Exploring the Differences between Ideal Gas and Van Der Walls Models

In summary, ideal gases and Van Der Waals gases differ in their representation of real gases, with ideal gases being a theoretical concept and Van Der Waals gases taking into account intermolecular forces and particle size. The behavior and properties of these gases also differ, with ideal gases following the ideal gas law and Van Der Waals gases following the Van Der Waals equation. Gas can only behave as one type at a time, depending on conditions. Real-life applications of these gases include their use in gas laws and calculations, as well as in predicting the behavior of real gases in non-ideal conditions and studying phase transitions. These gases also relate to the kinetic molecular theory, with ideal gases following its assumptions and Van Der Waals gases accounting for
  • #1
CollectiveRocker
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Why does the Van Der Walls equation give a less value for pressure than the Ideal Gas equation does?
 
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  • #3
The main point is a VDW model gas has electrostatic interactions between particles. Thus, the particles are not flowing as free as in an ideal model gas. Therefore the pressure is smaller than the pressure predicted by VDW.
 

1. What is the difference between an ideal gas and a Van Der Waals gas?

An ideal gas is a theoretical concept that follows the gas laws perfectly and has no intermolecular forces between particles. A Van Der Waals gas, on the other hand, takes into account the intermolecular forces and the size of the gas particles, resulting in a more accurate representation of real gases.

2. How do the behavior and properties of an ideal gas differ from those of a Van Der Waals gas?

The behavior of an ideal gas can be described by the ideal gas law, while a Van Der Waals gas follows the Van Der Waals equation. The properties of an ideal gas, such as volume and pressure, are directly proportional to temperature, while properties of a Van Der Waals gas are affected by intermolecular forces.

3. Can a gas be both ideal and Van Der Waals at the same time?

No, a gas can either behave like an ideal gas or a Van Der Waals gas, depending on the conditions. At low pressures and high temperatures, gases tend to behave more like ideal gases, while at high pressures and low temperatures, they behave more like Van Der Waals gases.

4. What are some real-life applications of ideal and Van Der Waals gases?

Ideal gases are commonly used in gas laws and calculations, such as in the ideal gas law and the combined gas law. Van Der Waals gases are used in more complex scenarios, such as predicting the behavior of real gases in non-ideal conditions, and in the study of phase transitions.

5. How do ideal and Van Der Waals gases relate to the kinetic molecular theory?

Ideal gases follow the assumptions of the kinetic molecular theory, which states that gas particles are in constant, random motion and have negligible volume and intermolecular forces. Van Der Waals gases take into account the deviations from these assumptions and provide a more accurate description of real gas behavior.

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