Question

Question:
Kinetic theory of gases correlates the macroscopic properties of gases to microscopic properties of
gas molecules, according to this theory, a given amount of gas is a collection of large number of
molecules that are in incessant random motion and obey Newton's law of motion. The molecules do
not exert force of attraction or repulsion.
(i) What is an ideal gas?
(ii) Is the consequence of kinetic energy of atoms and molecules of gas?
(iii) What is the cause of pressure exerted by the gas?
(iv) What does the concept of kinetic theory of gas imply in day to day life?​

Answer 1

Answer:

Kinetic Molecular Theory states that gas particles are in constant motion and exhibit perfectly elastic collisions.

Kinetic Molecular Theory can be used to explain both Charles’ and Boyle’s Laws.

The average kinetic energy of a collection of gas particles is directly proportional to absolute temperature only.

Terms

macroscopic properties that can be visualized or measured by the naked eye; examples include pressure, temperature, and volume

ideal gasa hypothetical gas whose molecules exhibit no interaction and undergo elastic collision with each other and the walls of the container