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

Expert Solution

The postulates of the Kinetic Molecular theory of gases are:

1. Gases are made of a large number of particles that behave like hard, spherical objects in a state of constant and random motion.

2. These particles move in a straight line until they collide with another particle or with the walls of the container.

3. These particles are much tinier than the distance between particles. Therefore, most of the volume in a gas is empty space.

4. There exists no force of attraction between two gas particles or between the particle and the walls of the container.

5. The collisions between two gas particles or the collisions of particles with the walls of the container are perfectly elastic. Energy of a gas particle is not lost when it collides with another particle or with the walls of the container.

6. The average kinetic energy of a collection of gas particles is dependent only on the temperature of the gas.

So, as the volume of the gas decreases, there are same number of molecules in the container and hence more number of collisions occur due to the decrease in the empty space between gas particles. Therefore the pressure of the gas increases. When the volume of gas increases, this space increases and there are fewer collisions on the walls of the container leading to a lower pressure.

Hence we can conclude that P is inversely proportional to V

queen_honey_blossom answered 2 years ago

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...

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

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...

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 the development of atomic theory from Dalton's Atomic Theory to the Modern Atomic Theory.

Explain the development of atomic theory from Dalton's Atomic Theory to the Modern Atomic Theory. Be sure to describe the fundamental particles of the atom throughout the development of the atom. Include at least the following scientists in your discussion; JJ Thomson, Robert Millikan, Ernest Rutherford, Niels Bohr, and Werner Heisenberg. Be sure to include how they completed their research as well.

Explain the functional relationship between volume changes, pressure changes, and gas flow into and out of...

Explain the functional relationship between volume changes, pressure changes, and gas flow into and out of the lung during pulmonary ventilation.

Think about the assumptions involved in the ideal gas law and kinetic molecular theory. For each...

Think about the assumptions involved in the ideal gas law and kinetic molecular theory. For each pair below determine which system is more likely to obey the ideal gas law and explain why you made your choice. A one liter container of Xe at 760 torr and 273 K or A one liter container of He at 760 torr and 273 K? A one liter container of He at 76.000 torr and 273 K or A one liter container of...

Give 5 manifestations of the kinetic molecular theory or of gas laws in your every day...

Give 5 manifestations of the kinetic molecular theory or of gas laws in your every day life. For example, why does the low tire pressure warning light in your car turn on when the temperature cools dramatically? (DON'T answer that question, it's just an example lol). Thanks!!! I'll give the best answer the points.

1. The average molecular velocity of gas molecules in Kinetic Theory is I have two balloons...

1. The average molecular velocity of gas molecules in Kinetic Theory is I have two balloons of the same kind. I fill both balloons to the same pressure and temperature, one with hydrogen and the other with Helium. The molecular mass of Hydrogen is 2g/mol and that of Helium is 4g/mol. From your understanding of the kinetic theory of gas: a. Consider the momentum transferred to balloon wall from molecular collisions. Is it higher for the Hydrogen balloon or the...

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