Name: _______________________
Boyle’s Law
Date: _________
Gas Laws Worksheet Part 1
Charles’s Law
Guy-Lassac’s Law
Period: ______
Combined Gas Law
For a given mass of gas at constant temperature, the volume of a gas varies inversely with pressure
𝑃
1
× 𝑉
1
= 𝑃
2
× 𝑉
2
The volume of a fixed mass of gas is directly proportional to its
Kelvin temperature if the pressure is kept constant.
𝑉
1
𝑇
1
Or
𝑉
1
× 𝑇
2
=
𝑉
2
𝑇
2
= 𝑉
2
× 𝑇
1
The pressure of a gas is directly proportional to the Kelvin temperature if the volume is kept constant.
Or
𝑃
1
𝑃
𝑇
× 𝑇
1
1
2
=
𝑃
2
𝑇
2
= 𝑃
2
× 𝑇
1
Combines Boyle’s,
Charles’, and the
Temperature-Pressure relationship into one equation. Each of these laws can be derived from this law.
Or
𝑃
1
𝑃
1
× 𝑉
1
× 𝑉
1
𝑇
1
× 𝑇
2
=
𝑃
2
× 𝑉
2
𝑇
2
= 𝑃
2
× 𝑉
2
× 𝑇
1
Ideal Gas Law
The Ideal Gas Law relates the pressure, temperature, volume, and mass of a gas through the gas constant “R”.
Dalton’s Law
𝑃 × 𝑉 = 𝑛 × 𝑅 × 𝑇
Or 𝑃 𝑡𝑜𝑡𝑎𝑙
= 𝑃
1
+ 𝑃
2
+ 𝑃
3
+ . . ..
𝑃𝑉 = 𝑛𝑅𝑇
Abbreviation atm = atmosphere mm Hg = millimeters of mercury torr = another name for mm Hg
Pa = Pascal kPa = kilopascal
K = Kelvin
°C = degrees Celsius
Conversions
K = °C + 273
°F  1.8°C 
32
°C =
1 cm
3
°F − 32
1.8
(cubic centimeter) = 1 mL (milliliter)
1 dm
3
(cubic decimeter) = 1 L (liter) = 1000 mL
𝑅𝑎𝑡𝑒
𝐴
𝑅𝑎𝑡𝑒
𝐵
=
√𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠
𝐴
√𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠
𝐵
Standard conditions
0°C = 273 K
1.00 atm = 760.0 mm Hg = 76 cm Hg =
101.3 kPa = 101, 300 Pa = 29.9 in Hg problem
Gas Law’s Equation Symbols
Subscript (1) = old condition or initial condition
Subscript (2) = new condition or final condition
Temperature must be in Kelvins n = number of moles = grams/Molar mass
R = 8.31
L·kPa
K·mol
or 0.0821
L·atm
K·mol
You must have a common set of units in the
At constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the pressures exerted by each gas,
Graham’s Law
The rate of effusion/diffusion of two gases (A and B) are inversely proportional to the square roots of their formula masses.

1. Convert the following temperatures to K. a) 104 C b) -3 C
2. Convert the following temperatures to C. a) 67 K b) 1671 K
3. A sample of nitrogen gas has a volume of 478 L and a pressure of
104.1 kPa. What volume would the gas occupy at 88.2 kPa if the temperature remains constant?
4. 8.98 mL of hydrogen gas is collected at 38.8 °C. Find the volume the gas will occupy at -
39.9 °C if the pressure remains constant.
5. A sample of gas has a volume of 215 L at 23.5 °C and 84.6 kPa.
What volume will the gas occupy at STP (standard temperature and pressure)?
6. A 495 mL of oxygen gas at
25.0 °C and 114.7 kPa, is put in a
536 mL flask. Find the total pressure in the flask, assuming the temperature remains constant.

7. A sample of gas is transferred from a 75 mL vessel to a 500.0 mL vessel. If the initial pressure of the gas is 145 atm and if the temperature is held constant, what is the pressure of the gas sample in the 500.0 mL vessel?
8. A sample of gas occupies a volume of 450.0 mL at 740 mm
Hg and 16°C. Determine the volume of this sample at
760 mm Hg and 37°C.
9. Convert a pressure of 0.0248 mm Hg to the equivalent pressure in kPa.
10. Air in a closed cylinder is heated from 25°C to 36°C. If the initial pressure is 3.80 atm, what is the final pressure?
11. A bubble of helium gas has a volume of 0.650 mL near the bottom of a large aquarium where the pressure is 1.54 atm and the temperature is 12°C. Determine the bubble’s volume upon rising near the top where the pressure is
760 torr and 16°C.
12. What is the pressure in mm of
Hg , of a gas mixture that contains
1g of H2, and 8.0 g of Ar in a 3.0
L container at 27°C.

Name: _______________________
13. To what temperature must
32.0 ft 3 of a gas at 2°C be heated for it to occupy 100.0 ft 3 at the same pressure? {HINT: ft 3 is a unit of volume)
Date: _________
Gas Laws Worksheet Part 2
14. A bag of potato chips is packaged at sea level (1.00 atm) and has a volume of 315 mL. If this bag of chips is transported to
Denver (0.775 atm), what will the new volume of the bag be?
15. A Los Angeles class nuclear submarine has an internal volume of eleven million liters at a pressure of 1.250 atm. If a crewman were to open one of the hatches to the outside ocean while it was underwater (pressure =
15.75 atm), what be would the new volume of the air inside the submarine?
16. A child has a toy balloon with a volume of 1.80 liters. The temperature of the balloon when it was filled was 20 0 C and the pressure was 1.00 atm. If the child were to let go of the balloon and it rose 3 kilometers into the sky where the pressure is 0.667 atm and the temperature is -10 0 C, what would the new volume of the balloon be?
17. A commercial airliner has an internal pressure of 1.00 atm and temperature of 25 0 C at takeoff. If the temperature of the airliner drops to 17 0 C during the flight, what is the new cabin pressure?
Period: ______

18. If divers rise too quickly from a deep dive, they get a condition called “the bends” which is caused by the expansion of very small nitrogen bubbles in the blood due to decreased pressure. If the initial volume of the bubbles in a diver’s blood is 15 mL and the initial pressure is 12.75 atm, what is the volume of the bubbles when the diver has surfaced to 1.00 atm pressure?
19. The temperature inside my refrigerator is about 4 0 Celsius. If
I place a balloon in my fridge that initially has a temperature of 22 0 C and a volume of 0.5 liters, what will be the volume of the balloon when it is fully cooled by my refrigerator?
20. 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 0 C, and I leave it in my car which has a temperature of 60 0 C, what will the new volume of the bag be?
21. A soda bottle is flexible enough that the volume of the bottle can change even without opening it. If you have an empty soda bottle (volume of 2 L) at room temperature (25 0 C), what will the new volume be if you put it in your freezer (-4 0 C)?

22. I have made a thermometer which measures temperature by the compressing and expanding of gas in a piston. I have measured that at 100 0 C the volume of the piston is 20 L. What is the temperature outside if the piston has a volume of 15 L? What would be appropriate clothing for the weather?
23. 1.00 L of a gas at standard temperature and pressure is compressed to 473 mL. What is the new pressure of the gas?
24. In a thermonuclear device, the pressure of 0.050 liters of gas within the bomb casing reaches
4.0 x 10 6 atm. When the bomb casing is destroyed by the explosion, the gas is released into the atmosphere where it reaches a pressure of 1.00 atm. What is the volume of the gas after the explosion?
25. The highest pressure ever produced in a laboratory setting was about 2.0 x 10 6 atm. If we have a 1.0 x 10 -5 liter sample of a gas at that pressure, then release the pressure until it is equal to
0.275 atm, what would the new volume of that gas be?

26. 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 3.04 x 10 4 mm Hg, what will be the volume of the gas when it is released from the tanks?
27. Submarines need to be extremely strong to withstand the extremely high pressure of water pushing down on them. An experimental research submarine with a volume of 15,000 liters has an internal pressure of 1.2 atm. If the pressure of the ocean breaks the submarine forming a bubble with a pressure of 250 atm pushing on it, how big will that bubble be?
Ideal gas law problems
28. At what temperature Celsius will 19.4 g of molecular oxygen,
O2, exert a pressure of 1820 mm
Hg in a 5.12 L cylinder?
29. A sample of nitrogen gas,N
2
, is collected in a100 mL container at a pressure of 688 mm Hg and a temperature of 565 °C. How many grams of nitrogen gas are present in this sample?
30. What is the pressure in atm exerted by 2.48 moles of a gas in a
250.0 mL container at 58°C?