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Name _______________________
Period _______
CRHS Academic Chemistry
Unit 11 - Gas Laws
Homework
Due Date
Assignment
On-Time (100)
Late (70)
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11.1
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11.2
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11.3
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11.4
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Warm-Up
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EC
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Notes, Homework, Exam Reviews and Their KEYS located on CRHS Academic Chemistry
Website: https://cincochem.pbworks.com
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WARM-UPS
Day 1
Day 2
Day 3
Day 4
Day 5
Day 6
Unit 11 HW
Unit 11 HW
Dalton’s Law
𝑃𝑇𝑜𝑡𝑎𝑙 = 𝑃1 + 𝑃2 + 𝑃3 …
Ideal Gas Law
𝑃𝑉 = 𝑛𝑅𝑇
𝑃1 𝑉1 𝑃2 𝑉2
=
𝑇1
𝑇2
Combined Gas Law
Boyle’s Law
Charles’s Law
Gay-Lussac’s Law
𝑃1 𝑉1 = 𝑃2 𝑉2
𝑉1 𝑉2
=
𝑇1 𝑇2
𝑃1 𝑃2
=
𝑇1 𝑇2
STP
Temperature: 273K = 0°C
Pressure: 101.3 kPa = 1.0 atm = 760 mmHg
K = °C + 273
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Unit 11 HW
11.1 GASES AND THE FOUR VARIABLES
For numbers 1-3, CIRCLE the italicized term that best completes the sentence.
1. During gas particle collision, kinetic energy…
( increases / decreases / stays the same).
2. As temperature increases, kinetic energy…
( increases / decreases / stays the same).
3. As the speed of gas molecules increases, kinetic energy…
( increases / decreases / stays the same).
4. Why are gases able to be compressed?
5. The SI unit for volume is _________________, pressure is ______________, and temperature is _________.
6. Convert the following.
a. 24 °C
_____ K
b. 58 °C
_____ K
c. 54 K
_____ °C
d. 324 K _____ °C
7. Convert the following.
a. 1.01 atm
_____ mmHg
b. 98.4 kPa
_____ atm
c. 0.95 atm
_____ kPa
d. 104.5 kPa _____ mmHg
8. What is absolute zero?
________________________________________________________
Unit 11 HW
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9. You have a sample of a gas in a sealed, rigid (cannot be stretched or enlarged) cylinder. If you INCREASE the
temperature of the cylinder, what happens to…
a. …the kinetic energy of the gas molecules.
__________________________________________________________________
__________________________________________________________________
b. …The pressure exerted by the gas molecules on the walls of the container.
____________________________________________________________
__________________________________________________________________
c. …The speed of the gas molecules.
__________________________________________________________________
__________________________________________________________________
d.
…The number of collisions of gas molecules with other gas molecules.
__________________________________________________________________
__________________________________________________________________
10. What is the total pressure (in mmHg) exerted by a sample of gases containing 319 mmHg H2, 201 kPa N2, and 0.6
atm O2?
11. If the total pressure of a mixture of O2, N2, and H2 is 902 mmHg, what is the pressure of O2 if there pressure of N2 is
355 mmHg N2 and H2 is 0.3 atm?
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Unit 11 HW
11.2 IDEAL GAS LAW
1. Determine the temperature (in °C ) of 2.49 moles of gas contained in a 1.00 L vessel at a pressure of 143 kPa.
2. What is the pressure (in kPa) of a 0.108 mol sample of helium gas at 20.0 C if its volume is 0.505 L?
3. Calculate the number of moles of gas that occupy a 3.45 L container at a pressure of 150 kPa and a temperature of
45.6 C.
4. If 0.2804 mol of methane gas (CH4) is introduced into a 2.00 L container at 35 C, what is the pressure in the
container?
5. A 2.00 L flask is filled with propane gas (C3H8) at 101.3 kPa and –15.0 C. What is the mass (in grams) of the propane
in the flask? (Hint: Convert moles to grams!)
Unit 11 HW
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6. Determine the pressure inside a television picture tube with a volume of 3.50 L that contains 2.00 x 10 –5 grams of
nitrogen gas at 22.0 C. (Hint: Convert grams to moles!
7. How many grams of oxygen gas must be present in a 2.00 L container at 35 C if the pressure is 212 kPa at 25oC?
Page 8 of 12
Unit 11 HW
11.3 COMBINED GAS LAW
For Questions 1-4, circle the correct answer
1. Assuming volume and temperature are held constant in a sealed container, what happens to pressure when more
molecules of gas are injected?
A – Decreases
B. Increases
C. Stays the Same
D. Cannot Determine
2. When the volume of a container is increased, the pressure inside the cylinder …….
A – Decreases
B. Increases
C. Stays the Same
D. Cannot Determine
3. As a gas heats up the average kinetic energy of its molecules will ….
A – Decreases
B. Increases
C. Stays the Same
D. Cannot Determine
4. Assuming pressure and temperature are held constant in a balloon, what happens to volume as gas molecules are
removed?
A – Decreases
B. Increases
C. Stays the Same
D. Cannot Determine
5. A helium filled balloon at sea level has a volume of 2.10 L at 0.998 atm and 36 C. If it is released and rises to an
elevation at which the pressure is 0.900 atm and the temperature is 28 C, what will be the new volume of the
balloon?
6. At 20.0 C and 1.00 atm pressure, a sample of gas occupies 0.03 L. If the temperature is increased to 30.0 C and the
entire sample is transferred to a 0.02 L container, what will be the gas pressure inside the container?
Unit 11 HW
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7. A sample of air in a syringe exerts a pressure of 1.02 atm at a temperature of 22.0 C. The syringe is then placed in a
boiling water bath at 100.0 C. The pressure of the air is increased to 1.23 atm by pushing the plunger in, which
reduces the volume to 0.224 L. What was the original volume of air?
8. An unopened cold 2.00 L soda bottle contains 46.0 mL of gas confined at a pressure of 1.30 atm at a temperature of
5.0 C. If the bottle is dropped into a lake and sinks to a depth at which the pressure is 2.85 atm and temperature is
2.09 C, what will the volume of the gas in the bottle be?
9. A sample of unknown pressure occupies 0.766 L at a temperature of 298 K. The same sample of gas is then tested
under known conditions and has a pressure of 32.6 kPa and occupies 0.644 L at 303 K. What was the original
pressure of the gas?
10. A gas at 110 kPa and 30.0 C fills a flexible container with an initial volume of 2.00 L. If the temperature is raised to
80.0 C and the pressure is increased to 440 kPa, what is the new volume?
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Unit 11 HW
11.4 INDIVIDUAL GAS LAWS
Read each question. Circle the gas law that applies to the problem. Then, solve for the missing variable.
1. If a basketball has a volume 2.5 L and a temperature of 25 °C, what will its new volume be if it is left in the cold at
temperature of – 10 °C? Assume that pressure remains constant.
( Boyle’s / Charles’s / Gay – Lussac’s )
2. If a balloon has a pressure of 1.3 atm and a temperature of 100 °C. If volume remains constant, and its temperature
is raised to 215 °C, what will the new pressure be? ( Boyle’s / Charles’s / Gay- Lussac’s )
3. If a balloon has a volume of 3 L and a pressure of 600 mmHg, what will its pressure be if its volume decreases to 2 L?
Assume that temperature remains constant. ( Boyle’s / Charles’s / Gay-Lussac’s )
4. If a ball has an initial temperature of 315 K, what will its final temperature be if the pressure is changed from 1.2 atm
to 13.2 atm? Assume that volume remains constant.
( Boyle’s / Charles’s / Gay – Lussac’s )
5. A ball has a volume of 3.5 L and a pressure of 450 kPa. If temperature remains constants, how large will the volume
be if we increase the pressure to 550 kPa?
( Boyle’s / Charles’s / Gay – Lussac’s )
6. If a balloon has a volume of 3.2 L at 273 K, what will its volume be at 473 K? Pressure is held constant.
( Boyle’s / Charles’s / Gay – Lussac’s )
Unit 11 HW
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Unit 11 HW