Incorrect Postulate Of Kinetic Molecular Theory Of Gases

The kinetic molecular theory of gases is a set of postulates that describe the behavior of gases under a variety of conditions. This theory was developed from the work of Daniel Bernoulli, who proposed that the pressure of a gas is a result of the collision of molecules of the gas with the walls of a container. While this theory has been accepted as an accurate description of gas behavior, there are some incorrect postulates that have been proposed over the years.

Postulate One: All Gases Are Composed of Identical Molecules

The first incorrect postulate of the kinetic molecular theory of gases is that all gases are composed of identical molecules. This postulate implies that all gases behave in the same way and that their behavior is invariant regardless of their composition. This is not true, as different gases can have different molecular structures and thus behave differently. For example, a gas composed of nitrogen and oxygen molecules will behave differently from one composed of carbon dioxide molecules.

Postulate Two: Gases Are Composed of Point Masses

Another incorrect postulate of the kinetic molecular theory of gases is that all gases are composed of point masses. This postulate implies that all molecules of a gas are perfectly spherical and of uniform size. This is not the case, as molecules of different gases can have different shapes and sizes. Additionally, molecules of a single gas can vary in size and shape, which can affect their behavior.

Postulate Three: Gases Have No Intermolecular Forces

The third incorrect postulate of the kinetic molecular theory of gases is that all gases have no intermolecular forces. This postulate implies that molecules of different gases do not interact with each other, even when they come into contact. This is not true, as molecules of different gases can interact with each other through various forces, such as van der Waals forces and hydrogen bonding.

Postulate Four: All Gases Have the Same Temperature

The fourth incorrect postulate of the kinetic molecular theory of gases is that all gases have the same temperature. This postulate implies that the temperature of a gas is constant regardless of its composition or the number of molecules it contains. This is not the case, as different gases can have different temperatures depending on their composition and the number of molecules they contain.

Postulate Five: Gases Are Incompressible

The fifth incorrect postulate of the kinetic molecular theory of gases is that all gases are incompressible. This postulate implies that the volume of a gas is constant regardless of the pressure that is applied to it. This is not true, as the volume of a gas can vary depending on the pressure that is applied to it.

Postulate Six: Gases Are Perfectly Elastic

The sixth incorrect postulate of the kinetic molecular theory of gases is that all gases are perfectly elastic. This postulate implies that gases are not affected by changes in pressure or temperature, and that they can be compressed and expanded without any energy loss. This is not the case, as gases can be affected by changes in pressure and temperature, and they can lose energy when they are compressed or expanded.

Conclusion

In conclusion, the kinetic molecular theory of gases is a useful tool for understanding the behavior of gases under different conditions. However, there are some incorrect postulates that have been proposed over the years that are not accurate descriptions of gas behavior. These postulates include that all gases are composed of identical molecules, that all gases are composed of point masses, that all gases have no intermolecular forces, that all gases have the same temperature, that all gases are incompressible, and that all gases are perfectly elastic. It is important to understand these incorrect postulates in order to correctly interpret the behavior of gases.