Boyle's law and pressure problem

In summary: Therefore, the pressure would be different if the inner area of the container is different, but it would not violate Boyle's law as long as the temperature remains constant.
  • #1
zeithief
29
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
 
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  • #2
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.
 
  • #3
thank you, it is a good explanation!
:)
 
  • #4
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.
 

What is Boyle's Law?

Boyle's Law is a gas law that describes the relationship between pressure and volume of a gas. It states that at a constant temperature, the pressure of a gas is inversely proportional to its volume. In other words, as the volume of a gas decreases, the pressure increases, and vice versa.

What is the equation for Boyle's Law?

The equation for Boyle's Law is P1V1 = P2V2, where P1 and V1 represent the initial pressure and volume, and P2 and V2 represent the final pressure and volume.

How does Boyle's Law relate to real-life scenarios?

Boyle's Law is applicable in various real-life scenarios, such as inflating a bike tire, scuba diving, and operating a syringe. It helps us understand the behavior of gases and how changes in pressure and volume affect their properties.

What is the significance of Boyle's Law in scientific research?

Boyle's Law is an essential concept in the field of chemistry and physics. It is used to predict the behavior of gases in different conditions and to calculate the properties of gases. It also serves as the basis for other gas laws, such as Charles's Law and Gay-Lussac's Law.

What are some common pressure problems related to Boyle's Law?

Some common pressure problems related to Boyle's Law include calculating the volume of a gas at a given pressure, determining the pressure of a gas at a given volume, and finding the final volume of a gas after a change in pressure. These types of problems are commonly encountered in chemistry and physics courses.

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