• Support PF! Buy your school textbooks, materials and every day products via PF Here!

Boyle's law and pressure problem

  • Thread starter zeithief
  • Start date
27
0
According to boyle's law, P1V1=P2V2 (without temp. change) right?
Therefore when 10cm^3 of oxygen is compresssed into a 5 cm^3 container , the pressure would double right? I believe that the pressure the molecules exerts on the container is due to the force that the molecules exert when they collide with the walls of the container. Therefore, if we compress 10cm^3 of oxygen into another 5cm^3 container of different inner area, will the pressure be different? If it's different will it violate boyle's law? Or there's a missing concept?
Confused boy
 

HallsofIvy

Science Advisor
Homework Helper
41,709
876
You are correct that if you compress a gas to half the volume, you double the pressure. It is NOT true that the surface area of the container affects the pressure. If you have the same amount of gas in the same. What happens is that the total force on the container sides depends on the area. For example, A cube 10 cm by 10 cm by 10 cm has volume 1000 cm3 and surface area 600 cm2 (6 sides each with area 10x10= 100 cm2). A rectangular solid 500 cm by 1 cm by 2 cm also has volume 1000 cmcm3 but now has 2 sides of area 500x1= 500 cm2, two sides of area 500x2= 1000cm2, and two sides of area 1x2= 2cm2 for a total surface area of 3002 cmcm3. Exactly the same amount of gas (same number of molecules) at the same temperature would have the same pressure in both but the latter, with larger surface area would have more total force on the walls.
 
27
0
thank you, it is a good explanation!
:)
 
538
2
According to boyle's law, P1V1=P2V2 (without temp. change) right?
Therefore when 10cm^3 of oxygen is compresssed into a 5 cm^3 container , the pressure would double right? I believe that the pressure the molecules exerts on the container is due to the force that the molecules exert when they collide with the walls of the container. Therefore, if we compress 10cm^3 of oxygen into another 5cm^3 container of different inner area, will the pressure be different? If it's different will it violate boyle's law? Or there's a missing concept?
Confused boy
Yes, when the volume is halved , the pressure doubles under condition that the temperature remains constant.Theoretically, when the volume reduces, the number of molecules remains the same and now they are confined to a much smaller volume ,because the temperature is kept the same , the KE of molecules remains the same but due to smaller volume , the collision with the walls is more rapid and dynamic resulting in increase in pressure.
 

Related Threads for: Boyle's law and pressure problem

  • Posted
Replies
1
Views
2K
  • Posted
Replies
3
Views
1K
Replies
3
Views
662
  • Posted
Replies
10
Views
3K
  • Posted
Replies
16
Views
10K
  • Posted
Replies
9
Views
3K
  • Posted
Replies
1
Views
2K
  • Posted
Replies
1
Views
1K

Physics Forums Values

We Value Quality
• Topics based on mainstream science
• Proper English grammar and spelling
We Value Civility
• Positive and compassionate attitudes
• Patience while debating
We Value Productivity
• Disciplined to remain on-topic
• Recognition of own weaknesses
• Solo and co-op problem solving
Top