Final answer:
The correct concept from the kinetic-molecular theory is that gas particles travel in a random, zigzag motion. This matches the theory's assumptions about the motion and interactions of gas particles, which include their negligible size, constant motion, elastic collisions, lack of intermolecular forces, and a kinetic energy that is dependent on temperature.
Step-by-step explanation:
The concept of the kinetic-molecular theory that is accurate among the options provided is: Particles of a gas travel in a random, zigzag motion. This concept aligns with the fundamental assumptions of the kinetic-molecular theory, which describe the behavior of ideal gases. According to the theory:
- Gases consist of tiny spherical particles that are far apart from each other relative to their size, meaning that the volume of these particles is negligible compared to the volume of the container they occupy.
- Gas particles are in constant rapid motion in random directions, and this motion is ceaseless because of the kinetic energy the particles possess.
- Collisions between gas particles are elastic, which means there is no net loss of kinetic energy during these collisions.
- There are no forces of attraction or repulsion between gas particles in ideal gas conditions, so each particle moves independently of others.
- The average kinetic energy of gas particles is directly proportional to the temperature of the gas, with higher temperatures resulting in greater speeds and kinetic energy.
The other options presented in the question either do not align with or contradict the assumptions of the kinetic-molecular theory. The notion that the volume of gas particles can be relatively large or that there is a strong attraction between gas particles are incorrect within the context of this theory.