Answer :
Ans: (2) The gas particles have no attractive forces between them.
The kinetic theory explains the behaviour of a hypothetical ideal gas. It explains pressure in terms of the collision of gas particles against the walls of the container which it occupies.
The kinetic theory of gases is based on three main postulates:
1) The collision between gas particles is elastic i.e. no energy is lost or gained
2) The gas particles are treated as point masses i.e. the volume occupied by the gas particles is negligible when compared to the volume of the container
3) There are no attractive or repulsive forces between particles.
The statement that describes the particles of an ideal gas, based on the kinetic molecular theory is [tex]\boxed{\left( {\text{2}} \right){\text{ The gas particles have no attractive forces between them}}}[/tex].
Further Explanation:
Kinetic theory of gases depicts gas as a large number of particles that are in continuous random motion. It explains the macroscopic properties of gases by taking into account their molecular composition and motion.
Postulates of kinetic theory of gases:
i) The gas molecules are very small and are located far apart from each other. Most of the volume occupied by the gas is an empty space.
ii). The molecules of the gas are in rapid random motion. These can move in all directions.
iii). The gas molecules undergo collisions with each other and with the walls of the container. The collisions between molecules and container walls are responsible for the pressure of the gas.
iv). There is no loss of kinetic energy when gas molecules collide so their collisions are known as perfectly elastic.
v). No interaction occurs between different molecules of gas during collisions.
(1) The motion of the gas particles is orderly and circular.
The molecules of a gas move randomly in all directions so their motion is not orderly and circular.
(2) The gas particles have no attractive forces between them.
The molecules of a gas move randomly in all directions so their motion is not orderly and circular.
(3) The gas particles are larger than the distances separating them.
The particles of gas are very small and are situated far away from each other. So the distance between the particles is larger than their size and not vice-versa.
(4) As the gas particles collide, the total energy of the system decreases.
The collisions of gas molecules are considered to be perfectly elastic. So the total energy of the system remains constant. It neither increases nor decreases.
Therefore option (2) describes the particles of an ideal gas on the basis of the kinetic molecular theory.
Learn more:
- What is the kinetic energy of electrons? https://brainly.com/question/5031462
- Which statement is true for Boyle’s law: https://brainly.com/question/1158880
Answer details:
Grade: High School
Subject: Chemistry
Chapter: Ideal gas equation
Keywords: collisions, gas, random motion, kinetic energy, perfectly elastic, interaction, container, kinetic theory of gases, volume, motion, orderly, circular, decreases.
