Question

Collisions of the molecules in a sample of gas with the walls of the container are responsible for the gas’s observed .

Answer 1

A gas gas consist of the large number of minute particles, called the molecules.

These molecules are in a state of the constant rapid motion in all possible directions colliding in a random manner with one another and with the walls of the container.

The molecular collisions are perfectly elastic so that there is no net loss of the energy when the gas molecule collide with with one another or against the walls of the container. The kinetic energy may be transferred from one molecule to another molecule but it i not converted into any other form of the energy such as heat.

There are no attractive forces between the molecules or between the walls of the container and gas molecules. The molecules move completely independent of one another.

The pressure of the gas is due to bombardment  of the molecules on the walls of the container.

The kinetic energy (E_K) for an individual atom can be calculated by the following equation:

E_K = 1\2 m v²   

where, m is the mass and v is the velocity of the molecule.

The molecules possesses the average speed( V_avg), root mean speed (V_rms) and most probable (Vmp) velocity.

Molecular speed distribution of noble gases is shown below as :

The collision takes place among the gaseous molecules and between the container wall and gaseous molecule is responsible for a reaction to happen.