What is true about the collisions between gas molecules, according to kinetic-molecular theory?

According to the kinetic-molecular theory, one of the foundational principles is that collisions between gas molecules are perfectly elastic. This means that during these collisions, both kinetic energy and momentum are conserved. In perfectly elastic collisions, the total kinetic energy of the system before and after the collision remains the same, which is a key aspect of how gas molecules behave.

In a gaseous state, molecules are in constant random motion, colliding with each other and the walls of their container. These collisions are essential for understanding the properties of gases, such as pressure and temperature. Since there is no energy loss during these interactions, the concept of perfectly elastic collisions helps explain why gases can expand and occupy volume uniformly.

The other options do not align with the kinetic-molecular theory. For instance, perfectly inelastic collisions suggest that kinetic energy is not conserved and some energy is transformed into other forms like heat, which contradicts the nature of gas molecule interactions as described by the theory. Similarly, implying that collisions involve energy loss also contradicts the perfect elasticity of gas collisions, as any loss would indicate a non-elastic interaction. Lastly, while collisions do contribute to pressure, the term "result in increased pressure" could suggest a dynamic state rather than a foundational principle of molecular