Gases exert pressure primarily due to the force exerted by their moving particles on the walls of a container.
In the gaseous state, particles are in constant, random motion. As these particles move around, they frequently collide with each other and, crucially, with the inner surfaces of the container holding the gas.
According to the provided reference: "In gaseous state, the particles move randomly. So, sometimes they hit each other and the walls of the container. The pressure exerted by the gas is because of the force exerted by the gas particles on the walls of the container."
Here's a breakdown of the process:
- Random Motion: Gas particles move chaotically in all directions.
- Collisions: They collide with each other and the boundaries of their container.
- Force on Walls: Each time a gas particle collides with a wall, it exerts a tiny force on that wall.
- Pressure: Pressure is defined as the force exerted per unit area. The collective effect of countless such collisions occurring rapidly over the entire surface area of the container walls results in a measurable pressure.
The magnitude of this pressure depends on several factors, including:
- Number of Particles: More particles mean more frequent collisions.
- Speed of Particles: Faster particles collide more forcefully and more often (related to temperature).
- Volume of Container: In a smaller volume, particles hit the walls more frequently.
Essentially, gas pressure is a macroscopic manifestation of the microscopic forces generated by individual particle collisions with a surface.
