Chapter 10 Homework
Part 1:
1. Explain each of the following properties of gases based on the KMT.
a. expansion
b. low density
c. fluidity
d. compressibility
e. diffusion
2. Describe the situations when gases act most ideal.
3. State the two reasons why real gases don’t act ideal.
4. Which TWO of the following gases would be most IDEAL (Hint: They should be
nonpolar molecules and relatively small)
A. Helium gas
B. Oxygen gas
C. Hydrogen gas
D. Water gas
E. Nitrogen gas
F. Ammonia gas (NH3)
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Part 2:
1. Name the four measurable quantities that describe gases.
2. Describe qualitatively the relationship between the following:
A. P vs V
B. T vs V
C. P vs T
D. P vs moles
3. Why does gas in a closed container exert pressure?
4. Explain the relationship between temperature and volume.
5. Explain the relationship between temperature and pressure.
6. Explain the relationship between moles and volume.
Unit Conversions:
1. 8.9 torr = ? mmHg
2. 696 mmHg = ? atm
3. 3.3 atm = ? kPa
4. 264 kPa = ? atm
5. 198.3 kPa = ? mmHg
6. 25oC = ? K
7. 295 K = ? oC
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Manometer Problems:
1. A gas sample in a closed manometer causes a Hg level difference of 190 mmHg.
What is the pressure of the gas?
2. A closed manometer has Ne gas in it. The Hg level difference 517.5 mm.
Atmospheric pressure is 750 mmHg. What is the pressure of the gas?
3. An open manometer contains oxygen gas. The mercury level is 75 mm higher in
the arm connected to the gas. Atmospheric pressure is 101.3 kPa. What is the
pressure of the gas in kPa?
4. An open manometer contains hydrogen gas. The mercury level is 30.0 mm higher
on the atmosphere side. The pressure of the atmosphere is 101.3 kPa. What is
the pressure of the gas in mmHg?
Gas Laws Problems:
1. If the pressure exerted on a 240 mL sample of hydrogen gas at constant
temperature is increased from 325 mmHg to 550 mmHg, what will the final
volume of the sample be?
2. A flask containing 155 mL of hydrogen was collected at a pressure of 22.5 kPa.
What pressure would have been required in order for the volume of the gas to
have been 90.0 mL at constant temperature?
3. A sample of air has a volume o 140.0 mL at 67oC. To what temperature must the
gas be lowered to reduce its volume to 50.0 mL at constant pressure?
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4. At standard temperature a gas has a volume of 275 mL. If the temperature is
increased to 130oC, but the pressure is held constant, what is its new volume?
5. A sample of hydrogen gas at 47oC exerts a pressure of 250 mmHg. If the gas is
heated to 77oC at constant volume, what will the new pressure be?
6. To what temperature must a sample of nitrogen at 27oC and 0.625 atm be heated
so that its pressure becomes 1.125 atm at constant volume?
7. A sample of gas at 47oC and 780 mmHg pressure occupies a volume of 2.20 L.
What volume would this gas occupy at 107oC and600.0 mmHg pressure?
8. A 350.0 mL air sample collected at 35oC has a pressure of 550 mmHg. What
pressure will the air exert if it is allowed to expand to 425 mL at 57oC?
9. A gas measures 1.75 L at –23oC and 150 kPa. At what temperature would the gas
occupy 1.30 L at 210 kPa?
10.A sample of oxygen at 40.0oC occupies 820.0 mL. If this sample occupies 1250
mL at 60.0oC and 1.40 atm, what was its original pressure?
11.A gas at 7.75 x 104 Pa and 17oC occupies a volume of 850 mL. At what
temperature, in degrees Celsius, would the gas occupy 720 mL at 8.10 x 104 Pa?
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Dalton’s Law of Partial Pressure Problems:
1. Three primary components of air are carbon dioxide, nitrogen, and oxygen. In a
sample containing a mixture of these gases at one atmosphere of pressure the
partial pressure of carbon dioxide is 0.285 mmHg, and the partial pressure of
nitrogen is 593.525 mmHg. What is the partial pressure of the oxygen in mmHg?
2. Determine the partial pressure of oxygen collected by water displacement if the
water temperature is 20.0oC (Pressure of water at 20.0oC 17.5 mmHg) and the
total pressure of the gases in the collection bottle is 730.0 mmHg.
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