How Does Intermolecular Potential Energy Behave in Ideal and Real Gases?

In summary, the kinetic model of an ideal gas assumes that there are no intermolecular forces and that the intermolecular potential energy is zero. For real gases, there may be intermolecular forces present, but for ideal gases, the kinetic energy of a given molecule is constant. The correct answer to the question is B, as the intermolecular potential energy is constant for ideal gases.
  • #1
sapphyrblud
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Homework Statement


In the kinetic model of an ideal gas, it is assumed that:
A. The forces between the gas and the container are zero
B. The intermolecular potential energy of the molecules of the gas is constant.
C. The kinetic energy of a given gas molecule is constant
D. The momentum of a given molecule of the gas is constant

Homework Equations

The Attempt at a Solution


I chose D, because collisions of ideal gases are perfectly elastic, but the answer was B. I wanted to know whether this answer means that for real gases, the intermolecular potential energy is not constant. [/B]
 
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  • #2
B is correct. Intermolecular potential energy is 0 for an ideal gas. The kinetic model for an ideal gas assumes that the molecules are point masses and that there are no intermolecular forces. If there were intermolecular forces one would have to take into account potential energy (as a function of intermolecular distances). For real gases there may or may not be intermolecular forces. For example, there are significant intermolecular forces between H2O molecules but not for He.

AM
 
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  • #3
D is not correct because molecules are constantly colliding and changing direction. Momentum is a vector quantity
 

Related to How Does Intermolecular Potential Energy Behave in Ideal and Real Gases?

1. What is the kinetic model of an ideal gas?

The kinetic model of an ideal gas is a theoretical model that describes the behavior of a gas at a microscopic level. It assumes that gas particles are in constant, random motion and do not interact with each other except during collisions.

2. What are the assumptions of the kinetic model of an ideal gas?

The assumptions of the kinetic model of an ideal gas include that gas particles have negligible volume, there are no intermolecular forces between particles, and collisions between particles are completely elastic.

3. How does temperature affect the kinetic model of an ideal gas?

According to the kinetic model of an ideal gas, temperature is directly proportional to the average kinetic energy of gas particles. As temperature increases, the particles move faster and collide more frequently, resulting in an increase in pressure.

4. What is the relationship between pressure, volume, and temperature in the kinetic model of an ideal gas?

According to the kinetic model of an ideal gas, pressure is directly proportional to the number of gas particles and their average kinetic energy. Volume is inversely proportional to pressure, and temperature is directly proportional to pressure.

5. How does the kinetic model of an ideal gas explain the gas laws?

The kinetic model of an ideal gas provides a theoretical basis for the gas laws, such as Boyle's law, Charles's law, and Gay-Lussac's law. These laws describe the relationships between pressure, volume, and temperature in a gas, based on the behavior of gas particles as described by the kinetic model.

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