How is Ideal Gas Different from Real Gas?
The concept of gases has been a fundamental aspect of chemistry and physics for centuries. Gases are one of the four fundamental states of matter, along with solids, liquids, and plasmas. While the behavior of gases has been extensively studied, there is a significant difference between the ideal gas and the real gas. In this article, we will explore how ideal gas differs from real gas and understand the implications of these differences.
1. Assumptions of Ideal Gas
An ideal gas is a theoretical concept that assumes certain properties to simplify the understanding of gas behavior. The assumptions of an ideal gas are as follows:
a. Gas particles are point masses with no volume.
b. Gas particles do not interact with each other except during collisions.
c. Gas particles move in a straight line at constant speeds.
d. The collisions between gas particles are perfectly elastic.
These assumptions allow us to use the ideal gas law, which is a mathematical relationship that describes the behavior of ideal gases. The ideal gas law is given by the equation PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.
2. Real Gas Behavior
Real gases, on the other hand, do not perfectly adhere to the assumptions of an ideal gas. Real gases have the following characteristics:
a. Gas particles have finite volume.
b. Gas particles interact with each other through attractive and repulsive forces.
c. Gas particles do not move in a straight line at constant speeds.
d. The collisions between gas particles are not perfectly elastic.
These deviations from the ideal gas behavior lead to deviations from the ideal gas law. As a result, real gases exhibit phenomena such as condensation, boiling, and the van der Waals forces.
3. Deviations from Ideal Gas Behavior
The deviations from ideal gas behavior can be quantified using the van der Waals equation, which is a modification of the ideal gas law. The van der Waals equation takes into account the finite volume of gas particles and the attractive and repulsive forces between them. The equation is given by:
(P + a(n/V)^2)(V – nb) = nRT
where a and b are constants specific to each gas.
4. Conclusion
In conclusion, the ideal gas and real gas differ in several aspects. The ideal gas is a theoretical concept that assumes certain properties to simplify the understanding of gas behavior, while the real gas takes into account the finite volume of gas particles and the attractive and repulsive forces between them. The deviations from ideal gas behavior are quantified using the van der Waals equation. Understanding these differences is crucial for accurately describing and predicting the behavior of gases in various applications.
