Download Chemistry Log Books - Social Circle City Schools

Chemistry Log Books
Preparation for the Gateway and GHSGT
INTRODUCTION TO CHEMISTRY LOG BOOKS
At the end of second semester this year, all students in the tenth grade attending Gwinnett County Schools
must earn the minimum acceptable score on the county’s science Gateway test in order to be granted their diploma
from a Gwinnett County High School. During their junior year, all students in Georgia are required to take and
pass the Georgia High School Graduation Test (GHSGT) in science. Students must pass this test in order to
graduate as well. To help students prepare for these high-stakes tests, log books are being required in many science
classes here at Berkmar; these log books can be saved from year to year to help you refresh your memory of the
AKS learned in each science class.
OBJECTIVES OF THE CHEMISTRY LOG BOOKS
1. To review all the chemistry Academic Knowledge and Skills (AKS).
2. To prepare a chemistry log book that should be saved and used to prepare for the science portion of the Gwinnett
County Gateway test given during the sophomore year.
3. To prepare a chemistry log book that should be saved and used to prepare for the science portion of the GHSGT
given during the junior year.
ORGANIZATION OF THE REVIEW SHEETS
At the top of each AKS review sheet page, the appropriate AKS correlations are listed. This enables the
students and their parents to understand the state and local requirements. After the solid black line, the review
questions for the unit are listed. Students can answer these questions in any format they choose. It is recommended
that students use some sort of bulleted list or graphic organizer to answer the question. These tend to be more
useful and the student is more likely to use the book to study for the end of semester final exam, the Gateway test,
and the GHSGT.
STUDENT INSTRUCTIONS FOR THE ASSIGNMENT
1. Students will receive an AKS review sheet for the upcoming unit (usually after the last unit test).
This sheet should then be glued/taped to fit the page in the composition log book. Students will read
the AKS listed at the top of the page to see what they will be learning in the upcoming unit.
2. Students will answer the AKS review sheet questions located below the solid black line. Questions will be
answered in the log book. Answers must be placed on the next blank page following the AKS review sheet
questions. Answers are not to be written on the AKS review sheet that is glued/taped to fit the page in the log
book. You may write on the back of pages in the log book.
3. Students will handwrite all answers in blue or black ink only; answers are NOT to be typed.
4. Students will need to place tabs between each section and clearly label on the tab what is covered in that section.
Placing labeled tabs between each section is an organizational tool that will help you when you begin to study for
the Gateway and GHSGT.
5. Students will turn in log books on test days, and the log book will be taken for a daily grade.
DO’s and DON’Ts
 Do place your name on the outer cover in permanent ink!
 Do be NEAT. Points will be lost for: lack of neatness, overhanging papers, messing cutting, messy taping,
etc. Directions must be followed every time – or points will be lost EVERY TIME!
 Do answer all the questions, and answer them correctly. When second semester of your junior year arrives,
and it is time to study for the GHSGT, you will appreciate the fact that you answered all of the questions
correctly when you realize how much chemistry you have forgotten and need to “brush-up” on.
 Don’t use “bungeed” log books or spiral bound log books.
 Don’t use “pull-out” paper log books.
Chemistry Log Books
First Semester Topics
Note: The topic titles below are what should be placed on the tabs to separate the sections in the log book from each
other.








Safety in Chemistry
Measurement
Matter
Atomic Structure: The Nucleus and Nuclear Chemistry
Atomic Structure: Organization of Electrons
Periodic Table
Chemical Bonding: Ionic and Covalent
Chemical Equations
Chemistry Log Books
Second Semester Topics
Note: The topic titles below are what should be placed on the tabs to separate the sections in the log book from each
other.






The Mole and Stoichiometry
Solutions
Acids and Bases
Energy (Thermochemistry/Organics)
Kinetics
Gas Laws
AKS Review
Safety in Chemistry
AKS Correlation
2 apply standard safety practices for all classroom laboratory investigation.
_____________________________________________________________________________
1. Identify and give the function of the teacher-selected scientific apparatus and safety equipment.
a. ________________________________________________________
b.________________________________________________________
c.________________________________________________________
d.________________________________________________________
e.________________________________________________________
2. List five (5) safety rules in your own words
1._______________________________________________________________
________________________________________________________________
2._______________________________________________________________
________________________________________________________________
3._______________________________________________________________
________________________________________________________________
4._______________________________________________________________
________________________________________________________________
5._______________________________________________________________
AKS Review
Measurement
AKS Correlation
5c. Explain the relationship between accuracy and precision
5e. Solve scientific problems by substituting quantitative values, using dimensional analysis and/or simple
algebraic functions as appropriate
8a1. Calculate density when given a means to determine mass and volume of a material
_____________________________________________________________________________
1.
Using dimensional analysis show how many seconds there are in 5 years.
2.
List the instrument and unit for measuring the following.
Quantity
Instrument
Unit (metric, SI)
Mass
Volume
Temperature
Length
3.
Explain how precision and accuracy are alike and how they differ.
4.
What is the formula for density?
5.
Determine the missing information in the chart below. Show work.
MASS
12 grams
b.
2 grams
WORK:
a. Density =
b. Mass =
c. Volume =
VOLUME
6 ml
5 ml
c.
DENSITY
a.
2.54 g/ml
12.0 g/ml
You are given a small rock and a shoe box. Explain how you would determine the density of each.
A small rock…….
Measuring instruments:
Procedure:
Sample calculations:
_______________________________________________________________________________________________
A shoe box…….
Measuring instruments:
Procedure:
Sample calculations:
AKS Review
Matter
AKS Correlation
8a. Identify substances based on chemical and physical properties/changes
_____________________________________________________________________________
1. How are the solid, liquid, and gas of a substance, such as water, alike?
2.
How are the solid, liquid, and gas of a substance, such as water, different?
3.
Define the following terms:
a. pure substance
b. heterogeneous
c. homogenous mixtures
d. solutions.
4.
Classify the following examples as pure substance or heterogeneous mixture, homogeneous mixture, and/or
solution.
a. pizza ____
b. salt water ____
c. clear red liquid ____
d. granite rock ____
e. copper wire ____
f. sodium chloride ____
g. sugar dissolved in water_____
5.
Define
a. physical property
b. chemical property
6.
Classify the following as examples of either physical properties or chemical properties.
a. A piece of metal has a mass of 60.0 g._____
b. Metals react with acids to produce hydrogen gas.____
c. Tommy’s weight on the moon 40 lbs.____
d. Susan’s weight on earth is 45.0 kg.____
e. The density of water is 1.00g per ml.____
f. Litmus turns red in the presence of an acid.___
g. The book burned for 20 seconds.____
h. A metal, such as copper, has a good electrical conductivity.___
i. Water boils at a temperature of 100 degrees Celsius.____
j. When sodium hydroxide dissolves in water, the solution becomes hot.____
k. Combustion____
l. Melting___
m. Fermentation___
n. Metabolism___
o. Boiling___
p. Electrolysis___
AKS Review
Atomic Structure
AKS Correlation
Use the modern atomic theory to explain the characteristics of atoms
10a. discriminate between the relative size, charge, and position of protons, neutrons, and electrons in an atom
10c. explain the relationship of the proton number to the element’s identity
10d. explain the relationship of isotopes to the relative abundance of atoms of a particular element
10d1. differentiate between alpha, beta, and gamma radiation
__________________________________________________________________
a.
b.
Trace the development of the modern atomic theory.
Atomic theories
Democritus
Dalton
Thomson
Rutherford
Bohr
Describe the basic structure of the atom as protons, neutrons and electrons in specific arrangements. Identify the
relative location, size and charge of subatomic particles.
proton
neutron
electron
Location
Mass
Charge
c.
How does the number of electrons in the outermost level determine the reactivity of an element?
d.
Give the electron orbital configuration for each element in periods 1,2,3,4.
e.
Draw electron Dot formulas for elements in periods 1-4.
f.
What is quantum number?
g.
Explain emission spectroscopy as it relates the energy loss by electrons when returning to ground state.
FILL OUT THE CHART BELOW.
Radiation type
Alpha
Symbol
Mass
Penetrating power
/Shielding
Beta
Gamma
h.
What will tend to happen to elements with 1 to 3 valence electrons?
i.
What will tend to happen to elements with 6-7 valence electrons?
j.
What will happen to elements with 8 valence electrons?
AKS Review
Periodic Table
AKS Correlation
11 use the organization of the periodic table of elements to predict the properties of elements
_______________________________________________________________________________
1. DEFINE CLEARLY:
Period
Actinides
Transition elements
Group(families)
Metal
Lanthanides
Periodic law
Noble gases
Metalloid
Semiconductor
Periodicity
Nonmetal
Synthetic
2. Give four examples of periodicity.
3. Where would you find a metal on the periodic table?
4 .Which elements are most likely to be used as semiconductors?
5. The father of the periodic table was_______.
6. List the columns of the periodic table 1A-8A, give the valence electrons for each and Lewis dot structure for
each?
7. List the three elements predicted by Mendeleev.
8. What are the characteristics of transition element?
9. Define:
a. Metallurgyb. Orec. Minerald. Alloye. Allotrope10. What state are most elements in at room temperature?____________
11. List several characteristics of
Metals-
Nonmetals-
Metalloids-
12. What are the group and period trends for ___?
atomic radii
group-period-ionization energy
group-period-electro negativity
group-period-AKS Review
Bonding
AKS Correlation
8b predict formulas for stable ionic compounds based on balance of charges
8c use IUPAC nomenclature from transition between the chemical names and
formulas of ionic compounds, covalent compounds
__________________________________________________________________
1. Describe the formation of ionic and covalent bonds.
2.
What type of elements will form ionic bonds?
3.
Which types of elements will form covalent bonds.
4.
When will a covalent bond be polar?
5.
How does polarity effect a molecules interaction with other molecules?
6.
Identify each of the following weak bonds.
Van de Waals
Hydrogen
Dipole-dipole
Ion-dipole
7. What type of bonding would most likely occur between:
a)metal-nonmetal _________________________
b)nonmetal-nonmetal _________________________
Fill in the chart below:
Name
Formula
Ionic
Silicon dioxide
Chlorine trifluoride
Carbon tetrachloride
Sulfur difluoride
N2F4
SO3
NO
SeO2
KClO2
Cu2O
Na3N
NiCl2
Iron (III) oxide
Calcium chloride
Sodium bromate
Ammonium bromide
Covalent
AKS Review
Chemical equations
AKS Correlation
9a identify and balance the following type of equations: synthesis (including condensation that synthesizes
carbohydrate, lipids, and proteins), decomposition, single replacement, double replacement, and combustion.
__________________________________________________________________
Write and balance the following chemical equations:
1. Aluminum reacting with oxygen to produce aluminum oxide.
Type of reaction___________________
2. Iron(II) chloride and sodium phosphate reacting to form sodium chloride and Iron(II) phosphate.
Type of reaction___________________
3. Methane( CH4 ) combining with oxygen gas producing carbon dioxide and water
Type of reaction___________________
4. Chlorine gas reacts with lithium bromide to produce lithium chloride and bromide gas
Type of reaction___________________
5. Calcium carbonate breaks down to Calcium oxide and Carbon dioxide
Type of reaction___________________
AKS Review
The Mole and Stoichiometry
AKS Correlation
9c. Apply concepts of the mole and Avogadro’s number to conceptualize and calculate:
-empirical/molecular formulas
-mass, moles, and molecules relationships
9d. Verify Conservation of Mass in a chemical reaction quantitatively by:
-identifying and solving different types of stoichiometry problems, specifically relating mass to moles and
mass to mass
-demonstrating the conceptual principle of limiting reactants
__________________________________________________________________
In all calculations that follow, SHOW ALL WORK AND USE SIGNIFICANT FIGURES.
1. Write Avogadro’s number conventionally and in scientific notation.
2. (a) What is molar mass?
(b) Find the molar mass of the following:
Fe
CCl4
Al2(CO3)3
3. Perform the following conversions.
(a) Determine the number of atoms in 3.75 mol Fe. (Tech can omit)
(b) How many moles of CaCl2 contain 1.26x1024 formula units of CaCl2? (Tech can omit)
(c) Determine the number of moles of arsenic in 1.90 g As.
(d) Calculate the mass in grams of 42.5 mol of potassium cyanide (KCN).
(e) Determine the mass in grams of 5.65 x 1024 atoms Se. (Tech can omit)
4. What is the percent composition by mass of each element in:
(a) water
(b) sucrose (C12H22O11)
5. (a) Define what an empirical formula is and give an example.
(b) Define what a molecular formula is and give an example.
6. A compound is 82.6 % C and 17.4 % H. Its molecular weight is 58.14 g/mol. (CP and Tech can omit)
(a) What is the empirical formula for this compound?
(b) What is the molecular formula for this compound?
(c) Draw 2 possible structural formulas for this compound.
7. (a) What is stoichiometry?
(b) How many moles of HCl will react with 0.200 mol Al(OH) 3? Use the following equation.(Tech can omit)
Al(OH)3 + 3 HCl  AlCl3 + 3 H2O
(c) What mass of chromium (III) oxide will be produced when 4.58 moles of chromium react?(Tech can
Use the following equation. 4 Cr + 3O 2  2 Cr2O3
omit)
(d) How many grams of carbon dioxide will be produced when 2.50g of NaHCO3 react with
excess acid according to the following equation: (Tech can omit)
3 NaHCO3 + H3C6H5O7  Na3C6H5O7 + 3 CO2 + 3 H2O
8. (a) Distinguish between limiting reactant and excess reactant.
(b) Find the limiting reactant when 4 mol LiOH react with 3 mol CO2 according to the following
equation: 2 LiOH + CO2  Li2CO3 + H2O. How many moles of water will be produced? (Tech can
omit)
(c) 45 g C6H6 react with 45 g Cl2 according to the equation: Cl2 + C6H6  C6H5Cl + HCl. What
is the limiting reactant? What mass of HCl will be produced?
(Tech can omit)
9. (a) Define actual yield, theoretical yield, and percent yield.
(b)
5.00 g of tin reacted with excess iodine according to the equation
Sn + 2I2  SnI4.
Calculate the percent yield of SnI4 if 25.0 g of SnI4 was recovered. (CP and Tech can omit)
AKS Review
Solutions
AKS Correlation
14a. Explain solubility in terms of substance involved (i.e. solute, solvent) and the process of dissolving a solute by:
 Observing factors that effect the rate at which a solute dissolves in a specific solvent
 Demonstrating that solubility is related to temperature by constructing a solubility curve
 Expressing concentrations in molarity
 Preparing and properly labeling solutions of specified molar concentrations
 Relate molality to colligative properties
__________________________________________________________________
1. (a) What is a solution?
(b) What are the two parts of a solution?
2. Identify the solute and solvent in an aqueous solution of sugarwater.
Solute: ____________
Solvent: ____________
3. If one liquid is soluble in another liquid, such as food coloring in water, the two liquids are considered
________________.
4. If one liquid is insoluble in another, such as oil in water, the two liquids are _____________.
5. Discuss the two processes that occur during solution formation.
6. (a) Explain the phrase “like dissolves like” using the terms polar and nonpolar.
(b) Identify whether the following substances would dissolve in WATER or GASOLINE (OCTANE).
NaCl
CH4
I2
7. Discuss three factors that affect the rate at which solvent particles dissolve solute particles.
8. What is solubility?
9. Distinguish between saturated solutions, supersaturated solutions, and unsaturated solutions.
10. (a) What happens to solid solutes as temperature increases?
(b) What happens to gaseous solutes as temperature increases?
11. What is the percent by mass of 81.0 g of NaCl dissolved in a solution of 525 g?
12. (a) 21.0 moles of sugar are in a solution of 52.0 L. What is the molarity of this sugar solution?
(b) Explain the steps you would follow in order to prepare the sugar solution with the molarity you calculated
above. Be specific with instructions and be sure to indicate the lab equipment needed.
(Tech can
omit)
13. (a) What is a colligative property?
(b) List the four types of colligative properties.
1.
2.
3.
4.
14. Use a colligative property to explain why salt is often thrown on icy steps and roads in the winter.
15. Use the graph below for the questions that follow.
Temperature in C
(a) How much ammonium chloride dissolves in 100. g of water at 50.C?
(b) At what temperature does 115 g of sodium nitrate dissolve in 100. g of water?
(c) Name all the gaseous solutes on the solubility graph above.
(d) If 40.0 g of NH4Cl is dissolved in 100. g of water at 90.C, how much more solute can be added before
the solution becomes saturated?
(e) At 80.C, 52 g of KCl is dissolved in 100. g of water. The temperature is then lowered to
How much KCl will precipitate out of solution?
(f) What is the mass of Yb2(SO4)3 that can dissolve in 350. g of water at 60.C?
10.C.
AKS Review
Acids and Bases
AKS Correlation
14. Analyze properties that describe solutions and the behavior of acids and bases.
14b. Compare, contrast and evaluate the nature and behavior of acids and bases in terms of Arrhenius, BronstedLowry acids/bases, strong vs. weak acids/bases in terms of percent dissociation and conductivity, hydronium
ion concentration, pH, and acid-base neutralization.
14c. Classify common substances as acid, base, or neutral based on chemical properties.
__________________________________________________________________
1. Examine the list of physical and chemical properties in the chart below. Decide if that property describes an
acid, base, both, or neither by placing a check in the column that the physical or chemical property matches. You
can have more than one check by a property or no checks by a property!
Property
Acid
Base
tastes sour
tastes bitter
pH > 7
PH < 7
good conductors of electricity
turns blue litmus red
turns red litmus blue
reactants in neutralization
turns pink in the presence of phenolphthalein
donates H+ ions
accepts H+ ions
contains OH- ions
contains H+ ions
reacts with metals and carbonates
dissolves in water to form
aqueous solutions
corrosive
alkaline
commonly used as cleaning agents
contains more OH- ions than H+ ions
contains more H+ ions than OH- ions
associated with hydronium (H3O+) ions
2. Fill in the chart below with the different views on acids and bases according to Arrhenius and Bronsted-Lowry.
Arrhenius
Bronsted-Lowry
Acids
Bases
3. (a) Distinguish between strong acids and weak acids in terms of percent dissociation.
(Tech can omit)
(b) Distinguish between strong bases and weak bases in terms of percent dissociation. (Tech can omit)
4. (a) What is the general chemical reaction for neutralization? Be sure to include the products made from a
neutralization reaction!
(b) What are always the two products of a neutralization reaction?
(c) What type of chemical reaction is a neutralization reaction (i.e. synthesis, decomposition, single
displacement, double displacement, or combustion)?
5. Draw a pH scale and label the location of acids, bases, and neutral substances.
6. Fill in the blanks in the following table and then answer the questions that follow.
More H+ or OH- ions or
Substance
[H+]
pH
Equal Amounts?
unknown A
1.0 x 10-6 M
unknown B
2.5 x 10-8 M
unknown C
1.0 x 10-10 M
unknown D
7.8 x 10-5 M
unknown E
1.0 x 10-7 M
Acid, Base, or Neutral?
(a) Show the formula for how you calculated the pH for the unknowns in the chart above.
(b) How much stronger is unknown A than unknown C? _____________ How do you know?
7. Examine the data in the following table to determine whether the substance is an acid, base, or neutral. If the
substance is already identified as an acid, base, or neutral substance, then fill in the data you would expect to
find if you tested it in lab.
turns red
Reaction with
Phenolphthalein
stays clear
Reaction with
Methyl Orange
turns red
stays blue
turns pink
turns yellow
Substance
Red Litmus
Blue Litmus
Unknown A
Unknown B
Unknown C
stays red
turns blue
Acid, Base,
or Neutral?
neutral
AKS Review
Energy (Thermochemistry and Organics)
AKS Correlation
13c. collect data in order to calculate the amount of heat given off or taken in by chemical or physical processes
(SC6b)
13d analyzing (both conceptually and quantitatively) flow of energy during change of state (phase) (SC6c)
__________________________________________________________________
1.
Energy is defined as the ability to do work or produce heat. How does energy affect the behavior of
molecules?
2.
(a) Where is energy stored in a molecule?
(b) What is chemical potential energy?
3.
List the two main forms of energy
a. _________________
b. __________________
4.
Are temperature and heat energy the same? Defend your answer.
5.
The amount of heat energy required to raise the temperature of 1 g of water 1 degree Celsius is _____.
6.
What is the difference between calories and Calories?
7.
How do you calculate the number of food calories in a food?
8.
One calorie is equal to ____ Calories = _____ kCal
9.
What is specific heat?
10. In the formula, q = mc∆T, what does each variable represent?
q = ______
m= ______
c = _______
∆T = ______
11. If the temperature of 34.4 g of ethanol increases from 25.0˚C to 78.8˚C, how much heat has been absorbed
by the ethanol?
12. Examine the Heating Curve Graph below and answer the following
questions.
Heating Curve Graph
for Benzene
D
100
b.
c.
d.
What do the plateaus on the heating curve
graph indicate?
Which letter on the heating curve graph
represents the liquid state of benzene?
Which letter on the graph represents
solidification?
Which letter represents the highest amount A
of kinetic energy in the molecules?
13. What is thermo chemistry?
80
Temperature (in degrees Celsius)
a.
90
C
70
60
50
B
40
30
20
10
0
14. How do you calculate change in enthalpy?
1
2
3
4
5
6
7
8
9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56
Time Heat Added (min)
AKS Review
Kinetics
AKS Correlation
12. Predict how various factors affect the rate of a chemical reaction
12a - demonstrate the effects of changing concentration, temperature and pressure on chemical reactions
(GPS)
12b - investigate the effects of a catalyst on chemical reactions and apply it to everyday
examples
(GPS)
13. Evaluate the motion and behavior of atoms and molecules in chemical and physical processes
13a - compare and contrast atomic/molecular motion of solids, liquids, gases and plasma (GPS)
13b - relate temperature, pressure and volume of gases to the behavior of gases
13c - collect data in order to calculate the amount of heat given off or taken in by chemical or
physical processes (GPS)
13d – analyze (both conceptually and quantitatively) the flow of energy during a change of state
(phase) (GPS)
__________________________________________________________________
1. (a) What are four factors that can affect the rate at which a reaction occurs?
(b) Explain how each factor can speed up a reaction.
2. (a) What is a catalyst?
(b) How does a catalyst do its job?
3. Explain what it means for a reaction to be at equilibrium. (Tech can omit)
4. Draw a rate of reaction graph and explain what happens to the rate of the forward reaction and the rate of the
reverse reaction over time. (CP and Tech can omit)
5. Explain Le Chatelier's Principle. (Tech can omit)
6. What is the KMT?
7. What are the main points of the KMT?
Use this equation for the stresses below:
2 H2(g) + O2(g)  2 H2O(l) + 69.2 kJ
8. Which way would the equilibrium shift if the reaction is heated? Why? (Tech can omit)
9. Which way would the equilibrium shift if pressure is increased? Why? (Tech can omit)
10. Which way would the equilibrium shift if more water is added to the mixture? Why? (Tech can omit)
10. Describe solids, liquids, and gases in terms of their molecular motion and energy.
11. Describe what happens to a substance during the melting phase and during the boiling phase.
12. Explain why there is no change in temperature when a substance changes phase.
13. Why is the Kelvin temperature scale used in science?
14. Label on the graph below the following items by writing the term in the appropriate spot on the graph:
a. melting (fusion)
c. vaporization
Heating Curve Graph
b. freezing (solidification)
d. condensation
Heating Curve Graph For Benzene
ees Celsius)
35
30
25
Heat Added Over Time (one second intervals)
15. Label on the graph by writing the term in the appropriate area of the graph where the solid, liquid, and gaseous
states of matter are.
AKS Review
Gas Laws
AKS Correlation
13b. Relate temperature, pressure and volume of gases to the behavior of gases
__________________________________________________________________
1. What are the four factors that affect the behavior of gases?
a.
b.
c.
d.
2. Define pressure AND give the units in which pressure is measured.
3. (a) State Boyle’s Law.
(b) What is the equation stated in Boyle’s Law?
(c) What type of relationship occurs in the law: direct or inversely proportional?
4. (a) State Charles’ Law.
(b) What is the equation stated in Charles’ Law?
(c) What type of relationship occurs in the law: direct or inversely proportional?
5. (a) State the Combined Gas Law.
(b) What is the equation stated in the Combined Gas Law?
(c) What type of relationship occurs in the law: direct or inversely proportional?
6. What is STP and the values it represents?
7. (a) What is Avogadro’s Principle regarding gases? (CP and Tech can omit)
(b) What is the volume of a gas at STP? (CP and Tech can omit)
8. Identify the following as being examples of either Boyle’s Law or Charles’ Law:
____(a) George left his basketball outside on a very cold night. The next morning
the basketball was very hard to bounce and appeared to be smaller than it
was the night before.
____(b) Felecia opens a can of soda and hears the sound of gas escaping.
____(c) Mario decides to shake his bottle of soda before opening it the first time.
He notices bubbles in the bottle.
____(d) Katherine squeezes a balloon.
9. A gas at 55C occupies a volume of 3.6 L. What volume will it occupy at 30.C? Assume pressure and mass
remain constant.
10. The pressure of air in a 2.25 L container is 1.20 atm. What is the new pressure if the sample is transferred to a
6.5 L container? Assume temperature and mass remain constant.
11. How many moles of air are in a 6.06 L tire at STP? (CP and Tech can omit)