A sample of oxygen with a volume of 2 L is compressed to a volume of 1 L . * 1 point Based on the kinetic molecular theory of gases, how will the number of collisions and the pressure change when the volume of the gas is decreased? The number of collisions and the pressure both decrease The number of collisions decreases and the pressure increases The number of collisions and the pressure both increase collisions increases and the pressure decreases

When the volume of a gas decreases, like our oxygen sample getting squished from 2 L to 1 L, the gas molecules are forced closer together. This leads to more frequent collisions between the gas molecules and the walls of the container. According to the kinetic molecular theory, this increase in collisions results in an increase in pressure. So, the correct answer here is that the number of collisions and the pressure both increase! It's like a crowded party where everyone is bumping into each other more frequently—definitely more lively! And while we're at it, ever wondered how this principle applies in real life? Think about a bike pump! When you push down the pump (reducing the volume of air inside), the pressure increases, making it easier to inflate your tire. It’s the same gas laws at play—making our lives a bit smoother one pump at a time!