According to the kinetic-molecular theory, the collision between two ideal gas particles is a result of

neither attraction nor repulsion.

repulsion from the wall of the container.

repulsion from other gas particles.

attraction between the two particles.

Question

Arjun Durham

Chemistry

17 November, 11:16

According to the kinetic-molecular theory, the collision between two ideal gas particles is a result of

neither attraction nor repulsion.

repulsion from the wall of the container.

repulsion from other gas particles.

attraction between the two particles.

+4

Answers (2)

Know the Answer?

Glenn Knapp · Answer 1

It is a result of neither attraction nor repulsion. They interact freely without any kinetic or chemical reaction.

Maverick Raymond · Answer 2

The correct answer is neither attraction nor repulsion.

Kinetic Molecular Theory explains that gas particles are in constant motion and exhibit perfectly elastic collisions. The motion of gas particles is random, meaning that there are no attractive forces on each other or on their surroundings. When two particles collide, the total kinetic energy is conserved.

According to the kinetic-molecular theory, the collision between two ideal gas particles is a result ofneither attraction nor repulsion.repulsion from the wall of the container.repulsion from other gas particles.attraction between the two particles.

According to the kinetic-molecular theory, the collision between two ideal gas particles is a result of

neither attraction nor repulsion.

repulsion from the wall of the container.

repulsion from other gas particles.

attraction between the two particles.