The kinetic theory of gases describes the behavior of gas molecules based on their motion and interactions. According to this theory, gas molecules are in constant random motion, colliding with each other and the walls of their container. Between two successive collisions, a gas molecule travels in a straight line path.

Explanation:
1. Random Motion of Gas Molecules:
- Gas molecules are in constant motion, moving in all directions at high speeds.
- This motion is random, meaning that the molecules move in various directions with no preferred pattern.
- The random motion of gas molecules is a result of their high kinetic energy.

2. Collisions Between Gas Molecules:
- Gas molecules collide with each other and the walls of their container.
- These collisions are elastic, meaning that no kinetic energy is lost during the collision.
- When two gas molecules collide, they change their direction of motion due to the forces exerted on each other.

3. Straight Line Path Between Collisions:
- Between two successive collisions, a gas molecule travels in a straight line path.
- This is because there are no external forces acting on the molecule to change its direction of motion.
- The gas molecule moves with a constant velocity in a straight line until it collides with another molecule or the container wall.
- After the collision, the molecule changes its direction of motion and continues in another straight line until the next collision occurs.

4. Assumptions of the Kinetic Theory:
- The kinetic theory of gases is based on several assumptions:
- Gas molecules are considered to be point masses with no volume.
- The collisions between gas molecules and the container walls are perfectly elastic.
- There are no attractive or repulsive forces between gas molecules.
- The average kinetic energy of gas molecules is directly proportional to the temperature of the gas.

In conclusion, according to the kinetic theory of gases, gas molecules travel in a straight line path between two successive collisions. This straight line motion is a result of the random and high-speed motion of gas molecules, which only changes when a collision occurs.

According to kinetic theory, the gas molecules are in a state of constant rapid motion in all possible directions colliding in a random manner with one another and with the walls of the container and between two successive collisions, molecules travel in a straight line path but show haphazard motion due to collisions.