Final answer:
The kinetic-molecular theory of gases is based on five basic assumptions: gases consist of tiny particles far apart from each other, gas particles are in constant motion, collisions are elastic, no forces of attraction or repulsion between particles, and average kinetic energy depends on temperature.
Step-by-step explanation:
The kinetic-molecular theory of gases is based on five basic assumptions:
- Gases consist of very large numbers of tiny spherical particles that are far apart from one another compared to their size. The volume of a gas is mainly composed of empty space between the particles.
- Gas particles are in constant rapid motion in random directions. This motion gives them a relatively large amount of kinetic energy.
- Collisions between gas particles and between particles and the container walls are elastic collisions, meaning there is no overall loss of kinetic energy during collisions.
- There are no forces of attraction or repulsion between gas particles. The particles of an ideal gas have no such attractive forces and their motion is independent of each other.
- The average kinetic energy of gas particles is dependent upon the temperature of the gas. As the temperature increases, the speeds of the particles also increase, leading to an increase in kinetic energy.