Download Name: 1) At 1 atmosphere and 298 K, 1 mole of H O(l) molecules

6569 - 1 - Page 1
Name: ____________________________________________
1)
At 1 atmosphere and 298 K, 1 mole of H2 O(l) molecules and
2)
1 mole of C2 H5 OH(l) molecules both have the same
A)
B)
C)
D)
mass
density
average kinetic energy
vapor pressure
Two samples of gold that have different temperatures are
placed in contact with one another. Heat will flow
spontaneously from a sample of gold at 60DC to a sample of
gold that has a temperature of
A) 50DC
B) 60DC
3)
Which kelvin temperature is equivalent to -24DC?
A) 273 K
B) 226 K
4)
C) 70DC
D) 80DC
C) 297 K
D) 249 K
At equilibrium, nitrogen, hydrogen, and ammonia gases form a mixture in a sealed container. The data table below gives some
characteristics of these substances.
Describe how to separate ammonia from hydrogen and nitrogen.
5)
In which equation does the term "heat" represent heat of
fusion?
9)
A) NaOH(aq) + HCl(aq) ‚ NaCl(aq) + H2 O(l) + heat
B) H2 O(l) + heat ‚ H2 O(g)
C) NaCl(s) + heat ‚ NaCl(l)
D) H2 O(l) + HCl(g) ‚ H3 O+(aq) + Cl-(aq) + heat
6)
A) water
B) propanone
10)
Given the particle diagram:
7)
Which grouping of the three phases of bromine is listed in
order from left to right for increasing distance between
bromine molecules?
A) solid, liquid, gas
B) liquid, solid, gas
8)
C) Xe
D) Rn
C) solid, gas, liquid
D) gas, liquid, solid
As the pressure on the surface of a liquid decreases, the
temperature at which the liquid will boil
A) remains the same
B) decreases
C) increases
C) ethanol
D) ethanoic acid
Using your knowledge of chemistry and the information in
the Vapor Pressure of Four Liquids chemistry reference
table, which statement concerning propanone and water at
50DC is true?
A) Propanone has a lower vapor pressure and weaker
intermolecular forces than water.
B) Propanone has a lower vapor pressure and stronger
intermolecular forces than water.
C) Propanone has a higher vapor pressure and weaker
intermolecular forces than water.
D) Propanone has a higher vapor pressure and stronger
intermolecular forces than water.
At 101.3 kPa and 298 K, which element could this diagram
represent?
A) Kr
B) Ag
Based on the Vapor Pressure of Four Liquids chemistry
reference table, which substance has the weakest
intermolecular forces?
11)
Which phase change results in the release of energy?
A) H2 O(g) ‚ H2 O(l)
B) H2 O(s) ‚ H2 O(l)
C) H2 O(l) ‚ H2 O(g)
D) H2 O(s) ‚ H2 O(g)
6569 - 1 - Page 2
12)
The graph below represents the uniform heating of a
substance, starting below its melting point, when the
substance is solid.
15)
Under which conditions of temperature and pressure would
helium behave most like an ideal gas?
A) 750 K and 600 kPa
B) 50 K and 600 kPa
16)
The temperature of a 2.0-liter sample of helium gas at STP is
increased to 27DC and the pressure is decreased to 80. kPa.
What is the new volume of the helium sample?
A) 2.0 L
B) 1.4 L
17)
13)
14)
C) 50 K and 20 kPa
D) 750 K and 20 kPa
C) 2.8 L
D) 4.0 L
At STP, 4 liters of O2 contains the same total number of
molecules as
A) 4 L of CO2
C) 2 L of Cl2
B) 1 L of NH3
D) 8 L of He
Which line segments represent an increase in average
kinetic energy?
Questions 18 and 19 refer to the following:
A) DE and EF
B) AB and BC
The diagram below shows a piston confining a gas in a cylinder.
C) AB and CD
D) BC and DE
Explain, in terms of molecular energy, why the vapor
pressure of propanone increases when its temperature
increases.
18)
Using the set of axes below, sketch the general relationship
between the pressure and the volume of an ideal gas at
constant temperature.
19)
The gas volume in the cylinder is 6.2 milliliters and its
pressure is 1.4 atmospheres. The piston is then pushed in
until the gas volume is 3.1 milliliters while the temperature
remains constant. Calculate the pressure, in atmospheres,
after the change in volume. [Show all work.]
Given the graph below that represents the uniform cooling
of a sample of lauric acid starting as a liquid above freezing
point.
(a)
Which line segment represents a phase change, only?
(b) What is the melting point of lauric acid?
(c)
At which point do the particles of lauric acid have the
highest average kinetic energy?
(d) Name the phase change that takes place during this
10-minute cooling time.
6569 - 1 - Page 3
Questions 20 and 21 refer to the following:
26)
Which electron transition represents a gain of energy?
A)
B)
C)
D)
Cylinder A contains 22.0 grams of CO2 (g) and cylinder B contains
N2 (g). The volumes, pressures, and temperatures of the two gases
are indicated under each cylinder.
27)
What determines the order of placement of the elements on
the modern Periodic Table?
A)
B)
C)
D)
28)
from 3rd to 2nd shell
from 2nd to 3rd shell
from 3rd to 1st shell
from 2nd to 1st shell
the number of neutrons, only
the number of neutrons and protons
atomic number
atomic mass
Which set of symbols represents atoms with valence
electrons in the same electron shell?
A) Ba, Br, Bi
B) Mn, Hg, Cu
29)
20)
Explain why the number of molecules of N2 (g) in cylinder B
is the same as the number of molecules of CO2 (g) in
A) 13
30)
The temperature of the CO2 (g) is increased to 450. K and the
volume of cylinder A remains constant. Show a correct
numerical setup for calculating the new pressure of the
CO2 (g) in cylinder A.
22)
attached to one unit of MgSO4 .]
23)
24)
B) 4
D) 7
31)
A) a hard sphere with negative particles uniformly
embedded
B) a hard sphere with positive particles uniformly
embedded
C) a positive nucleus surrounded by a hard negative shell
D) a positive nucleus surrounded by a cloud of negative
charges
A) decreases
B) increases
32)
33)
C)
B)
D)
34)
filled energy levels
mobile electrons
high ionization energies
high electronegativities
Which change occurs when a barium atom loses two
electrons?
A)
B)
C)
D)
Which Lewis electron-dot diagram represents a boron atom
in the ground state?
C) remains the same
The high electrical conductivity of metals is primarily due to
A)
B)
C)
D)
C) an ion
D) the nucleus
A)
D) 14
When an atom of phosphorus becomes a phosphide ion
(P3-), the radius
The region that is the most probable location of an electron
in an atom is
C) 2
As the elements in Period 2 of the Periodic Table are
considered in succession from left to right, there is a
decrease in atomic radius with increasing atomic number.
This may best be explained by the fact that the
Which of these phrases best describes an atom?
A) the excited state
B) an orbital
25)
C) 5
B) 1
A) number of protons increases, and the number of shells
of electrons increases
B) number of protons increases, and the number of shells
of electrons remains the same
C) number of protons decreases, and the number of shells
of electrons increases
D) number of protons decreases, and the number of shells
of electrons remains the same
What is the total number of oxygen atoms in the formula
MgSO4 d7H2 O? [The d represents seven units of H2 O
A) 11
An unknown element X can form a compound with the
formula XBr3 . In which group on the Periodic Table would
element X be found?
cylinder A.
21)
C) Sr, Sn, I
D) O, S, Te
It becomes
It becomes
It becomes
It becomes
a negative ion and its radius increases.
a negative ion and its radius decreases.
a positive ion and its radius decreases.
a positive ion and its radius increases.
At standard pressure, which element has a melting point
higher than standard temperature?
A) Br2
C) F2
B) Hg
D) Fe
6569 - 1 - Page 4
35)
Which trends are observed when the elements in Period 3
on the Periodic Table are considered in order of increasing
atomic number?
A) The atomic radius decreases, and the first ionization
energy generally increases.
B) The atomic radius increases, and the first ionization
energy generally increases.
C) The atomic radius decreases, and the first ionization
energy generally decreases.
D) The atomic radius increases, and the first ionization
energy generally decreases.
36)
Based on the Properties of Selected Elements chemistry
reference table, which of the following atoms requires the
least energy for the removal of the most loosely bound
electron?
A) Br
B) Sr
37)
The table below shows the electronegativity of selected elements
of Period 2 of the Periodic Table.
41)
C) Be
D) Sn
(a) On the grid below, set up a scale for electronegativity
on the y-axis.
(b) Plot the data by drawing a best-fit line.
Which list consists of elements that have the most similar
chemical properties?
A) K, Al, and Ni
B) K, Ca, and Ga
38)
Questions 41 and 42 refer to the following:
C) Mg, Al, and Si
D) Mg, Ca, and Ba
At 298 K, oxygen (O2 ) and ozone (O3 ) have different
properties because their
A)
B)
C)
D)
39)
atoms have different atomic numbers
atoms have different atomic masses
molecules have different average kinetic energies
molecules have different molecular structures
Which statement correctly describes diamond and graphite,
which are different forms of solid carbon?
A) They do not differ in their molecular structure or
properties.
B) They differ in their properties, only.
C) They differ in their molecular structure and properties.
D) They differ in their molecular structure, only.
40)
Potassium ions are essential to human health. The
(c) Using the graph, predict the electronegativity of
nitrogen.
42)
For the elements in the table, state the trend in
electronegativity in terms of atomic number.
43)
As two chlorine atoms combine to form a molecule, energy
is
movement of dissolved potassium ions, K+(aq), in and out
of a nerve cell allows that cell to transmit an electrical
impulse.
What property of potassium ions allows them to transmit an
electrical impulse in the situation described?
A) released
B) destroyed
44)
Which of the following elements has the least attraction for
electrons in a chemical bond?
A) chlorine
B) fluorine
45)
C) created
D) absorbed
C) nitrogen
D) oxygen
Which of the following solids has the highest melting
point?
A) SO2 (s)
C) H2 O(s)
B) CO2 (s)
D) Na2 O(s)
6569 - 1 - Page 5
46)
What is the correct Lewis electron-dot structure for the
compound magnesium fluoride?
51)
A)
52)
B)
Which formula represents a nonpolar molecule?
A) HCl
C) H2 O
B) CF4
D) NH3
Which Lewis electron-dot diagram is correct for CO2 ?
A)
C)
B)
D)
C)
D)
53)
47)
48)
intermolecular forces
Which compound contains both ionic and covalent bonds?
A) CaCO3
C) PCl3
B) CH2 O
D) MgF2
A solid substance was tested in the laboratory. The test
results are listed below.
Molecules in a sample of NH3 (l) are held closely together by
A)
B)
C)
D)
54)
caused by different numbers of neutrons
existing between ions
caused by unequal charge distribution
existing between electrons
The table below shows the normal boiling point of four
compounds.
d dissolves in water
d is an electrolyte
d melts at a high temperature
Based on these results, the solid substance could be
A) C
B) CuBr2
49)
50)
C) Cu
D) C6 H12 O6
Which molecule contains a triple covalent bond?
A) N2
C) H2
Which compound has the strongest intermolecular forces?
B) Cl2
D) O2
A) HCl(l)
B) CH3 F(l)
Which substance is correctly paired with its type of
bonding?
A) NaBr ‡‡ nonpolar covalent
B) HCl ‡‡ nonpolar covalent
C) Br2 ‡‡ polar covalent
D) NH3 ‡‡ polar covalent
C) HF(l)
D) CH3 Cl(l)
6569 - 1 - Page 6
55)
In the boxes below, draw a correct Lewis electron-dot structure for:
(a) an atom of hydrogen
(b) an atom of nitrogen
(c) a molecule of ammonia (NH3 )
Questions 56 and 57 refer to the following:
62)
A) The boiling point of the solution increases, and the
freezing point of the solution increases.
B) The boiling point of the solution increases, and the
freezing point of the solution decreases.
C) The boiling point of the solution decreases, and the
freezing point of the solution decreases.
D) The boiling point of the solution decreases, and the
freezing point of the solution increases.
Naphthalene, a nonpolar substance that sublimes at room
temperature, can be used to protect wool clothing from being
eaten by moths.
56)
Explain, in terms of intermolecular forces, why naphthalene
sublimes.
57)
Explain why naphthalene is not expected to dissolve in
water.
58)
The solubility of KClO3 (s) in water increases as the
A)
B)
C)
D)
59)
temperature of the solution increases
temperature of the solution decreases
pressure on the solution increases
pressure on the solution decreases
60)
C) sodium nitrate
D) sugar
64)
According to Solubility Curves chemistry reference table,
which solution is saturated at 30DC?
C) 30 grams of NaCl in 200 grams of water
D) 12 grams of KClO3 in 200 grams of water
65)
A student is instructed to make 0.250 liter of a 0.200 M
aqueous solution of Ca(NO3 )2 .
Show a correct numerical setup for calculating the total
number of moles of Ca(NO3 )2 needed to make 0.250 liter of a
C) 2 M
D) 8 M
C) 0.02 ppm
D) 2 ppm
C) 84 g
D) 38 g
A) 30 grams of NaCl in 100 grams of water
B) 12 grams of KClO3 in 100 grams of water
0.200 M calcium nitrate solution.
What is the concentration of a solution, in parts per million,
if 0.02 gram of Na3 PO4 is dissolved in 1,000 grams of water?
A) 20 ppm
B) 0.2 ppm
Based on the Solubility Curves chemistry reference table,
what is the maximum number of grams of KCl(s) that will
dissolve in 200 grams of water at 50DC to produce a
saturated solution?
A) 42 g
B) 58 g
What is the molarity of a solution of NaOH if 2 liters of the
solution contains 4 moles of NaOH?
A) 80 M
B) 0.5 M
61)
63)
At room temperature, the solubility of which solute in water
would be most affected by a change in pressure?
A) carbon dioxide
B) methanol
What occurs when NaCl(s) is added to water?
66)
Sulfur dioxide, SO2 , is one of the gases that react with water
to produce acid rain. According to the Solubility Curves
chemistry reference table, describe how the solubility of
sulfur dioxide in water is affected by an increase in water
temperature.
6569 - 1 - Page 7
Questions 67 and 68 refer to the following:
71)
A student uses 200 grams of water at a temperature of 60DC to
prepare a saturated solution of potassium chloride, KCl.
67)
The solution described is cooled to 10DC and the excess
KCl precipitates (settles out). The resulting solution is
saturated at 10DC. How many grams of KCl precipitated out
of the original solution?
(a) Describe the solubility of CO2 gas in water.
(b) Explain your response to part (a) in terms of the
molecular polarities of CO2 (g) and H2 O(l).
72)
Given the balanced equation:
4Fe(s) + 3O2 (g) ‚ 2Fe2 O3 (s) + 1,640 kJ
68)
According to the Solubility Curves chemistry reference
table, how many grams of KCl must be used to create the
saturated solution described?
Which phrase best describes this reaction?
A)
B)
C)
D)
Questions 69 through 71 refer to the following:
FIZZIES - A SPLASH FROM THE PAST
They're baaack... a splash from the past! Fizzies instant
sparkling drink tablets, popular in the 1950's and 1960's, are now
back on the market. What sets them apart from other powdered
drinks is that they bubble and fizz when placed in water, forming
an instant carbonated beverage.
The fizz in Fizzies is caused by bubbles of carbon dioxide
(CO2 ) gas that are released when the tablet is dropped into water.
73)
When a spark is applied to a mixture of hydrogen and
oxygen, the gases react explosively. Which potential energy
diagram best represents the reaction?
A)
Careful observation reveals that these bubbles rise to the surface
because CO2 gas is much less dense than water. However, not all
of the CO2 gas rises to the surface; some of it dissolves in the
water. The dissolved CO2 can react with water to form carbonic
acid, H2 CO3 .
B)
H2 O(l) + CO2 (aq) ‰Š‹ H2 CO3 (aq)
The pH of the Fizzies drink registers between 5 and 6, showing
that the resulting solution is clearly acidic. Carbonic acid is found
in other carbonated beverages as well. One of the ingredients on
any soft drink label is carbonated water, which is another name for
carbonic acid. However, in the production of soft drinks, the CO2
C)
is pumped into the solution under high pressure at the bottling
plant.
‡‡Brian Rohrig, Excerpted from "Fizzies ‡‡ A Splash from the
Past," Chem Matters, February 1998
69)
What is the only positive ion in an aqueous solution of
carbonic acid?
D)
70)
CO2 is pumped into the soft drink solution under high
pressure. Why is high pressure necessary?
endothermic with DH = -1,640 kJ
endothermic with DH = +1,640 kJ
exothermic with DH = +1,640 kJ
exothermic with DH = -1,640 kJ
6569 - 1 - Page 8
74)
The potential energy diagram below represents a reaction.
75)
Given the potential energy diagram for a chemical reaction:
Which arrow represents the activation energy of the
forward reaction?
A) A
B) B
C) C
D) D
Which statement correctly describes the energy changes
that occur in the forward reaction?
A) The activation energy is 10. kJ and the reaction is
exothermic.
B) The activation energy is 50. kJ and the reaction is
endothermic.
C) The activation energy is 10. kJ and the reaction is
endothermic.
D) The activation energy is 50. kJ and the reaction is
exothermic.
76)
In each of the four beakers shown below, a 2.0-centimeter strip of magnesium ribbon reacts with 100 milliliters of HCl(aq) under
the conditions shown.
In which beaker will the reaction occur at the fastest rate?
A) A
77)
B) B
Which statement best explains the role of a catalyst in a
chemical reaction?
A) A catalyst is added as an additional reactant and is
consumed but not regenerated.
B) A catalyst limits the amount of reactants used.
C) A catalyst changes the kinds of products produced.
D) A catalyst provides an alternate reaction pathway that
requires less activation energy.
C) C
78)
A catalyst is added to a system at equilibrium. If the
temperature remains constant, the activation energy of the
forward reaction
A) remains the same
B) increases
79)
D) D
C) decreases
Which sample has the lowest entropy?
A) 1 mole of KNO3 (s)
C) 1 mole of H2 O(l)
B) 1 mole of H2 O(g)
D) 1 mole of KNO3 (l)
6569 - 1 - Page 9
80)
Systems in nature tend to undergo changes toward
A)
B)
C)
D)
81)
84)
higher energy and higher entropy
lower energy and lower entropy
higher energy and lower entropy
lower energy and higher entropy
N2 O4 (g) ‰Š‹ 2NO2 (g)
Which statement correctly describes this system?
A) The concentrations of N2 O4 and NO2 are both
increasing.
B) The forward and reverse reaction rates are equal.
C) The forward and reverse reaction rates are both
increasing.
D) The concentrations of N2 O4 and NO2 are equal.
In the smelting of iron ore, Fe2 O3 is reduced in a blast
furnace at high temperature by a reaction with carbon
monoxide. Crushed limestone, CaCO3 , is also added to the
mixture to remove impurities in the ore. The carbon
monoxide is formed by the oxidation of carbon (coke), as
shown in the following reaction:
2C + O2 ‚ 2CO + energy
Given the equilibrium reaction at STP:
85)
Liquid iron flows from the bottom of the blast furnace and is
processed into different alloys of iron.
A student adds solid KCl to water in a flask. The flask is
sealed with a stopper and thoroughly shaken until no more
solid KCl dissolves. Some solid KCl is still visible in the
flask. The solution in the flask is
A)
B)
C)
D)
Using the set of axes provided, sketch a potential energy
diagram for the reaction of carbon and oxygen that
produces the carbon monoxide in the situation described.
86)
unsaturated and is not at equilibrium with the solid KCl
saturated and is not at equilibrium with the solid KCl
saturated and is at equilibrium with the solid KCl
unsaturated and is at equilibrium with the solid KCl
Given the reaction at equilibrium:
A(g) + B(g) ‰Š‹ AB(g) + heat
The concentration of A(g) can be increased by
A)
B)
C)
D)
87)
82)
Which statement correctly describes a chemical reaction at
equilibrium?
A) The concentrations of the products and reactants are
equal.
B) The concentrations of the products and reactants are
constant.
C) The rate of the forward reaction is greater than the rate
of the reverse reaction.
D) The rate of the forward reaction is less than the rate of
the reverse reaction.
83)
88)
Which species can conduct an electric current?
A) CH3 OH(aq)
C) NaOH(s)
B) HCl(aq)
D) H2 O(s)
The only positive ion found in an aqueous solution of
sulfuric acid is the
A) sulfate ion
B) hydronium ion
89)
90)
Which statement about a system at equilibrium is true?
A) The forward reaction rate is less than the reverse
reaction rate.
B) The forward reaction rate stops and the reverse
reaction rate continues.
C) The forward reaction rate is greater than the reverse
reaction rate.
D) The forward reaction rate is equal to the reverse
reaction rate.
increasing the concentration of B(g)
adding a catalyst
lowering the temperature
increasing the concentration of AB(g)
Which substance is an Arrhenius acid?
A) Mg(OH)2 (aq)
C) HBr(aq)
B) CH3 CHO
D) LiF(aq)
How are HNO3 (aq) and CH3 COOH(aq) similar?
A)
B)
C)
D)
91)
92)
C) sulfite ion
D) hydroxide ion
They are Arrhenius
They are Arrhenius
They are Arrhenius
They are Arrhenius
acids and they turn blue litmus red.
bases and they turn blue litmus red.
acids and they turn red litmus blue.
bases and they turn red litmus blue.
One acid-base theory states that an acid is
A) an electron donor
C) an OH- donor
B) a neutron donor
D) an H+ donor
Which of these pH numbers indicates the highest level of
acidity?
A) 12
B) 5
C) 10
D) 8
6569 - 1 - Page 10
93)
94)
Which of these 1 M solutions will have the highest pH?
A) NaCl
C) CH3 OH
B) HCl
D) NaOH
100 times the original content
10 times the original content
0.01 of the original content
0.1 of the original content
96)
C) H2 SO4 + Mg(OH)2 ‚ MgSO4 + 2H2 O
D) Na2 CO3 + CaCl2 ‚ 2NaCl + CaCO3
98)
Sulfuric acid, H2 SO4 (aq), can be used to neutralize barium
hydroxide, Ba(OH)2 (aq). What is the formula for the salt
produced by this neutralization?
Which indicator is yellow in a solution with a pH of 9.8?
A) methyl orange
B) thymol blue
Which equation represents a neutralization reaction?
A) Ni(NO3 )2 + H2 S ‚ NiS + 2HNO3
B) NaCl + AgNO3 ‚ AgCl + NaNO3
When the pH of a solution changes from a pH of 5 to a pH
of 3, the hydronium ion concentration is
A)
B)
C)
D)
95)
97)
C) bromthymol blue
D) bromcresol green
A student was given four unknown solutions. Each solution
was checked for conductivity and tested with
phenolphthalein. The results are shown in the data table
below.
99)
A) BaSO3
C) BaS
B) BaSO2
D) BaSO4
What is the molarity of an HCl solution if 20. milliliters of
this acid is needed to neutralize 10. milliliters of a 0.50 M
NaOH solution?
A) 1.0 M
B) 0.50 M
C) 0.25 M
D) 0.75 M
Based on the data table, which unknown solution could be
0.1 M NaOH?
A) A
100)
B) B
C) C
D) D
Four flasks each contain 100 milliliters of aqueous solutions of equal concentrations at 25DC and 1 atm.
(a) Which solutions contain electrolytes?
(b) Which solution has the lowest pH?
(c) What causes some aqueous solutions to have a low pH?
(d) Which solution is most likely to react with an Arrhenius acid to form a salt and water?
(e) Which solution has the lowest freezing point? [Explain your answer.]