# Gas Law

Topics: Pressure, Ideal gas law, Thermodynamics Pages: 7 (2135 words) Published: January 28, 2013
Complete ALL problems under each heading in your packer. SHOW ALL WORK AND LABELS!

Bolye’s Law Problems

Example: 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? • Read the problem and determine what is given and what is unknown? • Decide which law to use.

• Substitute the values (given numbers) from the problem into the equation Given: P1 = 1.5 atmUnknown or find: P2 = ? = X
V1 = 5.6 L
V2 = 4.8 L
Note: Since this problem involves two pressures and two volumes we will use Boyle’s law equation to solve it: P1V1 = P2V2

(1.5) (5.6) = X (4.8)
Now solve for X

8.4 = 4.8 X
4.8 4.8

1.75 atm = X = P2 The new pressure inside the piston is 1.75 atm.

1. I have added 15 L of air to a balloon at sea level (1.0 atm). If I take the balloon with me to Denver, where the air pressure is 0.85 atm, what will the new volume of the balloon be?

2. I’ve got a car with an internal volume of 12,000 L. If I drive my car into the river and it implodes, what will be the volume of the gas when the pressure goes from 1.0 atm to 1.4 atm?

3. 1.0 L of a gas at standard temperature and standard pressure is compressed to 473 mL. What is the new pressure of the gas?

4. In a thermonuclear device, the pressure of 0.050 liters of gas within the bomb casing reaches 4.0 x 106 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?

5. Synthetic diamonds can be manufactured at pressures of 6.00 x 104 atm. If we took 2.00 liters of gas at 1.00 atm and compressed it to a pressure of 6.00 x 104 atm, what would the volume of that gas be?

6. The highest pressure ever produced in a laboratory setting was about 2.0 x 106 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?

7. 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 104 mm Hg, what will be the volume of the gas when it is released from the tanks?(hint: convert pressure into atm)

8. While using explosives to knock down a building, the shock wave can be so strong that 12 liters of gas will reach a pressure of 3.8 x 104 mm Hg. When the shock wave passes and the gas returns to a pressure of 760 mm Hg, what will the volume of that gas be? (hint: convert pressure into atm)

9. 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?

10. Divers get “the bends” if they come up too fast because gas in their blood expands, forming bubbles in their blood. If a diver has 0.05 L of gas in his blood under a pressure of 250 atm, then rises instantaneously to a depth where his blood has a pressure of 50.0 atm, what will the volume of gas in his blood be? Do you think this will harm the diver?

Charles’ Law Problems

Example: If I have 45 liters of helium in a balloon at 250 C and increase the temperature of the balloon to 550 C, what will the new volume of the balloon be? • Read the problem and determine what is given and what is unknown? (Convert temperature into Kelvin) • Decide which law to use.

• Substitute the values (given numbers) from the problem...

Please join StudyMode to read the full document