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Notes: U4
Unit #4: Gases
Study Guide
Unit 4 Review Session: Monday, January 14 @ 4:00 PM
Unit 4 Exam: Tuesday, January 15
 SWBAT explain the movement and properties of gases through diffusion and
the kinetic molecular theory.
 SWBAT convert between Celsius and Kelvin
 SWBAT define pressure.
 SWBAT explain the relationship between temperature and pressure.
 SWBAT solve for an unknown variable given conditions involving changing
temperature and pressure (Gay Lussac’s).
 SWBAT explain the relationship between temperature and pressure.
 SWBAT solve for an unknown variable given conditions involving changing
temperature and volume (Charles’).
 SWBAT explain the relationship between volume and temperature.
 SWBAT solve for an unknown variable given conditions involving changing
pressure and volume (Boyle’s).
 SWBAT explain the relationship between volume and pressure.
 SWBAT use the ideal gas law to calculate for an unknown variable.
Why didn’t I get the correct answer?
1. Was your temperature converted to Kelvin?
2. Did you make sure your volume/pressure units were the same?
3. What was the unit supposed to be for the final answer? Did you convert it to be
that unit?
4. Did you use the correct numeric values in your calculation?
5. Did you use the correct equation?
6. Did you do your algebra properly?
GOOD LUCK!
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Notes: U4
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Use complete sentences for explanations and conceptual questions.
Show all work for quantitative and computational questions.
1. What does the Kinetic Molecular Theory state about the behavior of gases?
(3-4 key things)
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2. Gas molecules travel at a speed over 10 times faster than a car on a highway.
However, why would it take someone twenty feet away from a sample of
gasoline 10-20 seconds to smell it? (key word: diffusion)
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3. Please describe what “creates pressure” in the specific picture drawn below.
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Notes: U4
Mixed Gas Law Problems:
4. A sample gas occupies a volume of 8.50 L at 25.0ºC. What will the
temperature be, in degrees Celsius, if the volume of the gas is 4.00 L.
-132.8 OC
5. A rigid container of O2 has a pressure of 400 mmHg at a temperature of 440
OC. What is the pressure at 273 K?
153.2 mmHg
6. The air in a dry, sealed 2.0 L soda bottle is at STP. What will be its pressure if
it is brought to a higher altitude where the temperature is only 23ºC?
1.08 atm
7. An ideal gas at 300 K and 760 mmHg is contained in a flexible vessel. Its
temperature is halved. What will the volume become?
N/A
8. When a 375 mL sample of nitrogen is kept at constant temperature, it has a
pressure of 1.2 atmospheres. What pressure does it exert when compressed
to 125 mL?
3.6 atm
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Notes: U4
9. It is not safe to put aerosol canisters in a campfire, because the pressure
inside the canisters gets very high and they can explode. If I have a 1.0 liter
canister that holds 2 moles of gas, and the campfire temperature is 14000 C,
what is the pressure inside the canister?
274.7 atm
10. If I have 5.6 liters of gas in a piston at a pressure of 1.5 atm and compress the
gas until its volume is 4.8 L, what will the new pressure inside the piston be?
1.75 atm
11. A chemist produces 460 mL of oxygen gas at - 43 °C and constant pressure.
To what Kelvin temperature must the oxygen be warmed in order for it to
have a volume of 600 mL?
345 K
12. What pressure will a gas sample exert at 300 K if the same sample has a
pressure of 4 atmospheres at 120 K?
10 atm
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13. If I have a 600 milliliter container that holds 45 moles of gas at a temperature
of 2000 C, what is the pressure inside the container?
2,912 atm
14. If I have 43 liters of helium in a balloon at 250 C and increase the temperature
of the balloon to 580 C, what will the new volume of the balloon be?
51.7 L
15. If I have an unknown quantity of N2O gas at a pressure of 785 mmHg, a
volume of 32 liters, and a temperature of 87 0C, how many grams of gas do I
have?
49.2 grams
16. At what temperature will 16.00 g of CO, carbon monoxide gas, exert a pressure of
1.4 atm and a volume of 750. mL?
22.17 K
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Notes: U4
17. Create and explain a real life situation below that demonstrates the relationship
between volume and pressure.
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18. Create and explain a real life situation below that demonstrates the relationship
between temperature and volume.
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19. Create and explain a real life situation below that demonstrates the relationship
between temperature and pressure.
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Notes: U4
Extra-Credit Level Prep (Optional)
iv. Which of the following gases would occupy the largest volume at 25˚C and 1.00
atm pressure?
a. 100 g CH4
b. 100 g N2O
c. 100 g O2
d. 100 g CO2
e. All of the gases would have the same volume at STP.
ii. Acetylene gas, C2H2 is used for welding. A 5 liter supply of acetylene being stored
at -23 °C, exerts a pressure of 5 atm. At what temperature would the same number
of moles of acetylene, moved to a 10 liter container, produce a pressure of 2 atm?
200 K, or -73OC
iii. A 1.1 L container will hold about 1.6 g of which of the following gases at 0ºC and
1 atm?
a. SO2
b. O2
c. NH3
d. CH4
e. F2
b. O2
iv. A 600 mL sample of krypton is held at standard conditions. What volume does
the gas occupy when the pressure is tripled and the temperature doubles?
400 mL