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Results:
What did you notice when you pushed the plunger in? What happens to the volume of air inside the syringe? Did it become more or less difficult to push the plunger in as the volume of the air in the syringe decreased? In other words, did you have to apply more or less force to the plunger as the volume of air in the syringe decreased?
As the volume of air in the syringe decreases, you have to apply more force to the plunger to keep pressing it down. The pressure of the gas inside the syringe pushing back on the plunger is greater. Another way of saying this is that as the volume of the gas in the syringe decreases , the pressure of that gas increases .
Conclusion:
If the volume of the gas decreases, the pressure of the gas increases. If the volume of the gas increases, the pressure decreases. These results support Boyle's law.
In the previous demonstration, the volume of the gas decreased when the pressure increased, and the volume increased when the pressure decreased. This is called an inverse relationship . The inverse relationship between pressure and volume is shown in [link] .
Can you use the kinetic theory of gases to explain this inverse relationship between the pressure and volume of a gas? Let's think about it. If you decrease the volume of a gas, this means that the same number of gas particles are now going to come into contact with each other and with the sides of the container much more often. You may remember from earlier that we said that pressure is a measure of the frequency of collisions of gas particles with each other and with the sides of the container they are in. So, if the volume decreases, the pressure will naturally increase. The opposite is true if the volume of the gas is increased. Now, the gas particles collide less frequently and the pressure will decrease.
It was an Englishman named Robert Boyle who was able to take very accurate measurements of gas pressures and volumes using high-quality vacuum pumps. He discovered the startlingly simple fact that the pressure and volume of a gas are not just vaguely inversely related, but are exactly inversely proportional . This can be seen when a graph of pressure against the inverse of volume is plotted. When the values are plotted, the graph is a straight line. This relationship is shown in [link] .
The pressure of a fixed quantity of gas is inversely proportional to the volume it occupies so long as the temperature remains constant.
During this chapter, the terms directly proportional and inversely proportional will be used a lot, and it is important that you understand their meaning. Two quantities are said to be proportional if they vary in such a way that one of the quantities is a constant multiple of the other, or if they have a constant ratio. We will look at two examples to show the difference between directly proportional and inversely proportional .
Time (mins) | Distance (km) |
10 | 20 |
20 | 40 |
30 | 60 |
40 | 80 |
Speed (km/h) | Time (mins) |
100 | 60 |
80 | 75 |
60 | 100 |
40 | 150 |
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