Question

Which of the following statements about kinetic-molecular theory of gases is false?

A) The molecules of a gas are separated by large distances on the average compared to the size of the molecules.
B) The molecules are in constant random motion and undergo elastic collisions.
C) For two different gases, such as oxygen and hydrogen, at the same temperature, the average speeds of the molecules in the two gases are the same.
D) The average translational kinetic energy of the molecules of a gas is proportional to the Kelvin temperature.

Answer 1

The statement that the average translational kinetic energy of the molecules of a gas is proportional to the Kelvin temperature is true, in accordance with the kinetic-molecular theory of gases, which says that rising temperature causes an increase in the speed and kinetic energy of gas molecules.

Step-by-step explanation:

The statement in question, which pertains to the kinetic-molecular theory of gases, is actually true. The kinetic-molecular theory provides a series of postulates that explain the behavior of gases, and one of those postulates is that the average translational kinetic energy of the molecules of a gas is directly proportional to the gas's Kelvin temperature. This concept is fundamental in understanding how gases behave and how their temperature relates to the motion of their molecules. As the temperature increases, the speed of the particles also increases, leading to higher kinetic energy.

According to the theory, as the temperature of a gas rises, the molecules' energy - their ability to move and therefore to translate from one place to another - also increases. It means that at higher temperatures, gas molecules will typically move faster and have greater kinetic energy. This relationship between temperature and kinetic energy is not only a core concept in ideal gas law but is also an essential component of thermodynamics.