Imagine the movement of a single gas molecule inside a container. explain the particle’s motions in terms of kinetic-molecular theory.

According to the kinetic molecular theory, single gas molecule inside a container inside a container is engaged in a random motion and collides frequently with the walls of the container.

The kinetic theory states that the molecules of gases are in constant random motion and collide frequently with each other as well as with the walls of the container.

This means that the single gas molecule will constantly bump against the containers walls.

The force per unit area with which the single gas molecule collides with the walls of the container is the pressure of the gas.

The kinetic energy of this single gas molecule depends on the temperature of the gas. The higher the temperature of the gas, the higher the frequency with which this single gas molecule bumps against the walls of the container.

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Explanation:

As per the kinetic-molecular theory the particles (atoms or molecules) of gas occupy a negligible space and act independent of each other, i.e., in ideal conditions, there are not forces of attractions or repulsion among the particles.

Two facts characterize the motion of gas particles:

So, refering to a single gas molecule inside a container, the particle's motion is rectilinear uniform (since no forces are acting on it) until it collides with the walls of the container, from which it will bounce in a random direction, with the same speed (since the kinetic energy is conserved), traveling in straight line until a new collision happens, from which the particle will behave in the same way.

that's what i got you can count the number of atoms