Let's answer this question by understanding the behavior of gases and ideal gases.
Looking at each of the following statements:
- The average kinetic energy of the gas particles is directly proportional to the temperature in Kelvin.
This statement is correct. According to the kinetic theory of gases, the average kinetic energy of gas particles is directly proportional to the temperature in Kelvin. As the temperature increases, the kinetic energy of the gas particles also increases, leading to higher speeds and more energetic collisions.
- Gas particle collisions are perfectly elastic; they conserve momentum when they bounce off something.
This statement is correct. In an ideal gas, particles are considered to have perfectly elastic collisions. This means that no kinetic energy is lost when gas particles collide with each other or with the walls of their container. Instead, momentum is conserved, which leads to a transfer of energy between particles without any net loss.
- The attraction forces between gas particles are so small as to be negligible.
This statement is correct. In ideal gases, the particles are assumed to have negligible attractive forces between them. The intermolecular forces in ideal gases are so weak compared to the kinetic energy of the particles that they can be ignored. This assumption holds well for most real gases at low to moderate pressures and high temperatures.
- There is a vast distance between gas particles such that the volume occupied by the gas particles themselves is negligible.
This statement is correct. Gas particles are in constant, random motion and have significant empty spaces between them. The volume occupied by the gas particles themselves is minimal compared to the overall volume of the gas. The majority of the gas volume is composed of space, which is why gases can be easily compressed.
- A mixture of only gas particles can be either homogeneous or heterogeneous.
This statement is false. Mixtures of only gas particles are always homogeneous. In a gas mixture, different gas particles are uniformly distributed and evenly mixed throughout the container. There are no concentration gradients or distinct regions of different gases within the mixture, as found in heterogeneous mixtures. In contrast, mixtures of solids or liquids can be either homogeneous or heterogeneous, depending on how the components are distributed.
Answer: The false statement is "Mixtures of only gas particles can be either homogeneous or heterogeneous".