- #1
CollectiveRocker
- 137
- 0
Why does the Van Der Walls equation give a less value for pressure than the Ideal Gas equation does?
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.
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.
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.
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.
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.