Station 1 – LT 6.1 and 6.2
Lesson
6.2 – Pressure and Diffusion
What is pressure? Describe how pressure is created within a container.
Questions 1.
2. List 4 units that are used to measure pressure
3. What is diffusion? How does the motion of gas molecules explain
how a gas diffuses throughout a room?
4. Draw a picture of diffusion.
5. Gases move at hundreds of miles per hour. Why don’t you smell a gas
the second it is sprayed from a canister if you are on the other side of the
room?
6. Measurements inside a sealed container show that the pressure exerted
by a gas increases as the thermal energy of the gas increases. Which of
the following best explains this pressure increase?
A. The gas molecules stick to the walls of the container.
B. The gas molecules radiate energy in the form of nuclear
particles.
C. The gas molecules begin to bond together into heavier
molecules.
D. The gas molecules move faster and strike the container
walls more frequently.
7. When traveling from sea level to the top of a mountain, you would
expect air pressure to
a. Decrease
b. Increase
c. Double
d. Stay the same
8. When a sample of a gas is cooled, it condenses into a liquid. In which
of the following ways do the molecules of the original gas sample
compare with the molecules of the liquid?
A. The molecules are larger as a gas than they are as a
liquid.
B. The molecules weigh less as a gas than they do as a
liquid.
C. The molecules move faster as a gas than they do as a
liquid.
D. The molecules are closer together as a gas than they are
as a liquid.
9. Oxygen (O2) and nitrogen (N2) molecules are contained in a flask,
which is separated from a second flask by a closed valve, as shown
below. The second flask, of equal volume, is a vacuum.
The valve separating the two flasks is opened. Which of the following
diagrams represents the most likely arrangement of molecules after the
valve is opened?
A.
B.
C.
D.
Station 2 – LT 6.4, 6.5, and 6.6
Lesson
6.3 – Temperature Scales
the following Kelvin readings to Celsius:
Questions 1. Convert
a. 452 K = __________ oC
b. 321 K = __________ oC
c. 2 K = ____________ oC
2. Convert the following Celsius readings to Kelvin
a. 15 oC = ___________ K
b. -200 oC = _________ K
c. 1400 oC = _________ K
3. Is it possible to go below 0 K? Why or why not?
4.
5. Describe what the motion of molecules looks like in the gas
phase. Describe the motion of molecules looks like in the solid
phase. Describe what the motion of molecules looks like at absolute
zero.
Station 3 – LT 6.3
Lesson
6.3 – Temperature Scales
What is STP? What are the temperature and pressures under these
Questions 1.
conditions?
2.
Station 4 – LT 6.7, 6.8, 6.9
Lesson
6.4 – Charles, Boyle and Gay –
Lussac: The Gas Laws
Think back to the balloon that had liquid nitrogen poured on it.
Questions 1.
Why did the volume of the balloon decrease when liquid nitrogen
was poured on it and inflate when the dry ice was removed?
2. Draw a graph that describes the relationship between volume and
temperature. Is this a direct or indirect relationship? Do you have
volume at absolute zero?
3. A gas occupies 1.00 L at standard temperature. What is the
volume at 333.0 °C?
4. Carbon dioxide is usually formed when gasoline is burned. If 30.0
L of CO2 is produced at a temperature of 1000 °C and allowed to
reach room temperature (25.0 °C) without any pressure changes,
what is the new volume of the carbon dioxide?
5. Draw a graph that explains Boyle’s Law. Don’t forget to label
your axis!
6. The volume of the lungs is measured by the volume of air inhaled
or exhaled. If the volume of the lungs is 2.400 L during exhalation
and the pressure is 101.70 KPa, and the pressure during inhalation is
101.01 KPa, what is the volume of the lungs during inhalation?
7. Challenge - The total volume of a soda can is 415 mL. Of this
415 mL, there is 60.0 mL of headspace for the CO2 gas put in to
carbonate the beverage. If a volume of 100.0 mL of gas at standard
pressure is added to the can, what is the pressure in the can when it
has been sealed?
8. Think back to when I crushed the can without touching it. Why
did the can crush? Explain it using the terms pressure and
temperature. Draw a picture to help your explanation!
9. Draw a graph that describes Gay-Lussac’s Law. Is this a direct or
indirect relationship?
10. A sample of gas at 3000 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?
Station 5 – LT 6.7, 6.8, 6.9
Lesson
6.4 – Charles, Boyle and Gay –
Lussac: The Gas Laws
Question
s
Use
to answer the following questions:
1. The illustrations below represent the expansion of a gas in a
cylinder of an engine. The piston moves as the gas volume changes.
What could have been done to the gas in the cylinder to bring about
this change in volume?
A. Half of the molecules were released.
B. The Kelvin Temperature was doubled
C. The condensation rate for the gas was
doubled.
D. The amount of heat in the gas was reduced
by one half
2. The diagram below shows gas inside a sealed
container before and after force is applied to the
container’s movable piston. The temperature
inside the container remains the same after the
force is applied.
Applying force to the piston results in
compression of the gas particles and an increase
in gas pressure. Which of the following
statements best describes the change in gas
particles after compression?
A. The kinetic energy of the gas particles
increases.
B. The kinetic energy of the gas particles
decreases.
C. The velocity with which the gas particles
hit the container wall increases.
D. The frequency with which the gas
particles hit the container wall increases.
3. A sample of nitrogen (N2) gas in a 10.0 L
container has a pressure of 1.0 atm at 297 K.
Assuming ideal gas behavior, what will the
pressure be if the same amount of nitrogen gas is
put into a 5.0 L container at 297 K?
A. 0.40 atm
B. 0.50 atm
C. 2.0 atm
D. 2.5 atm
4. Which of the following statements explains
what happens to the gas inside a balloon as the
external pressure on the balloon decreases and
the temperature stays constant?
A. The volume increases.
B. The volume decreases.
C. The molecular speed increases.
D. The molecular speed decreases.
5. Assuming pressure is held constant, which of
the following graphs shows how the volume of
an ideal gas changes with temperature?
A.
B.
C.
D.
6. Which of the following is not true of a sample
of gas as it is heated in a rigid, closed container?
A. The pressure of the molecules increases.
B. The average speed of the molecules
increases.
C. The average distance between molecules
increases.
D. The number of collisions between
molecules increases.
7. The four tanks shown in the diagram below
contain compressed nitrogen gas. The
temperature of the gas is the same in each tank.
8. Which of the tanks contains the greatest
number of gas particles?
A. tank 1
B. tank 2
C. tank 3
D. tank 4
9.When a scuba diver is deep underwater and
exhales, air bubbles form and rise to the surface
of the water. Which of the following
statements best describes what happens to the air
bubbles as they rise to the surface?
A. The number of molecules in the bubbles
increases, and the diameter of the
bubbles increases.
B. The number of molecules in the bubbles
decreases, and the diameter of the
bubbles decreases.
C. The number of molecules in the bubbles
remains the same, and the diameter of
the bubbles increases.
D. The number of molecules in the bubbles
remains the same, and the diameter of
the bubbles decreases.
Station 6 – LT 6.10
Lesson
6.5 – Ideal and Combined Gas Law
If I initially have a gas with a pressure of 84 kPa and a
Questions 1.
temperature of 350 C and I heat it an additional 230 degrees, what
will the new pressure be? Assume the volume of the container is
constant.
2. My car has an internal volume of 2600 liters. If the sun heats my
car from a temperature of 200 C to a temperature of 550 C, what will
the pressure inside my car be? Assume the pressure was initially 1
atm.
3. How many moles of gas are in my car in problem #3? Use the
initial conditions, not the final conditions in your calculations.
4. A toy balloon filled with air has an internal pressure of 1.25 atm
and a volume of 2.50 L. If I take the balloon to the bottom of the
ocean where the pressure is 95 atmospheres, what will the new
volume of the balloon be? How many moles of gas does the balloon
hold? (Assume T = 285 K and use only final conditions)
Station 7 – LT 6.7, 6.8, 6.9, and 6.10
6.3 – Temperature Scales
Lesson
6.4 – Charles’s Law and Gay – Lussac’s Law
6.5 – Ideal Gas Law and Combined Gas Law
Questions
1. 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?
2. 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 30,400 mm Hg, what will be the volume
of the gas when it is released from the tanks?
3. At 27.00 °C a gas has a volume of 6.00 L. What will the volume
be at 150.0 °C?
4. A gas has a pressure of 0.370 atm at 50.0 °C. What is the pressure
at standard temperature?
Station 8 – LT 6.7, 6.8, 6.9, and 6.10
Lesson
6.3 – Temperature Scales
6.4 – Charles’s Law and Gay – Lussac’s Law
6.5 – Ideal Gas Law and Combined Gas Law
Questions
1. 2.00 liters of hydrogen, originally at 25.0 °C and 0.98 atm, are
heated until a volume of 20.0 liters and a pressure of 3.50
atmospheres is reached. What is the new temperature?
2. Determine the number of moles of Krypton contained in a 3.25
liter gas tank at 5.80 atm and 25.5 °C.
3. The temperature of a sample of gas in a steel container at 30.0 kPa
is increased from -100.0 °C to 10,000 °C. What is the final pressure
inside the tank? Assume that volume is constant
4. 1 g of H2 is contained in a 2.00 L container at 20.0 °C. What is the
pressure in this container in atm?
HINT – You need to convert grams to moles!
R=0.0821.
Station 9 – LT 6.7, 6.8, 6.9, and 6.10
6.3 – Temperature Scales
Lesson
6.4 – Charles’s Law and Gay – Lussac’s Law
6.5 – Ideal Gas Law and Combined Gas Law
Questions
1. Determine the volume of occupied by 2.34 grams of carbon
dioxide gas at STP. HINT – You need to convert grams of CO2 to
moles of CO2 using your stoichiometry road map .
2. A 5.0-L flask contains 0.60 g O2 at a temperature of 22oC. What
is the pressure (in atm) inside the flask?
3. An ideal gas is contained in a cylinder with a volume of 5.0 x 102
mL at a temperature of 30.oC and a pressure of 710. torr. The gas is
then compressed to a volume of 25 mL, and the temperature is raised
to 820.oC. What is the new pressure of the gas?
4. Consider the reaction between 42.5 g of liquid methyl alcohol,
CH3OH and 32 g of O2 at 27oC and a pressure of 2.00 atm. The
products of the reaction are CO2 (g) and H2O (g). Calculate the
number of moles of H2O formed if the reaction goes to completion.
The equation for the reaction is:
CH3OH (aq)+ O2 (g) CO2 (g)+ H2O (g)
Station 10 – LT 6.1 - 6.10
Lesson
6.2
6.3
6.4
6.5
–
–
–
–
Pressure and Diffusion
Temperature Scales
Charles’s Law and Gay – Lussac’s Law
Ideal Gas Law and Combined Gas Law
Questions
1. Determine the volume of occupied by 2.34 grams of carbon
dioxide gas at STP. HINT – You need to convert grams of CO2 to
moles of CO2 using your stoichiometry road map .
2. A 5.0-L flask contains 0.60 g O2 at a temperature of 22oC. What
is the pressure (in atm) inside the flask?
3. An ideal gas is contained in a cylinder with a volume of 5.0 x 102
mL at a temperature of 30.oC and a pressure of 710. torr. The gas is
then compressed to a volume of 25 mL, and the temperature is raised
to 820.oC. What is the new pressure of the gas?
4. Consider the reaction between 42.5 g of liquid methyl alcohol,
CH3OH and 32 g of O2 at 27oC and a pressure of 2.00 atm. The
products of the reaction are CO2 (g) and H2O (g). Calculate the
number of moles of H2O formed if the reaction goes to completion.
The equation for the reaction is:
CH3OH (aq)+ O2 (g) CO2 (g)+ H2O (g)