Explain the kinetic molecular theory and it's relationship with gases.

Expert Solution

Basic Assumptions of the Kinetic Molecular Theory :

By the late 19th century, scientists had begun accepting the atomic theory of matter started relating it to individual molecules. The Kinetic Molecular Theory of Gases comes from observations that scientists made about gases to explain their macroscopic properties. The following are the basic assumptions of the Kinetic Molecular

The volume occupied by the individual particles of a gas is negligible compared to the volume of the gas itself.
The particles of an ideal gas exert no attractive forces on each other or on their surroundings.
Gas particles are in a constant state of random motion and move in straight lines until they collide with another body.
The collisions exhibited by gas particles are completely elastic; when two molecules collide, total kinetic energy is conserved.
The average kinetic energy of gas molecules is directly proportional to absolute temperature only; this implies that all molecular motion ceases if the temperature is reduced to absolute zero.

queen_honey_blossom answered 2 years ago

Kinetic theory of gases

Molar volume is the volume occupied by 1 mol of any (ideal) gas at standard temperature and pressure (STP: 1 atmospheric pressure, 0 °C). Show that it is 22.4 litres.

To be able to predict and calculate properties of real gases. Kinetic molecular theory makes certain...

To be able to predict and calculate properties of real gases. Kinetic molecular theory makes certain assumptions about gases that are, in fact, not true for real gases. Therefore, the measured properties of a gas are often slightly different from the values predicted by the ideal gas law. The van der Waals equation is a more exact way of calculating properties of real gases. The formula includes two constants, a and b, that are unique for each gas. The van...

Use molecular kinetic theory of gas to explain the pressure-volume relationship from an atomic perspective.

Explain how the kinetic theory of gases can be applied to measure effusion rates?

A- Use Kinetic Molecular Theory to conceptually illustrate Charles’s law – the relationship between volume and...

A- Use Kinetic Molecular Theory to conceptually illustrate Charles’s law – the relationship between volume and temperature in an ideal gas is directly proportional. (in Detail please not just definition) B. Use Kinetic Molecular Theory to explain the constants a and b in the van der Waals equation – why are these corrections necessary for gases which do not behave ideally?( in detail please) c- Discuss the concept of Kinetic Molecular Theory, explaining what the theory is. Explain what factors...

Apply the Kinetic Theory of gases to explain Boyle's law, Charles' law and Dalton's law ?

Derive/explain how thermal conductivity can be explained in terms of the kinetic theory of gases.

use the kinetic molecular theory ( matter = particles ) to explain the differences between solid...

use the kinetic molecular theory ( matter = particles ) to explain the differences between solid vs liquid vs gas phase. And describe how particles are behaving during a phase change

Explain Boyle's Law in terms of the kinetic molecular theory. Decreasing the volume means that there...

Explain Boyle's Law in terms of the kinetic molecular theory. Decreasing the volume means that there are less gas molecules in the container, which increases pressure. Decreasing the volume means that at any one instant less molecules will collide with the walls of the container, which increases pressure. Decreasing the volume means that at any one instant more molecules will collide with the walls of the container, which increases pressure. Decreasing the volume means that there are more gas molecules...

One of the assumptions of the kinetic molecular theory is that there are no intermolecular forces...

One of the assumptions of the kinetic molecular theory is that there are no intermolecular forces (attractive or repulsive) between gas particles (atoms or molecules). How would the presence of intermolecular forces affect the ideal gas equation (PV = nRT)? Again, in your response, please use terms that a high school senior who hasn’t taken AP chemistry might use.

Question