Boyle's Law in Physics

 
BOYLE’S LAW
 
WJEC Physics Unit 1 - 1.8
WJEC Physics Unit 1 - 1.8
 
GAS
Click to
compress
the gas
 
Pressure
gauge
 
Squashy gases
 
You can squash a gas into a smaller volume. If you do this
without letting any gas escape from the container, or letting it
get hotter, then the pressure on the gas will also go up.
 
Digital
thermometer
 
1
 
2
 
3
 
4
 
5
 
6
 
7
 
0
 
GAS
Click to
compress
the gas
 
Pressure
gauge
 
Squashy gases
 
Have another look. Can you see any relationship between the
volume of the gas and the pressure?
Why does the pressure gauge start at 1?
 
Digital
thermometer
 
1
 
2
 
3
 
4
 
5
 
6
 
7
 
0
 
Pressure
(atmospheres)
 
Volume
(m
3
)
 
1
 
2
 
3
 
4
 
5
 
6
 
7
 
8
 
1
 
2
 
3
 
4
 
5
 
6
 
7
 
8
 
Squashy gases
 
Let’s consider a gas of volume 8m
3
 being
compressed to half its volume – what would
happen to its pressure?
 
Can you estimate the points on the graph as
the volume is halved 3 times, and the shape
of the line before revealing them?
Show points
Show graph line
 
It turns out that the pressure goes up in proportion to the amount of squashing you do.
If you squash the gas into half the amount of space then the pressure will double.
This works the other way, too. If you increase the pressure on a gas, without letting it
change temperature, it will squash into a smaller volume.
 
GAS
Show
molecules
within the gas
 
Pressure
gauge
 
How does this work?
 
Kinetic theory can explain the link between pressure and
volume. The pressure a gas exerts on a container depends on
two things: how fast the particles are zipping around  and
how often they hit the walls of the container.
 
Digital
thermometer
 
1
 
2
 
3
 
4
 
5
 
6
 
7
 
0
Compress gas
1
2
GAS
Show
molecules
within the gas
Pressure
gauge
How does this work?
If we squash the gas into a smaller space the particles bash
into the walls of the container more often and the pressure
increases. The speed of the particles will not change unless
the temperature changes.
Digital
thermometer
1
2
3
4
5
6
7
0
1
 
Boyle’s Law
 
Boyle’s law sums up the link between the
volume and pressure of a gas:
“When the pressure is increased on a fixed mass of
gas, kept at constant temperature, the volume will
decrease. The changes in pressure and volume are
in inverse proportion.”
 
Complete this summary of Boyle’s law.
Click the appropriate arrow to move the statement to the desired section
 
Boyle’s Law
If you increase the
volume of a gas the
pressure must
If you increase the
pressure of a gas the
volume must
If you decrease the
pressure the volume
must
If you decrease the
volume the pressure
must
 
Boyle’s law in Action
 
TASK:
Click on the syringe on the following animation to change the volume of the
gas inside the syringe.
Take at least 5 values of pressure and volume using the data in the animation.
 
 
 
 
 
 
Plot a suitable graph to represent your data.
 
Click the image to access the activity.
(Please note that this activity is flash based and
may not work in some browsers)
 
The equation
 
There is an equation to go with Boyle’s Law:
V
1
 = 320 cm
3
 
p
1
 = 2.5 atm
 
V
2
 = 180 cm
3
 
p
1
V
1
 = p
2
V
2
2.5 x 320 = p
2
 x 180
p
2
 = 
(2.5 x 320)
              180
p
2
 = 4.4 atm
p
1
V
1
 = p
2
V
2
 
Let’s look at an example:
A gas starting off at a volume of 320 cm
3
 and pressure of 2.5
atmospheres is compressed down to a volume of 180 cm
3
.
What is the final pressure?
 
p
1
 and V
1
 are the pressure
and volume of the gas at the
start and p
2
, V
2
 are the final
pressure and volume.
 
Solve these questions using the formula p
1
V
1
 = p
2
V
2
 
1.
A gas starting off at a volume of 2,000 cm
3
 and pressure of 5.5
atmospheres is compressed down to a volume of 500 cm
3
. What
is the final pressure?
2.
A gas in a volume of 550 cm
3
 is compressed down to a new
volume of 175 cm
3
 and has a new pressure of 4.7 atm. What was
the initial pressure?
3.
After compressing a gas  from 700 cm
3
 the pressure was found
to have risen from 3 atm to 6 atm. What was the final volume?
4.
A gas starts with a pressure of 2.5 atmospheres and is
compressed so that its final volume is one quarter of its initial
volume. What is the final pressure of the gas?
5.
In what volume did the gas at 3.1 atm start if its final pressure is
4.5 and its final volume is 600 cm
3
?
Answers
1.
22 atm
2.
1.5 atm
3.
350 cm
3
4.
10 atm
5.
 871 cm
3
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Boyle's Law explains the relationship between the volume and pressure of a gas. When pressure increases on a fixed mass of gas at constant temperature, the volume decreases. This inverse proportion between pressure and volume can be explained by the Kinetic Theory, where the speed of gas particles and their collisions with the container walls play a crucial role. As the gas is compressed into a smaller space, the particles collide more frequently, resulting in increased pressure. This fundamental principle is illustrated through interactive visuals and practical examples.

  • Boyles Law
  • Physics
  • Pressure
  • Gas Volume
  • Kinetic Theory

Uploaded on Aug 02, 2024 | 1 Views


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  1. BOYLES LAW WJEC Physics Unit 1 - 1.8

  2. Squashy gases You can squash a gas into a smaller volume. If you do this without letting any gas escape from the container, or letting it get hotter, then the pressure on the gas will also go up. Digital 0 thermometer 1 7 20 C 6 2 Pressure gauge 4 5 3 Click to compress the gas GAS

  3. Squashy gases Have another look. Can you see any relationship between the volume of the gas and the pressure? Why does the pressure gauge start at 1? Digital 0 thermometer 1 7 20 C 6 2 Pressure gauge 4 5 3 Click to compress the gas GAS

  4. Squashy gases Pressure (atmospheres) Let s consider a gas of volume 8m3 being compressed to half its volume what would happen to its pressure? 8 7 Can you estimate the points on the graph as the volume is halved 3 times, and the shape of the line before revealing them? 6 5 4 3 2 Show points 1 Show graph line Volume (m3) 1 2 3 4 5 6 7 8 It turns out that the pressure goes up in proportion to the amount of squashing you do. If you squash the gas into half the amount of space then the pressure will double. This works the other way, too. If you increase the pressure on a gas, without letting it change temperature, it will squash into a smaller volume.

  5. How does this work? Kinetic theory can explain the link between pressure and volume. The pressure a gas exerts on a container depends on two things: how fast the particles are zipping around and how often they hit the walls of the container. Digital 0 thermometer 1 7 20 C 6 2 Pressure gauge 4 1 5 Show molecules within the gas 3 Compress gas 2 GAS Compress gas

  6. How does this work? If we squash the gas into a smaller space the particles bash into the walls of the container more often and the pressure increases. The speed of the particles will not change unless the temperature changes. Digital 0 thermometer 1 7 20 C 6 2 Pressure gauge 4 1 5 Show molecules within the gas 3 GAS

  7. Boyles Law Boyle s law sums up the link between the volume and pressure of a gas: When the pressure is increased on a fixed mass of gas, kept at constant temperature, the volume will decrease. The changes in pressure and volume are in inverse proportion.

  8. Boyles Law Complete this summary of Boyle s law. Click the appropriate arrow to move the statement to the desired section Decrease Increase If you increase the volume of a gas the pressure must If you increase the pressure of a gas the volume must If you decrease the pressure the volume must If you decrease the volume the pressure must

  9. Boyles law in Action TASK: Click on the syringe on the following animation to change the volume of the gas inside the syringe. Take at least 5 values of pressure and volume using the data in the animation. Click the image to access the activity. (Please note that this activity is flash based and may not work in some browsers) Plot a suitable graph to represent your data.

  10. The equation There is an equation to go with Boyle s Law: p1 and V1 are the pressure and volume of the gas at the start and p2, V2 are the final pressure and volume. p1V1 = p2V2 Let s look at an example: A gas starting off at a volume of 320 cm3 and pressure of 2.5 atmospheres is compressed down to a volume of 180 cm3. What is the final pressure? V1 = 320 cm3 V2 = 180 cm3 p1 = 2.5 atm p1V1 = p2V2 2.5 x 320 = p2 x 180 p2 = (2.5 x 320) 180 p2 = 4.4 atm

  11. Solve these questions using the formula p1V1 = p2V2 A gas starting off at a volume of 2,000 cm3 and pressure of 5.5 atmospheres is compressed down to a volume of 500 cm3. What is the final pressure? A gas in a volume of 550 cm3 is compressed down to a new volume of 175 cm3 and has a new pressure of 4.7 atm. What was the initial pressure? After compressing a gas from 700 cm3 the pressure was found to have risen from 3 atm to 6 atm. What was the final volume? A gas starts with a pressure of 2.5 atmospheres and is compressed so that its final volume is one quarter of its initial volume. What is the final pressure of the gas? In what volume did the gas at 3.1 atm start if its final pressure is 4.5 and its final volume is 600 cm3? 1. 2. 3. 4. 5.

  12. Answers 1. 2. 3. 4. 5. 22 atm 1.5 atm 350 cm3 10 atm 871 cm3

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