Name:
Date:
Period:
This week, we will be studying how the atmosphere and global warming work in more detail by exploring properties of gases. For math, we will work on
converting between units and analyzing direct and inverse relationships between variables.
CLASS
MONDAY (11/14)
Activities
Quiz
Gas behavior (movement
and energy of particles,
diffusion, mass and
volume)
TUESDAY (11/15)
Warmup: Practice with
converting units
Gas & Pressure
Pressure Stations
WEDNESDAY (11/16)
Warmup: Practice with
converting units
Relationship between
pressure and volume for
gases (Boyle’s Law)
THURSDAY (11/17)
Warmup: Practice with
pressure and volume
Relationship between
volume and temperature for
gases (Charles’s Law)
FRIDAY (11/18)
Quiz
Relationship between
pressure and
temperature for gases
(Gay-Lussac’s Law)
Combined Gas Law
p. 7-8
Homework
p. 2-4
p. 14
p. 21-22
p. 17-18
p. 25-27
ALEKS
Enjoy your
Thanksgiving Break! 
http://phet.colorado.edu/en/simulation/gas-properties
http://virtual.yosemite.cc.ca.us/lmaki/Chem142/practice.htm
http://www.youtube.com/watch?v=AEFBtKoiQhA
1
Homework- Temperature and Volume Conversions
Temperature Conversions
***NOTE: To convert between Fahrenheit and Celcius—use the formulas above
***Converting between Kelvin and Fahrenheit is a 2-step process. You have to convert from Kelvin to Celcius first.
2
Other Conversions Using Dimensional Analysis
Reminders for Dimensional Analysis
1.) Go through and underline all the important information.
2.) Figure out what your “starting point” is and write it as a fraction. (If there is no “denominator,” the invisible number
is “1”).
3.) Write out the needed conversion factors both ways (flipped).
4.) Line up your units to cancel them out until you reach the “ending point” or the answer.
5.) Multiply across the top. Multiply across the bottom. Divide the top and bottom.
6.) Circle or box your answer.
See example below:
If you are going 50 miles per hour, how many feet per second are you traveling?
3
Problems:
Use Dimensional Analysis to solve the following problems.
a. How many seconds old are you? (Express to the hundredths place using scientific notation.)
b. It is 30 miles from my home to school. Convert this distance from miles to inches. (Express to the hundredths place
using scientific notation.) 1 mile = 5280 feet and 1 foot = 12 inches.
c. How many kilometers is it from your house to school? (Express to the hundredths place using scientific notation.)
d.
e.
A person’s weight is 154 pounds. Convert this to kilograms. (1 lbs. = 454 grams)
An aspirin tablet contains 325 mg of acetaminophen. How many grains is this equivalent to? (1 gram = 15.432
grains)
4
Warmup – Practice with Converting Units
Temperature Conversions
Other Conversions
Table of Weights and Measures
Volume
Length
Area
1 nautical mile = 6076.11549
feet
1 inch = 2.54 cm
1 league = 5 280 yards
1 cable = 120 fathoms
1 fathom = 6 feet
1 degree = 69.047 miles
1 mile = 5280 feet
1 hand = 4 inches
1 township = 36 square miles
*Derive your area conversion
factors by working with length
and squaring all dimensions. Ex.
122 inch2 = 12 foot2
or
144 square inch = 1 square foot
5
4 gills = 1 pint
2 pints = 1 quart
1 liter = 1.0567 quarts
1 bushel = 4 pecks = 32 quarts
1 gallon = 4 quarts
Solve using the conversion factors that are listed in the table on the previous page.
a. Your cruise ship is leaving for a 610-league adventure. How many nautical miles is this?
b. Later the ship is discovered at 38 fathoms deep under water. Convert this to meters.
c. Fortunately you survived! You are stranded on a deserted island that is located 12.5 degrees north of the
equator. How many kilometers is this?
d. If you are rationed to 32 gills of fresh water a day. How many liters is this?
e. The island has an area of 3.5 townships. How many square yards is this? (Please use scientific notation.)
f. To reach the top of a palm tree for a coconut you will have to climb 7.4 meters. How many hands is this?
g. The island is rich with hot chile peppers. You can collect 1.6 pecks a day. How many liters could you collect
in 1 week?
6
Homework– Converting Units
Do the following problems. The conversion units should be provided to you.
Reminders for Dimensional Analysis
1.) Go through and underline all the important information.
2.) Figure out what your “starting point” is and write it as a fraction. (If there is no “denominator,” the invisible number
is “1”).
3.) Write out the needed conversion factors both ways (flipped).
4.) Line up your units to cancel them out until you reach the “ending point” or the answer.
5.) Multiply across the top. Multiply across the bottom. Divide the top and bottom.
6.) Circle or box your answer.
a. Each liter of air has a mass of 1.80 grams. How many liters of air are contained in 2.5 x10 3 kg of air?
(You should know how many grams are in a kilogram. If you forgot, look it up online!)
b. 16.0 grams of food contain 130 calories. How many grams of food would you need in order to consume
2150 calories?
c. The cost of 1.00 Liters of gas is 26.9 cents. How many dollars will 12.0 gallons cost?
7
d. Light travels 186, 000 miles / second. How long is a light year in meters? (1 light year is the distance
light travels in one year)
e. 1 mole of Si atoms contains 6.02 x1023 atoms. 6.02 x1023 atoms of Si have a mass of 28.1 g. How many
atoms of Si are contained in a computer chip that masses 38.02-mg?
8
Warmup – Converting Between Units of Volume
The other day, I visited a Pepsi plant. They had a big vat full of syrup for making Pepsi. The head technician said it took
2.0 mL of syrup to make one 12 ounce Pepsi, and that there was enough syrup in the vat to make 500 cases (24 cans
each) of Pepsi.
Let’s write out conversion factors we see together:
Other conversion factors you might want to use: 1 gallon = 3.786 liters = 128 ounces
a.) How many cans make up enough syrup to fill a vat?
a) How many ounces (oz) of syrup does the vat hold?
b) What was the volume of the vat in liters?
c) What was the volume of the vat in gallons?
d) What was the volume of the vat in cubic centimeters (cm3)?
9
NOTES: Pressure of Gases
For each of these stations, draw diagrams/arrows to indicate where you think pressure from air molecules is occurring.
Also answer any questions associate with the activity.
Activity #1
1.) Lower an empty drinking glass, with its open end facing downward, into a larger container of water.
Record some observations you are seeing. What’s happening to the cup?
Draw arrows to represent the direction of the pressure of the air molecules.
2.) With the open end still under water, slowly tilt the drinking glass.
Record some observations you are seeing. What’s happening to the air in the cup?
Draw arrows to represent the direction of the pressure of the air molecules.
Reflection: Were your observations different between testing the straight cup and the tilted cup? Why or why not? Use
gas molecules/pressure in your answer.
10
Activity #2
1.) Fill a test tube to the rim with water
2.) Cover the test tube opening with a piece of stiff plastic (saran wrap).
3.) Press down the plastic to make a tight seal with the mouth of the test tube.
4.) While continuing to press the plastic to the test tube, invert the test tube above a sink or a pan.
5.) Without causing any jarring, gently remove your hand from the piece of plastic.
Record your observations. What do you see happening?
Draw arrows to represent the direction of the pressure of the air molecules.
6.) Repeat the process with a test tube half-full of water.
Record your observations. What do you see happening?
Draw arrows to represent the direction of the pressure of the air molecules.
Reflection: Were your observations between a full test tube and a half-filled test tube the same or different? Why or
why not?
11
Activity #3
1.) Fill a test tube to the rim with water.
2.) Cover the test tube mouth with a piece of plastic wrap (saran wrap).
3.) While continuing to press the plastic wrap to the mouth of the test tube, invert the test tube and partially immerse it
in a container of water.
4.) Remove the piece of plastic wrap.
5.) Move the test tube up and down, keep its lower (open) end under water.
Record your observations. What do you see happening?
Draw arrows to represent the direction of the pressure of the air molecules.
6.) Repeat the process with the test tube half-full of water.
Record your observations. What do you see happening?
Draw arrows to represent the direction of the pressure of the air molecules.
Reflection: Were your observations between a full test tube and a half-filled test tube the same or different? Why or
why not?
12
Activity #4
1.) Take the plastic bottle. Make sure it has a small hole in its side.
2.) Cover the hole in the side of the bottle with your finger.
3.) Fill the bottle with water.
4.) Replace the cap tightly.
5.) Holding the bottle over a sink, remove your finger from the hole.
Record your observations. What do you see happening?
Draw arrows to represent the direction of the pressure of the air molecules.
6.) Still holding the bottle over the sink, remove the cap.
Record your observations. What do you see happening?
Draw arrows to represent the direction of the pressure of the air molecules.
Reflection: Were your observations of the cap and uncapped bottle different? Why or why not?
13
Homework – Converting Units of Pressure
Abbreviations:
atm - atmosphere
mm Hg - millimeters of mercury
torr - another name for mm Hg
Pa - Pascal (kPa = kilo Pascal)
Bar (equal to 100 kPa)
Conversions:
1 atm = 760 mm Hg = 101325 Pa = 14.7 lb/in2 = 1.013 bar
1. The air pressure for a certain tire is 109 kPa. What is this pressure in atmospheres?
2. The air pressure inside a submarine is 0.62 atm. What would be the height of a column of mercury balanced by this
pressure?
3. The weather news gives the atmospheric pressure as 1.07 atm. What is this atmospheric pressure in mm Hg?
4. An experiment at Sandia National Labs in New Mexico is performed at 758.7 mm Hg. What is this pressure in atm?
5. A bag of potato chips is sealed in a factory near sea level. The atmospheric pressure at the factory is 761.3 mm Hg.
The pressure inside the bag is the same. What is the pressure inside the bag of potato chips in Pa?
6. The same bag of potato chips from problem 5 is shipped to Denver, Colorado, where the atmospheric pressure is
99.82 kPa. What is the difference (in Pa) between the pressure in the bag and the atmospheric pressure?
14
Warmup- Converting Units of Pressure & Volume
Abbreviations:
atm - atmosphere
mm Hg - millimeters of mercury
torr - another name for mm Hg
Pa - Pascal (kPa = kilo Pascal)
Bar (equal to 100 kPa)
Conversions:
1 atm = 760 mm Hg = 101325 Pa = 14.7 lb/in2 = 1.013 bar
1.) The pressure gauge on a compressed air tank reads 43.2 lb/in2. What is the pressure in atm?
2.) The pressure in the tire of an automobile is 34.8 lb/in2. What is the pressure in kPa?
3.) Convert the following pressure units using unit analysis when necessary. Show your work below.
a.) 2 atm = __________ bar
d.) 4.9 bar = __________ psi
b.) 2 bar = __________ atm
e.) 113 kPa = __________ bar
c.) 669 mm Hg = __________ bar
f.) 35 bar = ________ Pa
15
Practice with Volume-Pressure Relationship (Boyle’s Law)
16
Homework – Boyle’s Law
Use Boyles’ Law to answer the following questions:
1)
gas?
1.00 L of a gas at standard temperature and pressure is compressed to 473 mL. What is the new pressure of the
2)
In a thermonuclear device, the pressure of 0.050 liters of gas within the bomb casing reaches 4.0 x 106 atm.
When the bomb casing is destroyed by the explosion, the gas is released into the atmosphere where it reaches a
pressure of 1.00 atm. What is the volume of the gas after the explosion?
3)
Synthetic diamonds can be manufactured at pressures of 6.00 x 104 atm. If we took 2.00 liters of gas at 1.00 atm
and compressed it to a pressure of 6.00 x 104 atm, what would the volume of that gas be?
4)
The highest pressure ever produced in a laboratory setting was about 2.0 x 106 atm. If we have a 1.0 x 10-5 liter
sample of a gas at that pressure, then release the pressure until it is equal to 0.275 atm, what would the new volume of
that gas be?
17
5)
Atmospheric pressure on the peak of Mt. Everest can be as low as 150 mm Hg, which is why climbers need to
bring oxygen tanks for the last part of the climb. If the climbers carry 10.0 liter tanks with an internal gas pressure of
3.04 x 104 mm Hg, what will be the volume of the gas when it is released from the tanks?
6)
Part of the reason that conventional explosives cause so much damage is that their detonation produces a
strong shock wave that can knock things down. While using explosives to knock down a building, the shock wave can be
so strong that 12 liters of gas will reach a pressure of 3.8 x 104 mm Hg. When the shock wave passes and the gas returns
to a pressure of 760 mm Hg, what will the volume of that gas be?
7)
Submarines need to be extremely strong to withstand the extremely high pressure of water pushing down on
them. An experimental research submarine with a volume of 15,000 liters has an internal pressure of 1.2 atm. If the
pressure of the ocean breaks the submarine forming a bubble with a pressure of 250 atm pushing on it, how big will that
bubble be?
8)
Divers get “the bends” if they come up too fast because gas in their blood expands, forming bubbles in their
blood. If a diver has 0.05 L of gas in his blood under a pressure of 250 atm, then rises instantaneously to a depth where
his blood has a pressure of 50.0 atm, what will the volume of gas in his blood be? Do you think this will harm the diver?
18
Warmup – Boyle’s Law & Graphing
Here is a graph of pressure (kPa) and volume (L) of a gas.
1.) Based on the graph, when the volume is 2.0 L, what is the pressure?
2.) Based on the graph, what would the pressure by if the volume were increased to 3.0 L?
3.) Use Boyle’s Law (the equation!) to confirm this answer from the graph. So take the pressure and volume from #1
and the volume from #2 and solve for the pressure if the volume is increased to 3.0 L. Did you get the same answer as
the answer in #2? Why or why not?
4.) Use Boyle’s Law to find what the volume would be if the pressure was 125 kPa. (Pick another point on the graph as
your P1 and V1). Does your answer make sense and fit on the graph?
5.) Based on the shape of the graph, describe the general pressure- volume relationship. I.e. – as volume increase (as the
x-axis goes the right), what happens to the pressure (the y-axis values?)
19
Practice with Temperature and Volume (Charles’s Law)
20
Homework – Charles’s Law
Charles’ Law Worksheet
1)
The temperature inside my refrigerator is about 40 Celsius. If I place a balloon in my fridge that initially has a
temperature of 220 C and a volume of 0.5 liters, what will be the volume of the balloon when it is fully cooled by my
refrigerator?
2)
A man heats a balloon in the oven. If the balloon initially has a volume of 0.4 liters and a temperature of 20 0C,
what will the volume of the balloon be after he heats it to a temperature of 250 0C?
3)
On hot days, you may have noticed that potato chip bags seem to “inflate”, even though they have not been
opened. If I have a 250 mL bag at a temperature of 19 0C, and I leave it in my car which has a temperature of 600 C, what
will the new volume of the bag be?
4)
A soda bottle is flexible enough that the volume of the bottle can change even without opening it. If you have
an empty soda bottle (volume of 2 L) at room temperature (25 0C), what will the new volume be if you put it in your
freezer (-4 0C)?
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5)
Some students believe that teachers are full of hot air. If I inhale 2.2 liters of gas at a temperature of 180 C and it
heats to a temperature of 380 C in my lungs, what is the new volume of the gas?
6)
How hot will a 2.3 L balloon have to get to expand to a volume of 400 L? Assume that the initial temperature of
the balloon is 25 0C.
7)
I have made a thermometer which measures temperature by the compressing and expanding of gas in a piston.
I have measured that at 1000 C the volume of the piston is 20 L. What is the temperature outside if the piston has a
volume of 15 L? What would be appropriate clothing for the weather?
22
Warmup – Charles’s Law & Graphing
1.) Based on the graph, what is the unit of temperature?
2.) Based on the graph, when the volume is 2.0 L, what is the temperature?
3.) Based on the graph, what would the temperature by if the volume were increased to 3.0 L?
4.) Use Charles’s Law (the equation!) to confirm this answer from the graph. So take the pressure and volume from #1
and the volume from #2 and solve for the temperature if the volume is increased to 3.0 L. Did you get the same answer
as your answer in #3? Why or why not?
5.) Use Charles’s Law to find what the volume would be if the temperature was 500 K. (Pick another point on the graph
as your T1 and V1). Does your answer make sense and fit on the graph?
6.) Based on the shape of the graph, describe the general volume-temperature relationship. I.e. – as temperature
increase (as the x-axis goes the right), what happens to the temperature (the y-axis values?)
7.) Predicting: If the temperature of the gas were 0 K, what would the volume of the gas be? (Use Charles’s Law!)
23
Practice with Pressure and Temperature (Gay-Lussac’s Law)
Abbreviations
atm - atmosphere
mm Hg - millimeters of mercury
torr - another name for mm Hg
Pa - Pascal (kPa = kilo Pascal)
K - Kelvin
°C - degrees Celsius
Conversions
K = °C + 273
1 cm3 (cubic centimeter) = 1 mL (milliliter)
1 dm3 (cubic decimeter) = 1 L (liter) = 1000 mL
Standard Conditions
0.00 °C = 273 K
1.00 atm = 760.0 mm Hg = 101.325 kPa = 101,325 Pa
1.) Determine the pressure change when a constant volume of gas at 1.00 atm is heated from 20.0 °C to 30.0 °C.
2.) A gas has a pressure of 0.370 atm at 50.0 °C. What is the pressure at standard temperature?
3.) A gas has a pressure of 699.0 mm Hg at 40.0 °C. What is the temperature at standard pressure?
24
Homework – Gay Lussac’s Law
Abbreviations
atm - atmosphere
mm Hg - millimeters of mercury
torr - another name for mm Hg
Pa - Pascal (kPa = kilo Pascal)
K - Kelvin
°C - degrees Celsius
Conversions
K = °C + 273
1 cm3 (cubic centimeter) = 1 mL (milliliter)
1 dm3 (cubic decimeter) = 1 L (liter) = 1000 mL
Standard Conditions
0.00 °C = 273 K
1.00 atm = 760.0 mm Hg = 101.325 kPa = 101,325 Pa
1.) If a gas is cooled from 323.0 K to 273.15 K and the volume is kept constant what final pressure would result if the
original pressure was 750.0 mm Hg?
2.) If a gas in a closed container is pressurized from 15.0 atmospheres to 16.0 atmospheres and its original temperature
was 25.0 °C, what would the final temperature of the gas be?
3.) A 30.0 L sample of nitrogen inside a rigid, metal container at 20.0 °C is placed inside an oven whose temperature is
50.0 °C. The pressure inside the container at 20.0 °C was at 3.00 atm. What is the pressure of the nitrogen after its
temperature is increased?
4.) A sample of gas at 3.00 x 103 mm Hg inside a steel tank is cooled from 500.0 °C to 0.00 °C. What is the final pressure
of the gas in the steel tank?
5.) The temperature of a sample of gas in a steel container at 30.0 kPa is increased from -100.0 °C to 1.00 x 103 °C. What
is the final pressure inside the tank?
6.) Calculate the final pressure inside a scuba tank after it cools from 1.00 x 103 °C to 25.0 °C. The initial pressure in the
tank is 130.0 atm.
25
Homework – Combined Gas Law
Use the combined gas law to solve the following problems:
1)
If I initially have a gas at a pressure of 12 atm, a volume of 23 liters, and a temperature of 200 K, and then I raise
the pressure to 14 atm and increase the temperature to 300 K, what is the new volume of the gas?
2)
A gas takes up a volume of 17 liters, has a pressure of 2.3 atm, and a temperature of 299 K. If I raise the
temperature to 350 K and lower the pressure to 1.5 atm, what is the new volume of the gas?
3)
A gas that has a volume of 28 liters, a temperature of 45 0C, and an unknown pressure has its volume increased
to 34 liters and its temperature decreased to 35 0C. If I measure the pressure after the change to be 2.0 atm, what was
the original pressure of the gas?
4)
A gas has a temperature of 14 0C, and a volume of 4.5 liters. If the temperature is raised to 29 0C and the
pressure is not changed, what is the new volume of the gas?
26
5)
If I have 17 liters of gas at a temperature of 67 0C and a pressure of 88.89 atm, what will be the pressure of the
gas if I raise the temperature to 94 0C and decrease the volume to 12 liters?
6)
I have an unknown volume of gas at a pressure of 0.5 atm and a temperature of 325 K. If I raise the pressure to
1.2 atm, decrease the temperature to 320 K, and measure the final volume to be 48 liters, what was the initial volume of
the gas?
7)
If I have 21 liters of gas held at a pressure of 78 atm and a temperature of 900 K, what will be the volume of the
gas if I decrease the pressure to 45 atm and decrease the temperature to 750 K?
8)
If I have 2.9 L of gas at a pressure of 5 atm and a temperature of 50 0C, what will be the temperature of the gas if
I decrease the volume of the gas to 2.4 L and decrease the pressure to 3 atm?
9)
I have an unknown volume of gas held at a temperature of 115 K in a container with a pressure of 60 atm. If by
increasing the temperature to 225 K and decreasing the pressure to 30 atm causes the volume of the gas to be 29 liters,
how many liters of gas did I start with?
27