Essay On Kinetic Molecular Theory

In this essay, it will be discussed how the Kinetic Molecular Theory explains many gas law specifically Boyle’s gas law, Charles’ gas law, and Avogadro’s gas law. To understand what will be talked about is to first know what the Kinetic Molecular Theory is. In our textbook is says it is “A simple model for gases that predicts the behavior of most gases under many conditions.”
First off, we will take a look at Boyle’s Law. As stated in our lab manual “at constant temperature the pressure which a given mass of a gas exerts is inversely relate to its volume: P= k 1/V or PV= k.” The way the Kinetic Molecular Theory explains Boyle’s Law is that gases can be compacted because almost all of the volume of a gas is pretty much empty space. If you were to compact a gas and not change the temperature, the kinetic energy’s average of the gas particles would then stay the same. There wouldn’t be a difference in how fast or slow it is going in which the particles would move but in a container would then be smaller. The particles move from one end of the container to the other end in a small amount of time. Basically, they hit the walls more
Again, in the lab manual is says that “at constant pressure, the volume occupied by a given mass of a gas is directionally proportional to its temperature, measured in degrees Kelvin (˚K= 273+˚C): V=k’T.” The Kinetic Molecular Theory explains Charles’ Law by the average kinetic energy of the particles in a gas is linked to the temperature of the gas. The mass of these particles is constant, so the particles move faster while the gas becomes warmer. If they move faster, the particles will use a bigger force on the container every time they hit the walls in which it will escalate the pressure of the gas. If the walls of the container are flexible, it’ll enlarge until the pressure of the gas balances the pressure of the atmosphere. The volume of the gas gets bigger as the temperature of the gas goes