BOYLE’S LAW P1 X V1 P2 X V2

1011 BOYLE’S LAW IN A VACUUM DESCRIPTION SEVERAL DIFFERENT
A RESOURCE FOR FREESTANDING MATHEMATICS UNITS BOYLE’S LAW BOYLE’S
ACC CHEMISTRY CHAPTER 11 WORKSHEET 1 NAME (BOYLE’S

ALL CHEMISTRY CLASSES BOYLE’S LAW LAB NAME PURPOSE
BOYLE’S LAW P1 X V1 P2 X V2
CLASS COPY BOYLE’S CHARLES’ AND GAYLUSSAC’S GAS PROBLEMS 1

Boyle’s Law

Boyle’s Law

P1 x V1 = P2 x V2

 

Solve the following problems (assuming constant temperation).

 

  1. A sample of nitrogen gas occupies a volume of 175 mL at 740 mm Hg. What volume will it occupy at 800 mm Hg?

 

 

  1. A container of neon has 3.5 liter of gas at 150 kPa pressure. What pressure would the gas exert if the volume is decreased to 1.0 liters?

 

 

  1. A 2.0 liter container of carbon dioxide has a pressure of 3.2 atm. What volume would be necessary to decrease the pressure to 1.0 atm?

 

 

  1. Ammonia gas occupies a volume of 575 mL at a pressure of 850 mm Hg. What volume will it occupy at standard pressure?

 

 

  1. A 278 mL sample of oxygen had its pressure changed from 80 kPa to 150 kPa. What is its new volume?

 

 

  1. A sample of chlorine gas at 3.5 atm had its pressure decreased form 1.2 atm. What was the original volume, if the new volume is 850 mL?

 

 

  1. Fluorine gas occupies a volume of 0.5 Liters at 650 mm Hg pressure. What volume will it occupy at 2.2 mm Hg?

 

 

  1. Hydrogen gas exerts a pressure of 900 mm Hg. When the pressure is changed to 1.50 atm., its volume is 250 mL. What was the original volume?












Boyles’ Law Worksheet


  1. 1.00L of a gas at standard temperature and pressure is compressed to 473mL. What is the new pressure of the gas?









  1. In a thermonuclear device, the pressure of 0.050L 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 1.00atm. What is the volume of the gas after the explosion?









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









  1. 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 L sample of a gas at that pressure, then release the pressure until it is equal to 0.275atm, what would the new volume of that gas be?











  1. 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 10.0L 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?








  1. Part of the reason that conventional explosives cause so much damage is that their detonation produces a strong shock wave that can knock things down. While using explosives to knock down a building, the shock wave can be so strong that 12L 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?








  1. 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 15,000L has an internal pressure of 1.2 atm. If the pressure of the ocean breaks the submarine forming a bubble with a pressure of 250atm pushing on it, how big will that bubble be?








  1. 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 0.05L of gas in his blood under a pressure of 250atm, then rises instantaneously to a depth where his blood has a pressure of 50.0atm, what will the volume of gas in his blood be? Do you think this will harm the diver?



EXCERPT FROM ROBERT BOYLE’S OCCASIONAL REFLECTIONS ON SEVERAL SUBJECTS
EXPERIMENT 6 BOYLE’S AND CHARLES’ LAW NAME DATE
EXPERIMENT 9 EXPERIMENT 9 BOYLE’S LAW PURPOSE 1 TO


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