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Chapter 10 & 12 Worksheets
Monday Bellwork
Worksheet #1: The Kinetic Theory
1. Convert the following measurements. Be sure to show your work in the box provided.
Atmospheres mmHg kPa
2.11
825.0
0.69
109.4
2. Molly has two samples in her lab. She has 2 liters of water and 2 liters of oxygen gas. How would each sample differ in the following scenarios?
a. Each sample is transferred into a larger container.
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b. Each sample is heated from 250K to 300K.
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c. Each sample is compressed with a piston.
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3. Two balloons are each filled with 1L of He. Balloon A is taken to Corpus Christi in Texas. Balloon B is taken to the top of a mountain in Washington. Describe the size of EACH balloon once they have reached their destination and explain why they changed in size.
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4. Trey has a balloon filled with nitrogen. When released, it slowly rises, but after a few minutes, pops. What happened and why?
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Worksheet #2: The Gas Laws
1. If a gas is compressed from 4 L to 1 L and the temperature remains constant, what happens to the pressure?
2. The gas in a closed container has a pressure of 3.00 x 102 kPa at 30oC. What will the pressure be if
the temperature is lowered to -172oC?
3. Calculate the volume of carbon dioxide gas (in L) at a pressure of 844 kPa if its volume at 536 kPa is 1.50x 103mL.
4. A gas with a volume of 4.0 L at 90.0 kPa expands until the pressure drops to 20.0 kPa. What is the new volume if the temperature remains constant?
5. A gas with a volume of 849.0 mL at 150.0oC is heated until its volume is 5.707 L. What is the new
temperature of the gas if the pressure remains constant during the heating process?
6. A sealed cylinder of gas contains nitrogen gas at 1.00 x 103kPa pressure and a temperature of
20.0oC. The cylinder is left in the sun, and the temperature of the gas increases to 50.0oC. What is
the new pressure in the cylinder?
7. Calculate the number of liters occupied at STP.
a. 2.5 mol N2(g) c. 0.600 g H2(g)
b. 0.350 mol O2(g)
8. If you put a straw into water, place your finger over the mouth opening, then lift the straw, what would you see and why?
Wednesday Bellwork
Worksheet #3: The Ideal Gas Law
1. What is the Ideal Gas Law? List the variables and the unit each must be in.
2. If I have 4.0 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature of the gas?
3. Betty has an unknown quantity of gas at a pressure of 1.2 atm, a volume of 31 liters, and a temperature of 87 0C. How many moles of gas does she have?
4. 3.5 moles of nitrogen gas is sealed in a metal container with a volume of 60.0 mL at a temperature of 400 K. What is the pressure inside the container?
5. If 4.50g of methane gas (CH4) is introduced into an evacuated 2.00L container at 35.0oC, what is
the pressure in the container?
6. A metal tank contains three gases: oxygen, helium, and nitrogen. If the partial pressures of the three gases in the tank are 35 atm of O2, 5 atm of N2, and 25 atm of He, what is the total pressure
inside of the tank?
7. Blast furnaces give off many unpleasant and unhealthy gases. If the total air pressure is 0.99 atm, the partial pressure of carbon dioxide is 0.05 atm, and the partial pressure of hydrogen sulfide is 0.02 atm, what is the partial pressure of the remaining gases?
Worksheet #4: Solids and Liquids
1. In the spaces below, draw pictures of the particles of solids, liquids and gases.
Solid Liquid Gas
2. Match the term with the situation described below.
a. Evaporation _____ Particles of a gas cool and become a liquid
b. Condensation _____ Particles of a gas bump into the walls of their container c. Boiling point _____ Particles of a liquid heat up enough to become a gas d. Vapor pressure _____ Particles of a liquid cool a surface by absorbing heat to
become a gas
3. Why do you think it is easier to cool off by sweating in dry conditions rather than humid conditions?
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4. For each of the following, write a letter “H” if the substance has a high melting point or a letter “L” if it has a low melting point.
a. _____ H2O
b. _____ MgCl2
c. _____ CH4
d. _____ BeO e. _____ Fe2O3
5. A weather balloon is designed to hold no more than 2.5L of gas. It the balloon is filled with 2.0L of helium at sea level, then released, will it burst if the pressure decreases to 500. mmHg? Assume the temperature is constant.
6. Complete the following table for an ideal gas. Show all work in the boxes provided.
P (atm) V (L) n (mol) T
5.00 2.00 155°C
0.300 2.00 155K
4.47 25.0 2.01
2.25
10.5 75°C
7. A 2.50 liter container is filled with 175 grams of argon gas. a. If the pressure is 10.0 atm, what is the temperature?
b. If the temperature is 225K, what is the pressure?
Tuesday Bellwork
Chapter 10 and 12 Review Sheet
The following are problems that involve all of the gas laws we have learned. In order to solve these problems, you must use the variables to determine which formula needs to be used.
1. What would the temperature of a gas be if a 0.268 mole sample occupied a volume of 7290mL at a pressure of 1.83atm?
2. What would be the volume (in mL) of an ideal gas if a 0.245 mole sample had a temperature of 20°C at a pressure of 988.5 mmHg?
3. 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?
4. What would be the pressure if a 0.753 mole sample of carbon dioxide gas occupied a volume of 8110 mL at a temperature of 82.5°C?
5. 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?
6. If 4.77 moles of a gas at a pressure of 5.4 atmospheres has a volume of 120 mL, what is the temperature?
7. If I initially have a gas with a pressure of 845 kPa and a temperature of 35.00 C and I heat it an
8. 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 760
mm Hg.
9. How many moles of gas are in my car in problem #9? (Hint: Pick one set of P,V, T, and you know R)
10. A sealed canister contains three gasses. Gas A has a partial pressure of 1.4 atm. Gas B has a partial pressure of 0.44 atm. If the total pressure of the gasses is 3.75 atm, what is the partial pressure of gas C?
11. Which of the soda containers below would be most likely to spew soda if you opened it? Show work to explain.
T = 22.4ºC T = 46.7°C T = 19.3ºC
P = ? P = ? P = ?
V = 354 ml V = 2.0 L V = 244 ml
n = 1.66 mol CO2 n = 2.33 mol CO2 n = 1.83 mol CO2
12. Explain why a scuba diver might die if he/she rose too quickly to the surface after a deep dive.
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