A chemistry student relates the following story: I noticed \(\mathrm{my}\) tires were a bit low and went to the gas station. As I was filling the tires, I thought about the kinetic molecular theory (KMT). noticed the tires because the volume was low, and I realized that I was increasing both the pressure and volume of the tires "Hmmm," I thought, "that goes against what I learned in chemistry, where I was told pressure and volume are inversely proportional." What is the fault in the logic of the chemistry student in this situation? Explain why we think pressure and volume to be inversely related (draw pictures and use the KMT).

The fault in the chemistry student's logic is the assumption that increasing both the pressure and volume of the tires simultaneously contradicts the inverse relationship between pressure and volume in Boyle's Law. However, Boyle's Law only applies when the temperature and amount of gas (air) remain constant. In this situation, the student is adding more gas (air) to the tires, resulting in an increase in both pressure and volume. This does not violate Boyle's Law, as the amount of gas in the tires is changing. The Kinetic Molecular Theory explains the relationship between pressure and volume through collisions between gas particles and their container walls, which vary according to the amount of gas present and the volume of the container.