Which statement is false? The average kinetic energies of molecules from samples of different "ideal" gases are the same at the same tempera The molecules of an ideal gas are relatively far apart. All molecules of an ideal gas have the same kinetic energy at constant temperature. Molecules of a gas undergo many collisions with each other and the container walls. Mof greater mass have a lower average speed than those of less mass at the same temperature.

The false statement is: **"All molecules of an ideal gas have the same kinetic energy at constant temperature."** **Explanation:** - **Average Kinetic Energy:** While the *average* kinetic energy of molecules in different ideal gases is the same at the same temperature, individual molecules within a single gas can have varying kinetic energies. This variation is described by the Maxwell-Boltzmann distribution, which shows that molecules have a range of speeds and, consequently, kinetic energies at any given temperature. - **Other Statements:** - **Average Kinetic Energies:** True. Different ideal gases at the same temperature have the same average kinetic energy. - **Molecular Distance:** True. Ideal gas molecules are considered to be far apart relative to their size. - **Collisions:** True. Molecules in a gas continuously collide with each other and the container walls. - **Mass and Speed Relationship:** True. Heavier molecules move slower on average than lighter ones at the same temperature. In summary, while the *average* kinetic energy is consistent, individual molecules do not all possess the same kinetic energy, making the third statement false. **Answer:** The statement that all molecules have identical kinetic energy at a given temperature is false.