Kinetic theory of gases core idea:\nAccording to the kinetic theory, which statement is correct?

Introduction / Context:
The kinetic theory of gases provides a microscopic explanation of macroscopic gas properties, relating temperature and pressure to molecular motion and collisions.

Given Data / Assumptions:

• Ideal gas model: point particles, elastic collisions, negligible intermolecular forces except during collisions.
• Thermal energy is entirely kinetic in this model.

Concept / Approach:
In kinetic theory, absolute temperature T is proportional to the average translational kinetic energy of gas molecules. Collisions are perfectly elastic (no net energy loss), and the volume of molecules is negligible relative to the container volume.

Step-by-Step Reasoning:

Verification / Alternative check:
Gas temperature rises when average molecular speed increases; pressure at constant volume rises accordingly, consistent with kinetic interpretations.

Why Other Options Are Wrong:

• Energy loss in collisions or inelastic ideal-gas collisions contradicts the model.
• Appreciable molecular volume violates the point-particle assumption of ideal gases.
• “None of these” is invalid because option (c) is correct.

Common Pitfalls:
Extending ideal behavior to high pressures/low temperatures where real-gas effects and finite molecular size matter.

Final Answer:
Absolute temperature measures the average kinetic energy of molecules