Chapters: 15, 16, 19 (We just tested over this)-Solubility, Solutions, and Acids/Bases
-calculate pH, pOH, concentration of H and concentration of OH
-Determine the concentration of an unknown acid or base by using data from a titration
-Read a titration graph to determine equivalence point
-Calculate pH of acids, bases, and salt solutions based on the concentration of hydronium and hydroxide ions
-identify whether and acid/base is strong or weak
-explain the use of indicator
-explain how to change saturation level
-use bond types, temperature, and pressure to predict solubility
-read solubility graphs to determine whether a solution is saturated, unsaturated, or supersaturated
-Given the concentration of a solution, predict its effect on freezing point and boiling point
-predict the conductivity of a solution
-express concentration of a solution in terms of molarity or molality
1. ____ The fact that ice is less dense than water
is related to the fact that ____.
a.
the molecular structure of ice is much
less orderly than that of water
b.
the molecules of ice are held to each
other by covalent bonding
c.
ice has a molecular structure in which
water molecules are arranged
randomly
d.
ice has a molecular structure that is
an open framework held together by
hydrogen bonds
2. ____ Which of the following substances
dissolves most readily in gasoline?
a.
CH
b.
HCl
c.
NH
d.
NaBr
3. ____ Which of these compounds is likely to
have very low solubility in water?
a.
NaCl
b.
HCl
c.
CF
d.
CuSO
4. ____ Which of the following substances is
less soluble in hot water than in cold water?
a.
CO
b.
NaCl
c.
NaNO
d.
KBr
5. ____ Why is a nonpolar substance able to
dissolve a different nonpolar substance?
a.
They have similar attractive forces in
their molecules.
b.
They combine to produce a polar
substance.
c.
There is no attractive force between
them.
d.
Nonpolar substances cannot dissolve
in each other.
6. ____ Which of the following compounds is an
electrolyte in aqueous solution?
a.
methanol
b.
sugar
c.
carbon tetrachloride
d.
sodium hydroxide
7. ____ Which of the following usually makes a
substance dissolve faster in a solvent?
a.
agitating the solution
b.
increasing the particle size of the
solute
c.
lowering the temperature
d.
decreasing the number of particles
8. ____ The solubility of potassium chloride is
at 20 C. What is the maximum
amount of KCl that can dissolve in 200 g of
water at 20 C?
a.
17 g
b.
34 g
c.
68 g
d.
6800 g
9. ____ If the solubility of a particular solute is
at 20 C, which of the following
concentrations would represent a supersaturated
solution of that solute?
a.
at 25 C
b.
at 15 C
c.
at 20 C
d.
at 20 C
10. ____ What is the molarity of 200 mL of
solution in which 2.0 moles of sodium bromide
is dissolved?
a.
2.0M
b.
10M
c.
0.40M
d.
4.0M
11. ____ What is the number of moles of solute in
250 mL of a 0.4M solution?
a.
0.1 mol
b.
0.16 mol
c.
0.62 mol
d.
1.6 mol
12. ____ What mass of sucrose, C H O , is
needed to make 500.0 mL of a 0.200M solution?
a.
34.2 g
b.
100 g
c.
17.1 g
d.
68.4 g
13. ____ How many mL of a 2.0M NaBr solution
are needed to make 200.0 mL of 0.50M NaBr?
a.
25 mL
b.
50 mL
c.
100 mL
d.
150 mL
14. ____ If 2.0 mL of 6.0M HCl is used to make a
500.0-mL aqueous solution, what is the molarity
of the dilute solution?
a.
0.024M
b.
0.24M
c.
0.30M
d.
0.83M
15. ____ What is the number of kilograms of
solvent in a 0.70 molal solution containing 5.0
grams of solute? (molar mass of solute = 30 g)
a.
0.24 kg
b.
2.4 kg
c.
0.11 kg
d.
1.1 kg
16. ____ What is the boiling point of a solution
that contains 3 moles of KBr in 2000 g of water?
(K = 0.512 C/m; molar mass of water = 18 g)
a.
97 C
b.
99.7 C
c.
101.4 C
d.
103 C
17. ____ What is the molality of a solution of
water and KCl if the freezing point of the
solution is –3 C? (K = 1.86 C/m; molar mass
of water = 18 g)
a.
0.6m
b.
1.2m
c.
0.8m
d.
6m
18. ____ Which of the following is a property of
an acid?
a.
sour taste
b.
nonelectrolyte
c.
strong color
d.
unreactive
19. ____ What is a property of a base?
a.
bitter taste
b.
watery feel
c.
strong color
d.
unreactive
20. ____ What are the Brønsted-Lowry acids in
the following equilibrium reaction?
CN + H O
HCN + OH
a.
CN , H O
b.
c.
d.
H O, HCN
CN , OH
H O, OH
21. ____ How much H3PO4 is needed to
neutralize 1 liter of a 0.75M solution of NaOH ?
a.
0.25 mol
b.
0.75 mol
c.
1.0 mol
d.
2.25 mol
22. ____ What is the formula for phosphoric
acid?
a.
H PO
b.
H PO
c.
HPO
d.
HPO
23. ____ What is the best description for a
solution with a hydroxide-ion concentration
equal to 1 10 M?
a.
acidic
b.
basic
c.
neutral
d.
The answer cannot be determined.
24. ____ Which of these solutions is the most
basic?
a.
[H ] = 1 10 M
b.
[OH ] = 1 10 M
c.
[H ] = 1 10 M
d.
[OH ] = 1 10 M
Chapters: 9, 11, 13 (Monday)
-write covalent formulas from names
Ex: Sulfur Dioxide
Ex: Phosphorous Pentabromide
Ex: Dinitrogen Trioxide
- write ionic formulas from names
Ex: Calcium Oxide
Ex: Magnesium Fluoride
Ex: Beryllium Carbonate
Ex: Potassium Phosphate
-write skeleton symbolic equations from word equations
Ex: Zinc and lead (II) nitrate react to form zinc nitrate and lead.
Ex: Aluminum bromide and chlorine gas react to form aluminum chloride and bromine gas.
Ex: Sodium phosphate and calcium chloride react to form calcium phosphate and sodium chloride.
-classify chemical equations (type) based on the bonds present, balance equations
Ex: ____ CaCO3  ____ CaO + ____ CO2
Reaction Type : ______________
Ex: ____ NH3+ ____ H2SO4  ____ (NH4)2SO4
Reaction Type : ______________
Ex: ____ C5H9O + ____ O2  ____ CO2 + ____ H2O
Reaction Type : ______________
Ex: ____ Pb + ____ H3PO4  ____ H2 + ____ Pb3(PO4)2
Reaction Type : ______________
Ex: ____ Li3N + ____ NH4NO3  ___ LiNO3 + ___ (NH4)3N
Reaction Type : ______________
Ex: ____ HBr + ___ Al(OH)3  ___ H2O + ___ AlBr3
Reaction Type : ______________
-Predict the products formed in combustion, single replacement, double replacement, and neutralization, synthesis, and
decompostion reactions
1. C6H12 + O2 
2.
K2CO3 + HCl 
3.
Ca + O2 
4.
Cl2 + LiBr 
5.
MgO
6.
HF + Ca(OH)2 
-Use the reactivity series to predict reactions among substances
1. Ca + H2O
2.
Au + Mg(NO3)2
3.
Al + HCl
-Describe reactants and products in terms of state and solubility, Write complete and net ionic equations
1. _____ AgNO3 (__) + _____ K2CO3 (__)  _____ Ag2CO3 (__) + _____ KNO3 (__)
2. _____ MgBr2 (__) + _____ KOH (__)  _____ KBr (__) + _____ Mg(OH)2 (__)
3. _____ AlCl3 (__) + _____ K3PO4 (__)  _____ KCl (__) + _____ AlPO4 (__)
1. ____Potassium sulfate reacts with barium chloride to form potassium chloride and barium sulfate. Which
symbolic equation correctly represents this balanced double replacement reaction?
a. K2S + BaCl2
KCl + BaS
b. KSO4 + BaCl
KCl + BaSO4
c. K2SO4 + BaCl2
2KCl + BaSO4
d. K2SO4 + Ba(ClO3)2
2KClO3 + BaSO3
2. ____The equation shows a reaction between phosphorous trichloride (PCl3) and water (H2O). How many moles
of hydrogen chloride (HCl) are needed to balance the equation?
a. 1 mole
b. 2 moles
c. 3 moles
d. 6 moles
3. ____A student added a few pieces of mossy zinc (Zn) to a 6.0 molar solution of hydrochloric acid (HCl) and
observed the reaction. What products form from this reaction?
a. Zinc chloride and hydrogen gas
b. Zinc hydroxide and chlorine gas
c. Zinc chlorate and hydrogen
d. Zinc hydride and dichlorine
4. ____Which balanced equation correctly represents the decomposition of potassium chlorate into potassium
chloride and oxygen gas? (Hint: Chlorate is ClO3-1)
a. KClO
KCl + O2
b. 2KClO3
2KCl + 3O2
c. KClO3
KCl + O2
d. 2KClO
2KCl + O2
5. ____Consider this incomplete chemical equation:
What are the products of this equation?
a. BaCl2 and CuCl2
b. BaCuCl2 and Ba
c. BaCl2 and Cu
d. BaCu and Cl2
6. ____ What are the missing coefficients for the skeleton equation below?
Cr(s) Fe(NO ) (aq)
Fe(s) Cr(NO ) (aq)
a.
4, 6, 6, 2
b.
2, 3, 2, 3
c.
2, 3, 3, 2
d.
1, 3, 3, 1
7. ____
a.
b.
c.
d.
In order for the reaction 2Al 6HCl
2AlCl
Al must be above Cl on the activity series.
Al must be above H on the activity series.
Heat must be supplied for the reaction.
A precipitate must be formed.
3H to occur, which of the following must be true?
8. ____ Rewrite the following word equation as a balanced chemical equation. What is the coefficient and symbol
for fluorine?
nitrogen trifluoride
nitrogen fluorine
a.
6F
b.
F
c.
6F
d.
3F
9. ____ What are the correct formulas and coefficients for the products of the following double-replacement
reaction?
RbOH H PO

a.
Rb(PO ) H O
b.
RbPO
2H O
c.
Rb PO
3H O
d.
H Rb PO OH
10. ____ Use the activity series of metals to complete a balanced chemical equation for the following single
replacement reaction.
Ag(s) KNO (aq) 
a.
AgNO
K
b.
AgK NO
c.
AgKNO
d.
No reaction takes place because silver is less reactive than potassium.
11. ____
a.
b.
c.
d.
One of the products when aqueous Na CO reacts with aqueous Sn(NO ) is
NaNO .
NaSn.
Sn(CO ) .
CNO .
12. ____
a.
b.
c.
d.
13. ____
a.
b.
c.
d.
The complete combustion of which of the following substances produces carbon dioxide and water?
C H
K CO
CaHCO
NO
Which of the following elements exists as a diatomic molecule?
neon
lithium
nitrogen
sulfur
Chapters: 10 and 12 (Tuesday)
-Convert between moles and particles using avogadro’s number and dimensional analysis
Ex: How many atoms of Fe are in 2 moles of Fe?
Ex: How many moles of N2 are equivalent to 3.6x1024 molecules?
-calculate molar mass, convert between moles and mass using dimensional analysis
Ex: How many grams of Cl2 are in 4.5 moles of Cl2?
Ex: How many moles of HC2H3O2 are equal to 240 grams of HC2H3O2?
-use dimensional analysis for volume/mole, volume/mass, volume/particle conversions for a single substance
Ex: Considering this balanced chemical equation, how many grams of HgO will be produced when 44 g of Hg react with excess O 2?
Ex: What volume of NH3 at STP is produced if 25.0 g of N2 is reacted with an excess of H2?
N2 + 3H2
2 NH3
-convert between moles and volume for any substance at STP
Ex: How many liters would 5.6 moles of O2 occupy at room temperature?
Ex: How many moles of Cl2 occupy a volume of 90L?
-identify the limiting and excess reagents in a chemical reaction
Ex: In a reaction chamber, 3.0 mol of aluminum is mixed with 5.3 mol Cl2 and reacts. The following chemical equation describes the
reaction:
2Al + 3Cl2
2AlCl3
a.
Calculate the mass of product formed.
b.
What is the limiting reactant?__________________________
-calculate the percent yield of a given chemical reaction
Ex: If 400g of AlCl3 was formed in the reaction above, what is the percent yield?
-describe the four states of matter in terms of the kinetic molecular theory
Ex: Draw the microscopic views of each state of matter
-define temperature and explain how it is related to kinetic energy
Ex: Define temperature
-define pressure and explain how various factors affect it
Ex: Define pressure and name 3 ways to increase the pressure inside a container
-convert between all pressure units using dimensional analysis
Ex: The room is at a pressure of 740 torr, how many atmospheres is this? How many kilopascals?
-Vapor Pressure and Boiling Point
Ex: Define boiling point:
Ex: What is the boiling point on the graph below?
-interpret a phase diagram to identify MP, BP, CP, TP, and state of matter
Label all the points on the graph:
ABCDEFG-
1. ____What is the net ionic equation for the reaction between Pb(NO3)2 and HCl?
a. Pb+2 (aq) + 2 Cl- (aq)
PbCl2 (s)
–
+
b. 2 NO3 (aq) + 2H (aq)
2HNO3 (aq)
c. Pb(NO3)2 (aq) + 2 HCl (aq)
PbCl2 (s) + 2 HNO3 (aq)
+3
–
+
d. Pb (aq) + 2 NO3 (aq) + 2H (aq) + 2 Cl- (aq)
2NO3– (aq) + PbCl2 (s) + 2H+ (aq)
2. ____According to this balanced chemical equation, what volume of C2H2 is required to form 40.0 L of CO2?
a. 20.0 L
b. 44.8 L
c. 80.0 L
d. 100 L
3. ____Raphael is studying the movement of water molecules as ice changes from a solid to liquid water. Which
statement best describes the changes in the movement of the water molecules as heat causes the ice to melt?
a. The molecules in the solid stay tightly connected and do not move. As heat is added, the molecules in
the liquid move far apart and do not interact.
b. The molecules in the solid move freely around one another and do not interact. As heat is added, the
molecules are pushed closer together and begin to interact with one another.
c. The molecules in the solid are in a rigid lattice and vibrate more rapidly. As the ice melts, the molecules
in the liquid move more freely but are still attracted to each other.
d. The molecules in the solid are unmoving in a rigid lattice. As the ice melts, the molecules start to vibrate,
and then release from the lattice structure, moving freely as they drift farther apart to form a liquid.
8. The equation represents methane gas (CH4)
4. ____During an investigation, 0.500 moles of
sulfur react with excess oxygen. Based on
the equation, how many liters of
sulfur dioxide should be produced at
standard temperature and pressure (STP)?
S8(s) + 8O2(g)
8SO2(g)
a. 1.40 liters
b. 11.2 liters
c. 256 liters
d. 89.6 liters
5. ____ How many moles of tungsten atoms are
in 4.8 10 atoms of tungsten?
a.
8.0 10 moles
b.
8.0 10 moles
c.
1.3 10 moles
d.
1.3 10 moles
6. ____ How many atoms are in 0.075 mol of
titanium?
a.
1.2 10-25
b.
2.2 10
c.
6.4 10
d.
4.5 10
7. ____ What is the molar mass of (NH ) CO ?
a.
144 g
b.
138 g
c.
96 g
d.
78 g
burning in oxygen gas (O2). If 32 grams of
methane are burned, how many grams of
carbon dioxide (CO2) are produced? ____
CH4(g) + 2O2(g)
a.
b.
c.
d.
CO2(g) + 2H2O(g)
88 grams
56 grams
44 grams
28 grams
9. ____ What is the number of moles in 432 g
Ba(NO ) ?
a.
0.237 mol
b.
0.605 mol
c.
1.65 mol
d.
3.66 mol
10. ____ What is the volume, in liters, of 0.500
mol of C H gas at STP?
a.
0.0335 L
b.
11.2 L
c.
16.8 L
d.
22.4 L
11. ____ What is the number of moles in 9.63 L
of H S gas at STP?
a.
0.104 mol
b.
0.430 mol
c.
3.54 mol
d.
14.7 mol
12. ____ In a chemical reaction, the mass of the
products
a.
is less than the mass of the reactants.
b.
is greater than the mass of the
reactants.
c.
is equal to the mass of the reactants.
d.
has no relationship to the mass of the
reactants.
13. ____ How many moles of aluminum are
needed to react completely with 1.2 mol of FeO?
2Al(s) + 3FeO(s)  3Fe(s) + Al O (s)
a.
1.2 mol
b.
0.8 mol
c.
1.6 mol
d.
2.4 mol
14. ____ When iron rusts in air, iron(III) oxide is
produced. How many moles of oxygen react
with 2.4 mol of iron in the rusting reaction?
4Fe(s) + 3O (g)  2Fe2O (s)
a.
1.2 mol
b.
1.8 mol
c.
2.4 mol
d.
3.2 mol
15. ____ At STP, how many liters of oxygen are
required to react completely with 3.6 liters of
hydrogen to form water?
2H (g) + O (g)  2H O(g)
a.
1.8 L
b.
3.6 L
c.
2.0 L
d.
2.4 L
16. ____ The equation below shows the
decomposition of lead nitrate. How many grams
of oxygen are produced when 11.5 g NO is
formed?
a.
b.
c.
d.
1.00 g
2.00 g
2.88 g
32.0 g
17. ____ How many moles of H PO are
produced when 71.0 g P O reacts completely
to form H PO ?
a.
b.
c.
d.
0.063 5 mol
1.00 mol
4.00 mol
16.0 mol
18. ____ Glucose, C H O , is a good source of
food energy. When it reacts with oxygen, carbon
dioxide and water are formed. How many liters
of CO are produced when 126 g of glucose
completely react with oxygen?
C H O (s) + 6O (g)
6CO (g) + 6H O(l) +
673 kcal
a.
4.21 L
b.
5.33 L
c.
15.7 L
d.
94.1 L
19. ____ How many grams of chromium are
needed to react with an excess of CuSO to
produce 27.0 g Cu?
2Cr(s) + 3CuSO (aq)
Cr (SO ) (aq) +
3Cu(s)
a.
14.7 g
b.
18.0 g
c.
33.2 g
d.
81.5 g
20. ____ How many liters of NH , at STP, will
react with 5.3 g O to form NO and water?
4NH (g) + 7O (g)
4NO + 6H O(g)
a.
0.004 23 L
b.
2.12 L
c.
3.03 L
d.
6.49 L
21. ____ Identify the limiting reagent and the
volume of CO formed when 11 L CS reacts
with 18 L O to produce CO gas and SO gas
at STP.
CS (g) + 3O (g)
CO (g) + 2SO (g)
a.
CS ; 5.5 L CO
b.
O ; 6.0 L CO
c.
CS ; 11 L CO
d.
O ; 27 L CO
22. ____ Metallic copper is formed when
aluminum reacts with copper(II) sulfate. How
many grams of metallic copper can be obtained
when 54.0 g of Al react with 319 g of CuSO ?
Al + 3CuSO
Al (SO ) + 3Cu
a.
21.2 g
b.
127 g
c.
162 g
d.
381 g
Chapters: 14 (Wednesday)
-Calculate n, T, P, or V of a gas based on changes in another component, Calculate the total pressure of a mixture
of gases
1.
If I place 3 moles of N2 and 4 moles of O2 in a 35L container at a temperature of 25°C, what will the
pressure of the resulting mixture be?
2.
Nitrogen gas occupies has a volume of 500ml at a pressure of 0.971atm. What volume will the gas occupy
at a pressure of 1.50 atm, assuming the temperature remains constant?
3.
A sample of argon has a volume of 0.43 mL at 299K. At what temperature in degrees Celsius will it have a
volume of 1 mL?
4.
In a closed container at 1.0 atm, the temperature of a sample of gas is raised from 300K to 400K. What
will the final pressure of the gas be?
5.
When a supply of hydrogen gas is held in a 4 liter container at 320 K it exerts a pressure of 800 torr. The
supply is moved to a 2 liter container, and cooled to 160 K. What is the new pressure of the confined gas?
6.
If I contain 3 moles of a gas in a container with a volume of 60 liters and at a temperature of 400K what is
the pressure inside the container?
-compare and contrast real and ideal gases
Ex: What are the conditions (temperature and pressure) for an ideal gas?
Ex: In what ways could a real gas differ?
-Identify the components of redox reactions and write half-reactions
Ex: Label the oxidation number for each of the elements in the reaction below. Then, identify the element being
oxidized and the element being reduced.
Mg + AlCl3
MgCl2 + Al
1. ____The graph of the results of a scientific study on water was
a chemistry handbook. What is the independent variable in the
A.
B.
C.
D.
found in
study?
molar mass
melting point
vapor pressure
temperature
2. ____A student observed that the rate of a chemical reaction increased as the temperature of the system
increased. Which of the following statements best explains why thermal energy caused an increase in the
reaction rate?
a. The surface area of the product particles decreased.
b. The collision rate of the reactant particles increased.
c. The concentrations of the reactant particles increased.
d. The concentrations of the product particles decreased.
3. ____The boiling point of water is lower on a mountaintop than at sea level. This means that it takes less thermal
energy for water molecules on a mountaintop to
a. Break into atoms
b. Break into molecules of hydrogen and oxygen gas
c. Overcome the attraction of other water molecules
d. Overcome the force of gravity
4. ____Liquid iron vaporizes at a temperature of 2,750°C. Which statement correctly describes the changes that
occur at the atomic level when a sample of iron reaches this temperature?
a. The iron atoms start losing electrons.
b. The distances between iron atoms increase dramatically as the atoms break free of one another.
c. The velocity (speed) with which the gas particles hit the container wall increases.
d. The frequency with which the gas particles hit the container wall increases.
5. ____Gas pressure is caused by
a. Gas molecules heating up
b. Gas molecules reacting with other gas molecules
c. Gas molecules hitting the walls of a container
d. Gas molecules hitting other gas molecules
6. ____Based on the phase diagram for carbon dioxide, which
change in conditions will result in carbon dioxide changing
from a liquid into a gas?
a. [-10°C, 73 atmospheres]
1.00 atmospheres]
b. [-90°C, 1.00 atmosphere]
1.00 atmosphere]
c. [0°C, 5.11 atmospheres]
d. [-68°C, 1.00 atmosphere]
5.11 atmospheres]
[-10°C,
[-56.4°C,
[0°C, 73 atmospheres]
[-68°C,
7. ____A real gas behaves least like an ideal gas under which of the following conditions?
a. Low temperature and low pressure
b. Low temperature and high pressure
c. High temperature and low pressure
d. High temperature and high pressure
8. ____The Cartesian diver pictured to the right contains 1.2 milliliters of air and floats in a plastic bottle filled with
water. The student compresses the bottle, increasing the pressure from 1.0 to 1.5
atmospheres. What is the new volume of air in the Cartesian diver?
Hint: P1V1 = P2V2
a. 0.30 milliliters
b. 0.60 milliliters
c. 0.80 milliliters
d. 1.8 milliliters
9. ____What would be the volume of 2.50 moles of an ideal gas at 600. K and 5.00 atmospheres?
Use: R = 0.0821
Hint: PV = nRT
e. 4.50 liters
f. 11.2 liters
a. 24.6 liters
b. 280 liters
10. ____A student varied the pressure on a sample of air and observed the
volume. The temperature was kept constant at 20°C. The student
graphed the results. Which value is the best prediction for the volume
of the air in this experiment at 16.0 atmospheres (atm)?
Hint: P1V1 = P2V2
a. 0.75 milliliters
b. 1.3 milliliters
c. 3.8 milliliters
d. 5.0 milliliters
11. ____ Particles in a gas are best described as
a.
slow-moving, kinetic, hard spheres.
b.
spheres that are in fixed positions when trapped in a container.
c.
small, hard spheres with insignificant volumes.
d.
hard spheres influenced by repulsive forces from other spheres.
12. ____ The pressure of a gas in a container is 152 mm Hg. This is equivalent to
a.
0.2 atm.
b.
2 atm.
c.
0.3 atm.
d.
0.4 atm.
13. ____ What happens to the average kinetic energy of the particles in a sample of matter as the temperature of the
sample is increased?
a.
The average kinetic energy decreases.
b.
The average kinetic energy increases.
c.
The average kinetic energy does not change.
d.
The change in average kinetic energy cannot be determined.
14. ____ What happens to the temperature of a liquid as it evaporates?
a.
It increases.
b.
It decreases.
c.
It does not change.
d.
The change cannot be determined.
15. ____
a.
b.
c.
d.
What happens to the rate of evaporation of a liquid as the liquid is cooled?
It increases.
It decreases.
It does not change.
The change cannot be determined.
16. ____
a.
Why does the pressure inside a container of gas increase if more gas is added to the container?
There is an increase in the number of collisions between particles and the walls of
the container.
There is an increase in the temperature of the gas.
There is a decrease in the volume of the gas.
There is an increase in the force of the collisions between the particles and the
walls of the container.
b.
c.
d.
17. ____
a.
b.
c.
d.
If the volume of a container of gas is reduced, what will happen to the pressure inside the container?
The pressure will increase.
The pressure will not change.
The pressure will decrease.
The pressure depends on the type of gas.
18. ____
a.
b.
c.
d.
What happens to the temperature of a gas when it is compressed?
The temperature increases.
The temperature does not change.
The temperature decreases.
The temperature becomes unpredictable.
19. ____ If a balloon is heated, what happens to the volume of the air in the balloon if the pressure is constant?
a.
It increases.
b.
It stays the same.
c.
It decreases.
d.
The change cannot be predicted.
20. ____ If a balloon is heated, what happens to the pressure of the air inside the balloon if the volume remains
constant?
a.
It increases.
b.
It stays the same.
c.
It decreases.
d.
The change cannot be predicted.
21. ____ Which law can be used to calculate the number of moles of a contained gas?
a.
Boyle’s law
b.
combined gas law
c.
ideal gas law
d.
Charles’s law
22. ____ Under what conditions of temperature and pressure is the behavior of real gases most like that of ideal
gases?
a.
low temperature and low pressure
b.
low temperature and high pressure
c.
high temperature and low pressure
d.
high temperature and high pressure
23. ____ Which of the following gases will effuse the most rapidly?
a.
bromine
b.
chlorine
c.
ammonia
d.
Hydrogen
Chapters 17 (Thursday)
- graph energy changes of the reactants and products during chemical reactions, differentiate between activation energy in endo vs
exothermic reactions
Ex: Define endo and exothermic then draw energy coordinate diagrams for each. Label the activation energy, ΔH, and state
whether the ΔH would be positive or negative.
a.
Endothermic:
b.
Exothermic:
Ex: Is the forward activation energy of an endothermic reaction greater or the reverse activation energy? Explain.
-describe chemical reactions with energy as a reactant or product
For each of the reactions below, rewrite the reaction with heat correctly placed as a reactant or product
a. H2(g) + 1/2 O2(g) H2O (l)
–286 kJ/mol
b.
H2O(l)  H2O(g)
44 kJ/mol
-differentiate endo/exothermic reactions using enthalpy values
Ex: For each of the reactions above, state whether the reaction was endo or exothermic.
1.
2.
-graph and compute the energy changes that occur between state changes
1. Ex: Draw the temperature versus heat (or time) graph for Sulfur. State what is happening in each of the 4 parts of the
graph and label the melting point at 115°C and the boiling point at 445°C.
-solve problems involving heat flow and temperature changes by using known values of specific heat and latent heat of phase change
Heat of Fusion
54 J/g
Heat of Vaporization
1406 J/g
Specific Heat
3.4 J/g°C
a.
Calculate the energy needed to raise the temperature from 100°C to the melting point, 115°C __________
b.
Calculate the energy needed to melt the solid sulfur__________________
c.
Calculate the energy needed to raise the liquid sulfur from 115°C to the boiling point, 445°C __________
-calculate the heat of reaction using graphs or data
Ex: Carbon tetrachloride can be formed by reacting chlorine with methane:
CH4 + 2 Cl2  CCl4 + 2 H2
Given that the heat of formation of methane is –75 kJ/mol and the heat of formation of carbon tetrachloride is
determine the heat of reaction.
Ex: What would the ΔH be if we began with 3 moles of CH4?
-build and use a coffee cup calorimeter or bomb calorimeter
Ex: Define calorimetry and describe how we measure it. (Draw a picture of how each setup works)
-135 kJ/mol,
1. ____The graph shows the potential energy curve for the hypothetical reaction
A+B
a.
b.
c.
d.
C + D. Which conclusion is supported by this graph?
The reaction is exothermic with an activation energy of 250 kilojoules.
The reaction is endothermic with an activation energy of 50 kilojoules.
The reaction is endothermic with an activation energy of 250 kilojoules.
The reaction is exothermic with an activation energy of 50 kilojoules.
2. ____A research team heats a substance with unknown properties at a constant rate in a
sealed container. The team concludes that the substance boiled during this time. Is the
information provided by the graph sufficient to support this conclusion?
a. Yes, because there is a period without temperature change while heat increases
b. Yes, because the periods of rising temperature reflect two different heat
capacities.
c. No, because substances in sealed containers cannot boil.
d. No, because the data indicate only that a phase change took
place.
3. ____A student did an experiment to find the heat of reaction of
hydrochloric acid and sodium hydroxide using a foam cup calorimeter.
Data from the experiment and a chemistry handbook are shown in the
table. Which value is closest to the amount of energy, in joules, produced
by the reaction? Hint: Q = mc(Tf – Ti )
a. 170 Joules
b. 690 Joules
c. 1,400 Joules
d. 8.300 Joules
4. ____Which graph depicts energy changes characteristic of an
endothermic reaction?
a.
b.
c.
d.
5. ____A sample of ice at -10°C is converted to liquid water at 10°C by adding energy at a constant rate. Which
heating curve shows the temperature changes that should occur in this process?
c.
a.
d.
b.
6. ____ How much ice at 0°C could be melted by the addition of 15 kJ of heat? ( Hfus = 6.01kJ/mol)
a.
0.4 g
c.
7.2 g
b.
2.5 g
d.
45 g
7. ____ How much water at 100°C could be vaporized by the addition of 120 kJ of heat? ( Hvap = 40.7 kJ/mol)
a.
2.9 g
c.
53 g
b.
6.1 g
d.
87 g
8. ____ Which statement correctly describes the energy of the chemical bonds of the reactants in an exothermic
reaction?
a.
equal to the energy stored in the bonds of the products
b.
greater than the energy stored in the bonds of the products
c.
less than the energy stored in the bonds of the products
d.
independent of the energy stored in the bonds of the products
9. ____
a.
B
c.
d.
What do you know about a chemical reaction if the value of H is positive?
The reaction is exothermic.
The reaction is endothermic.
The reaction occurs without the addition of energy.
The reaction cannot occur at room temperature.
10. ____ What is the specific heat of a substance if 1560 cal are required to raise the temperature of a 312-g sample
by 15 C?
a.
c.
0.033
0.99
b.
0.33
d.
1.33
11. ____ One mole of hydrogen is burned in oxygen to produce water in the gas phase, H = 285.8 kJ. What is
the energy change when 1 mole of water, in the gas phase, decomposes to form hydrogen and oxygen?
a.
142.9 kJ of heat is absorbed.
c.
142.9 kJ of heat is released.
b.
285.8 kJ of heat is absorbed.
d.
285.8 kJ of heat is released.
12. ____ Calculate H for the reaction of sulfur dioxide with oxygen.
2SO (g) + O
(g)
2SO (g)
( H SO (g) = –296.8 kJ/mol; H SO (g) = –395.7 kJ/mol)
a.
–98.9 kJ
b.
–197.8 kJ
c.
98.9 kJ
d.
197.8 kJ
13. ____ Calculate the energy released when 24.8 g Na O reacts in the following reaction.
Na O(s) + 2HI(g)
2NaI(s) + H O(l)
H = –120.00 kcal
a.
0.207 kcal
b.
2.42 kcal
c.
48.0 kcal
d.
3.00 10 kcal
14. ____ Calculate H for the following reaction.
C H (g) + H (g)
C H (g)
( H for C H (g) = 52.5 kJ/mol; H for C H (g) = –84.7 kJ/mol)
a.
–137.2 kJ
b.
–32.2 kJ
c.
32.2 kJ
d.
137.2 kJ
15. ____The reaction that produces ammonia (NH3) is reversible.
N2 + 3H2
2NH3 + 92.4 kJ
The reverse reaction should be classified as an
a. Exothermic combination (synthesis) reaction
b. Endothermic combination (synthesis) reaction
c. Exothermic decomposition reaction
d. Endothermic decomposition reaction
16. ____The heat of fusion of sodium is 2.598 kilojoules per mole. How much heat energy does it
take to liquefy 46.00 grams of solid sodium at its melting point?
a. 2.598 kilojoules
b. 5.196 kilojoules
c. 17.71 kilojoules
d. 119.5 kilojoules
17. ____A chemical reaction occurs in 250 grams of solution within a coffee cup calorimeter. The
temperature of the solution drops from 22.4°C to 19.8°C during the reaction. The specific heat
of the solution is 4.15 J/g*°C. How much heat energy did the solution lose?
Hint: Q = mc(Tf – Ti )
a. 2,100 Joules
b. 2,700 Joules
c. 21,000 Joules
d. 23,000 Joules
Suppose that 1 gram (g) of Material A, initially a liquid, is kept in a cylinder fitted with a piston at a
constant pressure of 1 atmosphere (atm). Table 1 and Figure 1, respectively, show how Material A's
volume and temperature vary over time as Material A absorbs heat at a rate of 10 calories per second
(cal/sec). Table 2 gives the boiling points of liquid Materials B–D at 1 atm; the heat absorbed refers to
the amount of heat that is needed to turn
1 g of a liquid at its boiling point into a gas.
Time
(sec)
Volume of Material
A (cm3)
0
2
4
6
8
10
12
14
16
18
20
22
24
1
1
136
271
406
541
676
811
946
1,081
1,216
1,351
1,541
Table 1
Material
Boiling point
(°C)
Heat
absorbed
(cal)
B
C
D
13
19
28
500
610
270
Table 2
Figure 1
1. Based on Figure 1, Material A's temperature increased
the fastest during which of the following time
intervals?
5. Suppose 1 g of Material D at –10°C is heated at the
rate of 10 cal/sec and kept at 1 atm until all of the
liquid is vaporized. Based on Figure 1 and Table 2, a
plot of Material D's temperature versus time would be
best represented by which of the following graphs?
A. 0– 2 sec
B. 2–12 sec
C. 12–22 sec
D. 22–24 sec
2. Suppose 1 g samples of liquid Materials A–D are just
beginning to boil. If each of the liquids absorbs heat at
the rate of 10 cal/sec while kept at 1 atm, which of the
liquids will be the first to be completely turned into a
gas?
A.
A. Material A
B. Material B
C. Material C
D. Material D
B.
3. Table 1 and Figure 1 best support which of the
following hypotheses about the temperature and
volume of Material A ?
(Note: Pressure is assumed to stay constant.)
F. If liquid Material A is in contact with gaseous
Material A and the volume of the gas increases, the
gas's temperature will increase.
G. If liquid Material A is in contact with gaseous
Material A and the volume of the gas increases, the
gas's temperature will decrease.
H. When the temperature of gaseous Material A
increases, its volume will increase.
J. When the temperature of liquid Material A
increases, its volume will increase.
4. Based on the passage and Table 1, what was the
density of liquid Material A ?
F. 0.5 g/cm3
G. 1 g/cm3
H. 5 g/cm3
J. 10 g/cm3
C.
D.