A question of the Intercompatibility of the Gas Laws.

[modulus]

I was recently taught about the three gas laws:

1)Boyle's Law, which stated that pressure is inversely proportional to volume and vice-versa at a constant temperature.

2)Charle's Law, which stated that volume is directly proportional to temperature at a a constant pressure

3)Amonton Law, which stated that pressure is directly proportional to temperature at a constant volume.

I have no confusion regarding the first two laws, but, I don't understand how increasing temperature would increase pressure (Amonton's Law) unless the gas is in an enclosed container (so that when it's temp. is increased, it's volume increases too, which will cause it's molecules to collide with the container more often to produce more pressure).
If we consider Amonoton's Law to be in the context of a closed container, then Boyle's Law and Charle's Law would also be in the context of a closed container (because the three laws are used together to derive the gas equation PV=nRT). But, then Boyle's Law would make no sense.
So, the three laws are not intercompatible, which means the gas equation is wrong ... but ... how??

 

[TheDestroyer]

I have no confusion regarding the first two laws, but, I don't understand how increasing temperature would increase pressure (Amonton's Law) unless the gas is in an enclosed container (so that when it's temp. is increased, it's volume increases too, which will cause it's molecules to collide with the container more often to produce more pressure).

Your perspective about the pressure is totally right, but you've overlooked the fact that you're studying the gas not the container that contains the gas. When you want to study the gas, you put it in different containers and in different circumstances and watch how it'll act in every environment, so you can give a general law for it everywhere in any situation.
Eventually, you can combine everything you saw in 1 law that tells you everything you want in every environment, which means that the general law (ideal gas law) should agree with the 3 partial laws you've seen in the experiment, which is the case in in the ideal gas law PV=nRT when you set any of the 3 variables to be a constant.

If this answer doesn't convince you, ask again and you're welcome :)

Good luck :)

 

[sir-pinski]

It is understandable to have confusion about the intercompatibility of the gas laws, as they can seem contradictory at first glance. However, it is important to keep in mind that these laws were developed under specific conditions and may not apply in all situations.

Boyle's Law, Charles's Law, and Amonton's Law were all formulated based on experiments conducted with ideal gases, which are gases that follow certain assumptions such as having no intermolecular forces and occupying no volume. In reality, most gases do not behave exactly like ideal gases, especially at high pressures and low temperatures.

Furthermore, these laws were developed independently and may not be applicable in all situations. For example, Boyle's Law assumes that temperature remains constant, while Charles's Law assumes that pressure remains constant. These conditions may not always be true in real-world scenarios.

The gas equation PV=nRT is a combination of these three laws and is used to describe the behavior of ideal gases. It is important to note that this equation is an approximation and may not hold true for all gases under all conditions.

In conclusion, while the three gas laws may seem contradictory, they are still useful in understanding the behavior of gases under certain conditions. It is important to keep in mind their limitations and the fact that they were developed based on ideal gas behavior.