2H5OH
burns completely, the volume of O2 consumed, measured at standard
temperature and pressure, is (Ch.
a. Variable d. 44.8 liters
b. 7.5 liters e. 67.2 liters
c. 22.4 liters
4. How many grams of H2O are formed
when one mole of ethanol burns? (Ch.
a. 3.0 grams d.
36 grams
b. 6.0 grams e.
54 grams
c. 18 grams
5. If all the heat evolved from burning 1.0 mole
of ethanol is transferred to 10,000 grams of water, the temperature of the
water will rise approximately (Ch. 10)
a. 8.0 °C d.
430 °C
b. 33 °C e. 327
kcal
c. 43 °C
6. How many moles of gas are present in a sample
which occupies 2.05 liters at 3.0 atm pressure and 27 °C? (Ch.
a. 0.15 moles d.
2.77 moles
b. 0.25 moles e.
3.0 moles
c. 2.05 moles
7. If 100 moles of Mg and 100 moles of O2
are allowed to react to form MgO, the maximum mass of MgO that can be formed is
(Ch.
2 Mg + O2 → 2
MgO
8. Which of the following statements about ionic
and covalent bonding is false? (Ch.
a. Covalent bonds are
formed between atoms having high ionization energies.
b. Ionic bonding results in
substances which form conducting solutions when dissolved in water.
c. In ionic bonding, atoms
gain and lose electrons to obtain the same number as the nearest noble gas.
d. Covalent bonding can
only happen between like atoms.
e. Covalent bonding may
result in single, double or triple bonds.
9. Assume that each of the following reactions
is initially at equilibrium. For which of them will a decrease in pressure
favor increased formation of products? (Ch. 17)
a. H2(g) + I2(g) Û 2 HI(g)
b. 2 NOBr(g) Û 2 NO(g) + Br2(g)
c. H2O(g) +
CuSO4(s) Û CuSO4·2H2O(s)
d. 2 NO(g)
Û N2O4(g)
10. The number of moles of sulfate ion, SO42-,
in 500 mL of a 0.2 M solution of Al2(SO4)3 is (Ch.
a. 0.1 mole d.
0.4 mole
b. 0.2 mole e.
0.5 mole
c. 0.3 mole
11. The incoming heat energy is converted mainly into
potential energy. (
a. (1) d.
(4)
b. (2) e.
(5)
c. (3)
12. The incoming heat
energy is being converted mainly into kinetic energy. (Ch.
a. (1) d.
(4)
b. (2) e.
(5)
c. (3)
13. For each of the
following, determine whether you would use Q=mCDT , DHfus, or DHvap to
calculate the amount of heat energy involved in the change. (Ch.
a. (1) d.
(4)
b. (2) e. (5)
c. (3)
14. The equation for the dissolving of
Ba(NO3)2 in water is which of the following? (Ch. 15)
a. Ba(NO3)2(s) ® Ba2+(aq) + 2
NO3-(aq)
b. Ba(NO3)2(s) ® Ba2+(aq) +
(NO3)2-(aq)
c. Ba(NO3)2(s) ® Ba2+(aq) +
(NO3)22-(aq)
d. Ba(NO3)2(s) ® Ba(NO3)2(aq)
e. Ba2+(aq) +
(NO3)2-(aq) ® Ba(NO3)2(s)
15. Which of the following statements
about the part of the electromagnetic spectrum that is visible is not true? (Ch.
a. The velocity of visible
light is 3.00 x 108 meters/second.
b. The frequency of visible
light can be found by the relationship n = c/l.
c. The higher the frequency
of light, the greater its energy per photon.
d. The longer the
wavelength of light, the greater its energy per photon.
e. Visible light is a very
small part of the entire electromagnetic spectrum.
16. What is the partial pressure of helium
in a mixture that consists of 8.0 g helium gas, He, and 8.0 g of hydrogen gas,
H2, if the total pressure is 1,200 mm Hg? (Ch.
a. 120 mm Hg d.
600 mm Hg
b. 240 mm Hg e.
800 mm Hg
c. 400 mm Hg
17. A 2-cm-thick piece of cardboard placed
over a radiation source would be most effective in protecting against which
type of radiation? (Ch.
A) alpha C)
gamma
B) beta D) x-ray
18. Which of the following atoms has six
valence electrons? (Ch.
A) magnesium (Mg) C) sulfur (S)
B) silicon (Si) D) argon
(Ar)
19. Which of the
following statements about the quantum-mechanical model for the atom is not true? (Ch.
a. Electrons exist only in shells which are a
specific distance from the nucleus, determined by the principal quantum number, n.
b. The principal quantum number, n, is used to describe the energy level
change in which an electron may be found.
c. For every principal quantum number, n, there are n2 orbitals available for electron occupancy.
d. It is often useful to consider the electron’s
wave characteristics rather than its particle characteristics.
e. The quantum-mechanical model tells only the
probability of finding an electron in a given area of space.
20. Given the
generalizations implied by the periodic table, which of the following formulas
is not reasonable? (Ch.
a. SiO2 d.
NO
b. Al2O3 e.
BeF2
c. CO2
21. The mass of a 1.00
liter sample of gas, measured at STP, is found to be 1.96 grams. The gas could
have which of the following formulas? [HINT:
Calculate the moles of gas. Molar mass has these units…. Grams / moles] (Ch.
a. CH4 d. N2
b. NH3 e. CO2
c. NO2
22. Consider two
identical flasks, both at 25 °C and 1 atm pressure. One contains H2
gas and the other O2 gas. Which of the following statements about
the gases contained in the two flasks is not
true? (Ch.
a. The same number of
molecules are contained in each flask.
b. The average kinetic
energy of the molecules in both flasks is the same.
c. The average velocity of
the molecules in both flasks is the same.
d. The flask filled with H2
gas will have a smaller mass than the flask filled with O2 gas.
e. The molecules in both
flasks are in rapid motion.
23. Positive ions are
usually formed by which of the following processes? (Ch.
a. gain of protons by the
nucleus.
b. loss of electrons from
the nucleus.
c. loss of neutrons from
the nucleus.
d. gain of electrons either
inside or outside the nucleus.
e. loss of electrons from
outside the nucleus.
24. Plutonium-238 (238Pu)
undergoes radioactive decay to give ?U as one of products. The other
product and the mass number of the uranium produced are which of the following?
(Ch.
a. an alpha particle (4He)
and 238.
2
b. a beta particle (0e-) and 239
-1
c. a gamma ray and 235
d. an alpha particle (4He)
and 234
2
e. a beta particle (0e-) and 235
-1
25. Which of the
following statements about the periodic table is false? (Ch.
a. Metals are generally
located on the left side of the periodic table, and nonmetals on the right.
b. The elements are
arranged in order of increasing atomic number.
c. Elements in each
vertical column of the periodic table have similar chemical reactions.
d. Elements in each
horizontal row have nearly identical physical characteristics.
e. Elements on the left
side of the periodic table generally form positively charged ions when they
react.
26. Consider Al, As, Ga, Ge. Which of the following
elements has the same Lewis dot structure as silicon? (Ch.
A) germanium (Ge) C) arsenic (As)
B) aluminum (Al) D)
gallium (Ga)
27. Given the reaction at equilibrium
N2O4(g) Û 2 NO2(g) DH = +14.1 kcal
Which of the following
changes would not increase the
concentration of NO2(g)? (Ch.
a. increasing the
concentration of N2O4(g)
b. increasing the volume of
the container
c. decreasing the pressure
on the system
d. addition of a catalyst
e. increasing the
temperature at which the reaction is run
28. Which of the following is not a characteristic of an exothermic
reaction? (Ch.
a. The enthalpy of the
products is greater than that of the reactants.
b. The reaction container
becomes hot.
c. DH is negative.
d. Heat is a product of the
reaction.
e. The reaction will probably
go farther toward completion at low temperatures than at high temperatures.
29. Which of the following would not cause an increase in the volume of a
gas trapped in a syringe with one atm pressure upon it? (Ch.
a. changing to a different
gas of higher molecular weight
b. heating the syringe
c. increasing the amount of
gas in the syringe
d. a sudden, dramatic
decrease in atmospheric pressure
e. placing the syringe in a
vacuum
30. Which of the following electron
configurations for neutral atoms in their lowest energy state is not correct? (Ch.
a. fluorine 1s22s22px22py22pz1
b. rubidium [Kr]
5s1
c. scandium 1s22s22p63s23p64s24px1
d. zinc [Ar]
4s23d10
e. germanium [Ar]
4s23d104px14py1
32. An isotope of krypton, 89Kr,
has a half-life of 3.2 minutes. If the original sample was 100 grams, how many
grams
of the original sample will remain undecayed at
the end of 9.6 minutes? (Ch.
a.
none d.
37.5 g
b.
12.5 g e.
50 g
c. 25 g
33. The isotope 27Al contains
______ protons in its nucleus. (Ch.
a. 13 d.
40
b. 14 e.
none of these
c. 27
34. Two identical containers, one
containing helium gas and the other containing oxygen gas, are at the same
temperature and pressure. Which of the following statements is false? (Ch.
a. The average kinetic
energy of the oxygen molecules is the same as the average kinetic energy of the
helium molecules.
b. The average velocity of the helium molecules
is the same as the average velocity of the oxygen molecules.
c. The oxygen in one container weighs eight
times more than the helium gas in the other container.
d. The number of moles oxygen in one flask is
the same as the number of moles of helium in the other.
e. If both containers
were heated to 100 ºC, the average kinetic energies of both gases would
increase but remain equal to
each other.
35. Which of the following types of
nuclear decay results in an increase in the nuclear charge? (Ch.
a. alpha emission d. positron
emission
b. beta emission e. gamma
emission
c. electron capture
36. Which
element is a liquid at room temperature? (Ch. 3)
a. N2 d.
S
b. Fe e.
Na
c. Hg
37. Oxygen gas can be produced by the
decomposition of potassium chlorate, according this equation:
2 KClO3(s) ® 2 KCl(s) + 3 O2
(g). The oxygen gas is collected over water at 27 °C in a 2.00 liter
container at a total pressure of 760. torr.
The vapor pressure of water at 27 °C is 26.0 torr.
Determine the moles of potassium chlorate that reacted in this experiment. (Ch.
a. 0.0790 moles d.
0.0813 moles
b. 0.119 moles e. 0.0345 moles
c. 0.0527 moles
38. Which of the following is the correct
form of the equilibrium constant expression for the reaction below? (Ch.
NH3(aq) + H2O(l) Û NH4+(aq) +
OH-(aq)
a. K = [NH4+][OH-
b. K = [NH3]
c. K = [NH4+][OH-
d. K = [NH4+][OH-
e. K = [NH3][H2O]/[NH4+][OH-
39. Which atom has the highest ionization
energy? (Ch.
a. Mg b. Be c. Ba d.
Ca e.
Sr
40. One gram (1.00 g) of a gaseous
hydrocarbon occupies 0.821 L at 1.00 atm and 147 °C. The compound is
[HINT: calc moles of the gas using PV=nRT. Solve for molar mass by dividing
grams by moles (g/mole)] (Ch.13)
a. CH4 d.
C2H2
b. C2H4 e.
C3H6
c. C4H8
41. Which type of orbital has the highest
energy? (Ch.
a. 6s b. 5p c. 5s d.
5d e. 4f
42. When acid is added to an active metal,
___________ a flammable gas is produced. (Think about the gas produced when you
added hydrochloric acid to magnesium metal in our lab). (Ch.
a. CO b.
H2 c. OH-
43. Which element in the nitrogen family
is most metallic? (Ch.
a. nitrogen d.
antimony
b. phosphorus e. bismuth
c. arsenic
44. Which of the following is a chemical
property for carbon? (Ch.
a. it is a solid at room
temperature
b. it is not magnetic
c. it has a density of 2.25
g/cm3
d. it undergoes a
combustion to carbon dioxide
e. it boils at 4200 °C
45. In the reaction of
CaO
+ 3 C ® CaC2 +
CO
If 52 grams of CaO are mixed with 27 grams of C,
how many grams of CaC2 can be produced? (Ch.
a. 25 b.
75 c.
57 d. 48 e. 133
46. What is the percentage composition of
N in the fertilizer (NH4)2SO4? [HINT: percent composition is just the mass of the
individual element divided by the mass of the total compound, x 100] (Ch.
a.10.6% b. 7.58% c.
5.30% d. 21.1% e. 37.9%
47. In 0.500 moles of acetic acid, CH3COOH,
there are (Ch.
a. 6.02 x 1023 molecules d. 2.4 x 1024 atoms
b. 1.2 x 1024 molecules e. 4.8 x 1024 atoms
c. 1.8 x 1024
atoms
48. Which one of the following statements
about the periodic table is false? (Ch.
a. The noble gases, the
least reactive of all the elements, are located in the last vertical column to
the far right of the table.
b. Each vertical column of the periodic table
contains elements with similar chemical and physical properties.
c. Metals are generally located on the left side
of the periodic table, and nonmetals on the right.
d. Elements in the same horizontal row of the
table have similar physical characteristics.
e. The alkali metals are located in the first
vertical column at the far left of the table.
49. Which of these involves a chemical
change? (Ch.
a. burning b.
dissolving c. melting d. dilution e. condensation
50. Hydrogen sulfide reacts with oxygen
gas to produce sulfur dioxide and water. What is the sum of the coefficients
for the balanced equation? (Ch.
a. 6 b. 8 c. 9 d.
11 e. 17
51. Which of the following is not a solid at room temperature? (Ch.
a. sodium b.
bromine c. phosphorous d. boron e. silicon
52. Once cubic millimeter is equal to a
volume of (Ch.
a. 1 mL b. 0.01 mL c. 100 mL d. 0.001 mL e.10
mL
53. What is the mass of one platinum atom?
(Ch.
a. 1.6
x 10-22 g d. 195.08 g
b. 3.2
x 10-22 g e.
none of these
c.
5.13
x 10-3 g
54. A 6.12 g sample of silver undergoes a
temperature change from 25.5 °C to 55.0 °C when 10.24 calories of
heat are supplied. What is the specific heat of silver in calories /g °C ? (Ch.
a. 0.0669 b.
0.0567 c. 0.0304 d. 1.67 e. 1.00
55. Which is not true for covalent bonds? (Ch.
a. The pair of electrons is
shared between the two atoms.
b. More than two electrons
can be shared between the two atoms.
c. Covalent bonds usually
do not break in aqueous solutions.
d. One electron in the bond
must come from each atom.
e. Ionic bonds are about as
strong as covalent bonds.
56. Which of the following molecules
contains one triple bond? (Ch.
a. NH3 d. H2CCH2
b. CO e.
HNNH
c. H2CCO
57. Which of the following diatomic
molecules has the greatest bond strength? (Ch.
a. H2 d.
O2
b. F2 e.
HF
c. N2
58. How many atoms are in 160 grams of
diatomic nitrogen gas? (Ch.
a. 6.9 x 1024 d. 9.6 x 1025
b. 3.4 x 1024 e. 1.6 x 1023
c. 1.4 x 1025
59. Which of the following is not a pure substance? (Ch.
a. table salt d.
water
b. milk e.
hydrochloric acid
c. baking soda
60. A phase change from solid to gas
without melting in between is called (Ch.
a. sublimation d.
vaporization
b. freezing e. fusion
c. precipitation
61. Which of the following is a metal? (Ch.
a. B d.
Be
b. C e.
Ge
c. Si
62. The physical state that retains both
volume and shape is (Ch.
a. excited d.
solid
b. gas e.
liquid
c. plasma
63. What is the electron configuration of
a stable magnesium atom? (Ch.
a. 1s22s22p5 d. 1s22s22p63s2
b. 1s22s22p6 e. 1s22s22p63s23p1
c. 1s22s22p63s1
64. The following species S2-,
Cl-, Ar, K+ , all have the same number of (Ch.
a. protons d. neutrons
b. nucleons e. isotopes
c. electrons
65. Which pair of atoms is most likely to
form a covalent chemical bond? (Ch.
a. H and H d. Na and Cl
b. He and Ne e. Li and Br
c. Na and Na
66. Which of the following is likely to
have the largest radius? (Ch.
a. H d.
Rb
b. Mn e.
Ag
c. Cl
67. Which property is not a characteristic of the alkali metals? (Ch.
a. Their chlorides are
water soluble.
b. They react with water to
give off hydrogen gas.
c. They can be found as the
free element in nature.
d. They are all reactive,
readily losing one electron to form ions with a +1 charge.
e. They all have the outer
electron configuration ns1.
68. How many valence electrons are in the
outer shell of a Pb atom? (Ch.
a. 2 d.
5
b. 3 e.
6
c. 4
69. Atmospheric pressure is most often
measured with a (Ch.
a. manometer d.
hydrometer
b. barometer e.
spectrophotometer
c. conductivity apparatus
70. A given mass of gas in a rigid
container is heated from 200 °C to 600 °C. Which of the
following responses best describes what will happen to the pressure of the gas?
(Ch.
a. P will stay the same
b. P will decrease by a
factor of 3
c. P will increase by a
factor of 3
d. P will decrease by a
factor of less than 3
e. P will increase by a
factor of less than 3
71. For the reaction
2 C2H6(g) +
O2(g) ® 4 CO2(g) +
6 H2O(g)
what total volume of products would be
formed from 7 liters of C2H6 and excess oxygen at STP? (Ch.
a. 10 L b. 20 L c. 25 L d. 30 L e. 35 L
72. What is the density of nitrogen gas at
227 °C
and 5.00 atm pressure? [HINT: use PV=nRT to calculate the volume of one mole of
diatomic nitrogen gas. Density is mass divided by volume, so you need to divide
the mass of one mole of the gas by its volume] (Ch.
a. 2.93 g/L d.
3.41 g/L
b. 0.293 g/L e.
1.25 g/L
c. 2.30 g/L
73. A gas has a density of 1.45 g/L at 741
mm Hg and 26.0 °C. What is the molar mass of the gas?
(Use PV=nRT and a volume of 1 L to calculate moles of the gas. Units of molar
mass are grams/mole so divide 1.45 g by the number of moles in 1 L of the gas).
(Ch.
a. 36.5 grams/mole d. 44.0 grams/mole
b. 48.0 grams/mole e. cannot be determined
c. 57.6 grams/mole
74. A container with a volume of 10.0 L
contains 2.80g nitrogen gas, 0.403 g of hydrogen gas, and 79.9 g argon gas.
Calculate the total pressure inside the container at 25 ºC. (Ch.
a. 0.471 atm d.
5.62 atm
b. 6.43 atm e.
2.38 atm
c. 3.20 atm
75. When the following equation is
balanced
Al2(CO3)3
(s) +
HCl(aq) ® AlCl3 +
CO2 + H2O
The sum of the coefficients is (Ch.
a. 7 d.
30
b. 10 e.
none of these
c. 15
76. An element E has the electron
configuration [Kr]4d105s25p2. The formula for
the fluoride of E is most likely (Ch.
a. EF14 d. EF4
b. EF8 e. EF
c. EF6
77. Of the following elements, which needs
three electrons to complete its ns2np6 valence shell? (Ch.
a. Ba d. Ca
b. Si e. P
c. Cl
78. Which of the following groups of
compounds contains no ionic compounds? (Ch. 12)
a. HCN NO2 Ca(NO3)2
b. PCl5 LiBr Zn(OH)2
c. KOH CCl4 SF4
d. NaH CaF2 NaNH2
e. H2O H2S NH3
79. A reaction has an equilibrium constant
= 4.0 x 108 at 25º. When the system is at equilibrium, which of
these represents the “favored” situation? (Ch.
a. Product concentration will be
favored.
b. Reactant concentration will
be favored.
c. Product concentration will equal Reactant
concentration. Neither is favored.
d.. One cannot determine based on this
information.
80. Aluminum has a density of 2.7 g/mL.
How much volume will be occupied by 4.0 moles of aluminum? (Ch.
a. 10. mL d.
40. mL
b. 20. mL e.
80. mL
c. 30. mL
81. What volume is occupied by 4.00 grams
of carbon dioxide gas at a pressure of 0.976 atm and a temperature of 25.0 °C? (Ch.
a. 0.191 L d.
22.8 L
b. 19.1 L e.
2.03 L
c. 2.28 L
82. What is the answer to the correct
number of significant figures? (Ch.
(0.0821)(0.023)(298)
/ 1.5
a. 0.38 d.
0.375
b. 0.4 e.
0.37514227
c. 0.3751
83. When ammonium chloride is heated, two
gases are produced.
NH4Cl(s) ® NH3(g) +
HCl(g)
What is the total volume of gas produced at 793
K and 2.50 atm pressure when 164 grams of ammonium chloride decomposes
completely? (Ch.
a. 160 L d. 173.4 L
b. 27.3 L e. 54.6 L
c. 63.8 L
84. According to collision theory, the
rate of a chemical reaction (how fast the reaction takes place), depends on
several factors. Which one of the factors listed below will make a reaction go
faster or slower? (Ch.
a. The number and strength of
the chemical bonds that must be broken in the reaction.
b. The number of collisions that
are hard enough to break bonds per unit of time.
c. The kinetic energy of the
colliding molecules.
d. The relative amount of
surface area in contact between reactants (increased by stirring or grinding).
e. All of these factors affect the rate of a
reaction.
85. Which electron configuration is
impossible? (Ch.
a. 1s22s22p63s2
b. 1s22s22p62d2
c. 1s22s22p63s23p6
d. 1s22s22p63s1
e. 1s22s22p63s23p64s1
86. Which is a chemical property of chlorine? (Ch.
a. It is yellowish green.
b. It burns in sodium
vapor.
c. It has a density of 3.2
g/L at STP.
d. It dissolves in carbon
tetrachloride.
e. It boils at -34 °C.
87. Which pair is geometrically similar? (Ch.
a. SO2 and CO2
b. PH3 and BF3
c. CO2 and OF2
d. SO2 and O3
e. CO32-
and NH3
88. A metal M, forms an oxide of formula M2O3.
The ground state valence shell electron configuration of the M atom is (Ch.
a. ns2np1 d. ns2
b. 4s13d10 e. ns1
c. ns2np3
89. Which ion is smallest in size? (Ch. 11)
a. Al3+ d.
Na+
b. F- e.
N3-
c. O2-
90. When a metal is heated in a flame, the
flame has a distinctive color. This information was eventually extended to the
study of stars because (Ch.
a. the color spectra of stars indicate which
elements are present.
b. a red shift in star color indicates stars are
moving away.
c. star color indicates absolute distance.
d. it allows the observer to determine the size
of stars.
91. How many total moles of aluminum and
sulfate ions are there per mole of Al2(SO4)3? (Ch.
a. 1 d.
4
b. 2 e.
5
c. 3
92. The molecule CCl2F2
is expected to have what kind of geometry? (Ch.
a. bent d.
trigonal planar
b. tetrahedral e.
pyramidal
c. see-saw
93. An atom has in its nucleus 47 protons
and 60 neutrons. What is the isotope symbol for this element? (Ch.
a. 60Ag
b. 107Nd
c. 13Al
d. 107Ag
94. If the following pairs of elements
form ions, which pair would form an ionic compound of the general formula C2A
(where C = cation and A = anion)? (Ch.
a. sodium and sulfur
b. aluminum and oxygen
c. calcium and bromine
d.
magnesium and sulfur
95. Reading
from left to right across a row of the periodic table, the atomic radius
becomes (Ch.
a. larger, owing to increased nuclear charge that
is only partially shielded by additional valence electrons.
b. smaller, owing to increased nuclear charge
that is only partially shielded by additional valence electrons.
c. smaller, owing to placement of additional
electrons in more strongly bonding (closer) orbitals.
d. larger, owing to placement of additional
electrons in more strongly bonding (closer) orbitals.
96.
Which of the following shows atoms in
expected order of increasing ionization energy? (Ch.
I.
Be,
Mg, Ca
II. B, C, N
III. K, Na, Li
a. I only
b. II only
c.
III
only
d. II and III only
97. A gas mixture is made up of 0.18 moles
of hydrogen gas and 0.72 moles of helium gas. If the total mixture is 4.40 atm,
what is the partial pressure of the helium? (Ch.
a. 0.16 atm
b. 1.60 atm
c.
3.50
atm
d. 0.88 atm
98. A solution containing dissolved solute
is placed between the electrodes of a conductivity apparatus. The bulb is dimly
lit, showing low conductivity. The best explanation for this result is that (Ch.
a. the solution is either a
very dilute solution of a strong electrolyte, or the solute is a weak
electrolyte that doesn’t dissociate much.
b. he solution must be
very dilute.
c. the solution must
contain a weak electrolyte.
d. the solute is a
non-electrolyte.
e. the solution much not be
saturated.
99. How many grams of alcohol are
contained in 467 grams of a mixture of alcohol and water that is 23.0 % alcohol
by mass?
(Ch.
a. 20.30 grams
b. 23.0 grams
c. 359.6 grams
d. 107.4 grams
100. How many atoms of hydrogen are
represented in the following formula? (Ch.
(NH4)2CO3
a. 4 b. 8 c. 24 x 1023
d. 48 x 1023
|
In an
experiment similar to your silver - copper Lab, a student suspended a
silver (Ag) wire in a solution of gold nitrate, (Au(NO3)3,
until the reaction was complete. By the end of the experiment, the mass of
the silver wire had decreased by 2.70 +/- 0.02 g, and 1.64 +/- 0.02 g of
goldhad precipitated. (Atomic wts: Ag=108, Au=197). Use this information to
answer the next 3 questions.
|
101. How many moles of silver is reacted? (Ch.
|
a.
|
0.0250
mole
|
d.
|
0.0400
mole
|
|
b.
|
0.00250
mole
|
e.
|
0.400 mole
|
|
c.
|
2.70 mole
|
||
102. How many moles of gold
precipitated? (Ch.
|
a.
|
0.0832
mole
|
d.
|
1.64 moles
|
|
b.
|
0.00832
mole
|
e.
|
1.20 moles
|
|
c.
|
12.0 moles
|
||
103. Use mole ratios to determine
the most likely equation for the reaction (Ch.
|
a.
|
3 Ag + Au(NO3)3 ® Au + 3 AgNO3
|
d.
|
Ag + Au(NO3)3 ® Au + Ag(NO3)3
|
|
b.
|
Ag + 3
AuNO3 ® AgNO3
+ 3 Au
|
e.
|
2 Ag + Au(NO3)3 ® Au + 2 AgNO3
|
|
c.
|
AgNO3
+ Au ® AuNO3 + Ag
|
||
104. A
cube measures 3.00 cm on an edge and has a mass of 16.23 g. The correct density
is (Ch.
|
a.
|
5.41 g/cm3
|
c.
|
0.601 g/cm3
|
|
b.
|
2.71 g/cm3
|
d.
|
1.80 g/cm3
|
105. How many zeros in 0.00052010
are significant? (Ch.
|
a.
|
1
|
c.
|
5
|
|
b.
|
2
|
d.
|
6
|
106. How
many atoms are there in 4.00 moles of sodium? (Ch.
|
a.
|
6.02 x 1023
atoms
|
c.
|
6.02 x 1026
atoms
|
|
b.
|
1.20 x 1024
atoms
|
d.
|
2.41 x 1024
atoms
|
107. The correct name for Cu2O
is (Ch.
|
a.
|
copper
oxide
|
c.
|
copper
(II) oxide
|
|
b.
|
copper (I)
oxide
|
d.
|
dicopper
monoxide
|
108. Which of the following has the
largest radius? (Ch.
|
a.
|
S
 |
d.
|
K
 |
|
b.
|
Cl-
|
e.
|
Ca
 |
|
c.
|
Ar
|
||
109. 
is the electron configuration for which one of
the following ions? (Ch.11)
is the electron configuration for which one of
the following ions? (Ch.11)|
a.
|
S
 |
d.
|
F
 |
|
b.
|
Ca
|
e.
|
none of
these
|
|
c.
|
Na
|
||
110.
How many lone pairs of electrons are in the Lewis structure for ammonia,
NH3 ? (Ch.
|
a.
|
0
|
d.
|
3
|
|
b.
|
1
|
e.
|
4
|
|
c.
|
2
|
||
111. The electron dot structure of
an atom of phosphorus is (Ch.
|
a.
|
 |
c.
|
 |
|
b.
|
 |
d.
|
 |
112. The electron dot structure for
water is (Ch.
|
a.
|
 |
c.
|
 |
|
b.
|
 |
d.
|
 |
113. The electron dot structure for
Cl is (Ch.
|
a.
|
 |
c.
|
 |
|
b.
|
 |
d.
|
 |
114. How does a neutral atom of
calcium (Ca) become a Ca++ ion? (Ch.
|
a.
|
by gaining
2 protons
|
c.
|
by losing
2 protons
|
|
b.
|
by gaining
2 electrons
|
d.
|
by losing
2 electrons
|
115. Acetylene gas, C2H2,
is produced as a result of the following unbalanced equation. What mass
of acetylene gas is produced from the reaction of 10.0 grams of calcium
carbide, CaC2? (Ch.
CaC2 (s)
+ H2O (l) ® C2H2
(g) + Ca(OH)2 (s)
|
a.
|
24.6
|
d.
|
2.03
|
|
b.
|
10.0
|
e.
|
0.156
|
|
c.
|
4.06
|
||
116. How many grams of K2SO4
(molar mass= 174g/mol) would be needed to prepare 4.00 L of a 0.0510 M solution?
(Ch.
|
a.
|
17.8g
|
d.
|
43.5g
|
|
b.
|
35.5g
|
e.
|
63.8g
|
|
c.
|
71.0g
|
||
117. A solution is prepared by
dissolving 200.1 g of NaOH (molar mass = 40.0 g/mol) in enough water to make
851 mL of solution. Calculate the molarity of the solution. (Ch.
|
a.
|
11.8M
|
d.
|
3.65 M
|
|
b.
|
4.78 M
|
e.
|
4.25 M
|
|
c.
|
5.88 M
|
||
118. A solution is prepared by
dissolving 7.31g of Na2SO4 in enough water to make 225 mL
of solution. Calculate the solution molarity (Ch.
|
a.
|
30.8M
|
d.
|
0.229M
|
|
b.
|
1.64M
|
e.
|
3.11M
|
|
c.
|
0.136M
|
||
119. What are the concentrations of
Na+ ions and S-2
in a 0.209 M Na2S
solution? (Ch.
|
a.
|
Na+
= 0.209 M S-2 = 0.1045 M
|
d.
|
Na+
= 0.1045 M S-2 = 0.1045 M
|
|
b.
|
Na+
= 0.1045 M S-2 = 0.209 M
|
e.
|
Na+
= 0.418M S-2 = 0.209 M
|
|
c.
|
Na+
= 0.209 M S-2 = 0.209 M
|
||
120. Which one of the following
statements about the nuclear model of the atom is false? (Ch.
|
a.
|
The
protons and neutrons in the nucleus are very tightly packed.
|
d.
|
The atom
has no definite boundary.
|
|
b.
|
The
electrons occupy a very large volume compared to the nucleus.
|
e.
|
Almost all
the mass of the atom is concentrated in the nucleus.
|
|
c.
|
The number
of protons and neutrons are always the same in a neutral atom.
|
||
121. If you disregard energy
considerations, which one of the following reactions is not possible? (Ch.
|
a.
|
Na(g) ® Na+(g)
+ electron
|
d.
|
O2-(g) +
two electrons ® O(g)
|
|
b.
|
Ca+ (g) ® Ca++ (g) + electron
|
e.
|
Cl (g) + electron ® Cl- (g)
|
|
c.
|
Al
(g) )
® Al+++ (g) + 3 electrons
|
||
122. What volume of 18.0 M sulfuric
acid is required to prepare 16.5 L of 0.126 M H2SO4? (Ch.
|
a.
|
11.6 mL
|
d.
|
0.264 L
|
|
b.
|
0.116 L
|
e.
|
1.16 L
|
|
c.
|
232 mL
|
||
123. Adding a catalyst generally
speeds up the rate of a reaction by (Ch.
|
a.
|
raising
the activation energy
|
c.
|
raising
the heat of the reaction
|
|
b.
|
lowering the activation energy
|
d.
|
lowering
the heat of the reaction
|
124. If K= 4.5 x 10-11
for a reaction, which of the following would be true? (Ch.
|
a.
|
reactants
are favored at equilibrium
|
|
b.
|
products
are favored at equilibrium
|
|
c.
|
reactants
and products are equally favored at equilibrium
|
|
d.
|
the
reaction proceeds very rapidly
|
125. For the system SO2
(g) + Cl2 (g) ® SO2Cl2 (g) at
equilibrium, adding Cl2 (g) to the reaction container will have
which of the following effects? (Ch.
|
a.
|
the
reaction will shift to the right
|
c.
|
the
concentration of SO2(g) will decrease
|
|
b.
|
the
concentration of SO2Cl2(g) will increase
|
d.
|
all of the
above will occur
|
126. If the equilibrium
concentrations of A(g) + 2 B(g) ® C(g) are found to be [A] = 0.015 M, [B] = 2.0
x 10-4 M, and [C] = 3.0 x 10-9 M, the equilibrium
constant would be (Ch.
|
a.
|
5.0
|
c.
|
1.0 x 10-3
|
|
b.
|
0.20
|
d.
|
9.0 x 10-15
|
127. For the endothermic reaction
A(g) + 2 B(g) ® C(g) , which of the following will drive the
reaction towards the products? (Ch.
|
a.
|
lowering
the temperature
|
c.
|
adding more C(g)
|
|
b.
|
decreasing
the volume
|
d.
|
removing
some A(g)
|
128. The
quantum mechanical model of atoms explains or enables predictions of all except
one of the following characteristics.
Identify the exception. (Ch.
|
a.
|
The probability of an electron being at a given location at any
instant.
|
d.
|
The specific energy levels the electrons can occupy.
|
|
b.
|
The general shape of the electron orbitals
|
e.
|
The frequencies of light absorbed or emitted by gaseous atoms.
|
|
c.
|
The path or trajectory of the electrons.
|
|
|
129. Calculate the total amount of
energy required to change 25.0 g of ice at 0 °C into steam
at 100 °C. (DHfus = 6.02 kJ/mole, DHvap
= 40.6 kJ/mole) (Ch. 14 )
|
a.
|
581 J
|
d.
|
56, 326 J
|
|
b.
|
10,460 J
|
e.
|
75, 210 J
|
|
c.
|
8,931 J
|
||
130. Given the reaction A(g) + B(g) ® C(g) + D(g). You have the gases A, B, C, and D at
equilibrium. Upon adding gas A, the
value of K (Ch.
|
a.
|
increases
because by adding A, more products are made, increasing the product-reactant
ratio
|
|
b.
|
decreases
because A is a reactant so the product-to-reactant ratio decreases
|
|
c.
|
does not
change because A does not figure into the product-to-reactant ratio
|
|
d.
|
does not
change as long as the temperature is constant
|
|
e.
|
depends on
whether the reaction is endothermic or exothermic
|
131. The sharing of electrons in
bond formation always involves (Ch.
|
a.
|
the formation
of positive and negative ions
|
d.
|
Shared
electrons being attracted more by one atom than another.
|
|
b.
|
Formation
of polar molecules.
|
e.
|
Lower
energy content for the bonded than for the unbonded atoms.
|
|
c.
|
Shared
electrons being located equally near the nuclei involved.
|
|
|
132. In which reaction is entropy
expected to be increasing? (Ch.
|
a.
|
I2(g)
® I2(s)
|
c.
|
2O2(g)
+ 2 SO(g) ® SO3(g)
|
|
b.
|
H2O(l) ® H2O(s)
|
d.
|
none of these
|
133. Which of the following shows an
increase in entropy? 10)
|
a.
|
Br2(g)
® Br2(l)
|
c.
|
H2(g) Cl2(g) ® 2 HCl(g)
|
|
b.
|
NaBr(s) ® Na+(aq)
+ Br-(aq)
|
d.
|
2 NO2(g) ® N2O4(g)
|
134. Which of the following
statements would not be included in our kinetic molecular theory of gases? (Ch.
|
a.
|
Molecules
are in constant motion at all temperatures above absolute zero.
|
c.
|
The
temperature is a measure of the potential energy of the molecules.
|
|
b.
|
Kinetic
energy is conserved during molecular collisions.
|
d.
|
The mass
of a gas is the sum of all the masses of the individual molecules.
|
135. In neutral atoms of two different isotopes of the same
element, which one of the following properties is different
in the two isotopes? (Ch.
|
a.
|
Atomic
number
|
d.
|
General
chemical reactions
|
|
b.
|
Number of
electrons
|
e.
|
Number of
protons
|
|
c.
|
Mass
|
||
136. A solution is saturated
when the maximum amount of solute is dissolved in the solvent. If the
solubility of NaCl at
25
ºC is 36.2 g/100 g H2O, what mass of NaCl can be dissolved in 50.0 g of H2O?
(Ch.
|
a.
|
18.1 g
|
c.
|
72.4 g
|
|
b.
|
36.2 g
|
d.
|
86.2 g
|
137. A chemical reaction is most
likely to be spontaneous if (Ch.
|
a.
|
the
potential energy of the system is
lowered and entropy increases.
|
c.
|
potential
energy of the system is lowered and entropy decreases.
|
|
b.
|
potential
energy of the system is increased and
entropy increases.
|
d.
|
potential
energy of the system is increased and entropy decreases.
|
138.
A box measures 3.50 cm x 2.915 cm.
The product of these numbers = 10.2025 cm2. What is the
proper way to report the area of the box? (Ch.
|
a.
|
10.20 cm2
|
c.
|
10 cm2
|
|
b.
|
10.2 cm2
|
d.
|
10. cm2
|
139. The result of 2.350 x (4.0 +
6.311) is, (Ch.
|
a.
|
24
|
c.
|
24.21
|
|
b.
|
24.2
|
d.
|
24.205
|
140. The term that refers to the
reproducibility of a laboratory measurement is (Ch.
|
a.
|
precision
|
c.
|
repeatability
|
|
b.
|
accuracy
|
d.
|
exactness
|
141. The marks on the following
target represent someone who is: (Ch.
|
a.
|
accurate,
but not precise.
|
c.
|
both
accurate and precise.
|
|
b.
|
precise,
but not accurate.
|
d.
|
neither
accurate nor precise.
|
142. How many 1 mg salt tablets can
be made from 1 kg of salt? (Ch.
|
a.
|
1000
|
d.
|
1,000,000
|
|
b.
|
10,000
|
e.
|
10,000,000
|
|
c.
|
100,000
|
||
143. The number of significant
figures in 30500 is (Ch.
|
a.
|
1
|
d.
|
4
|
|
b.
|
2
|
e.
|
5
|
|
c.
|
3
|
||
144.
The number of cubic centimeters (cm3) in 43.0 mL is (Ch.
|
a.
|
43.0 cm3
|
c.
|
0.0403 cm3
|
|
b.
|
4.30 cm3
|
d.
|
cannot
convert between cm3 and mL
|
145.
How many significant figures should be in the measurement of the piece
of wood below? (Ch.
|
a.
|
3
|
c.
|
1
|
|
b.
|
2
|
d.
|
0
|
146. The volume of 400 mL of
chlorine gas at 400 mm Hg is decreased to 200 mL at constant temperature. What
is the new
gas pressure? (Ch.
|
a.
|
400 mm Hg
|
d.
|
600 mm Hg
|
|
b.
|
300 mm Hg
|
e.
|
650 mm Hg
|
|
c.
|
800 mm Hg
|
||
147. What is the equivalent
of 423 Kelvin in degrees Celsius? (Ch.
|
a.
|
–223 ºC
|
d.
|
696 ºC
|
|
b.
|
–23 ºC
|
e.
|
423 ºC
|
|
c.
|
150 ºC
|
||
148. Order these gases in order of
increasing velocity: (Ch.
F2,
Cl2, NO, NO2, CH4
|
a.
|
Cl2 < NO2 < F2 < NO < CH4
|
d.
|
CH4 < NO < F2 < NO2 <
Cl2
|
|
b.
|
Cl2 < F2 < NO2 < CH4 < NO
|
e.
|
F2 < NO < Cl2 < NO2 < CH4
|
|
c.
|
CH4 < NO2 < NO < F2 <
Cl2
|
||
149. Titanium (IV) oxide has the
formula (Ch.
|
a.
|
Ti4O
|
c.
|
Ti(IV)O
|
|
b.
|
TiO4
|
d.
|
TiO2
|
150. The correct name for P2O5 is (Ch.
|
a.
|
phosphorus(II)
oxide
|
d.
|
diphosphorus
pentoxide
|
|
b.
|
phosphorus(V)
oxide
|
e.
|
phosporus
pentoxide
|
|
c.
|
diphosphorus
oxide
|
||
151.
Calculate the pH of a solution with [OH- ]
= 1.0 x 10-9 M. (Ch.
|
a.
|
9
|
d.
|
1
|
|
b.
|
5
|
e.
|
Not enough
information
|
|
c.
|
14
|
||
152.
Is the solution in #151 acidic, basic, or neutral? (Ch.
|
a.
|
acidic
|
c.
|
neutral
|
|
b.
|
basic
|
d.
|
Not enough
information
|
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