Kinetic Theory | MCQs

Explanation

When a gas is heated in a container of fixed volume, the molecules of the gas:

• Move faster (their kinetic energy increases, causing them to move more rapidly)
• Collide more frequently with the container walls (resulting in increased pressure)
• Do not expand (the container volume is fixed)
• Do not move further apart (the density of the gas remains the same, as the volume

Explanation

According to the kinetic molecular theory, the pressure exerted by a gas is caused by the bombardment of gas molecules on the walls of the container.

The gas molecules are in constant motion, colliding with each other and the container walls, resulting in a force exerted on the walls.

This force is what we experience as pressure.

Explanation

In a gas, the particles are:

• Widely spread out, with no fixed position or arrangement
• Not in a regular pattern, with no repeating structure or order
• Separated by large empty spaces, with no close packing or cohesion