Why do gases exert pressure?

Answer:- The random motion of particles in a gas causes the pressure it exerts. Gases have weak intermolecular interactions, and the particles are in a constant state of random motion, colliding with the container’s walls. These encounters with the container’s walls put pressure on the gas.

The simple kinetic theory of gases can explain the pressure exerted by gases.

• Gases have high kinetic energy and a negligible force of attraction, allowing them to flow at a high rate in all directions.
• Because of the strong random mobility of the particles, they collide with one other and with the container’s walls.
• The pressure on the container walls is caused by the collisions of the gas particles with the container walls.

The formula PV=nRT can be used to compute the pressure of any gas.

where, P = The applied pressure on the gas.

V= The volume of the container 

n = The amount of gas is n.

R = The constant.

T = Temperature in Kelvin

The pressure exerted by the gas can be increased in a variety of ways, including:

• Raise the temperature.
• By increasing the gas supply
• By shrinking the container’s volume

Since gas particles have less intermolecular interaction, it exerts more pressure on the container wall than solid or liquid particles.