Ideales Gas vs. Reales Gas

Attribute	Ideales Gas	Reales Gas
Particle Volume	Negligible	Considerable
Particle Interactions	No	Yes
Pressure-Volume Relationship	Follows Ideal Gas Law	Deviation from Ideal Gas Law
Temperature-Volume Relationship	Follows Ideal Gas Law	Deviation from Ideal Gas Law
Boyle's Law	Follows	Deviation

Introduction

Gas is a state of matter that is commonly found in our everyday lives. When studying the behavior of gases, scientists often use ideal gas and real gas models to simplify their analysis. While ideal gases follow the ideal gas law perfectly under all conditions, real gases deviate from this law due to their interactions with each other. In this article, we will compare the attributes of ideal gas and real gas to understand their differences and similarities.

Definition

Ideal gas is a theoretical concept that assumes gas particles have no volume and do not interact with each other. This means that ideal gases obey the ideal gas law, which states that the pressure, volume, and temperature of a gas are related by the equation PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature. On the other hand, real gases have volume and interact with each other through intermolecular forces. Real gases do not always follow the ideal gas law due to these interactions.

Behavior

Ideal gases exhibit behavior that is predictable and easy to analyze. They expand to fill their container completely, and their pressure, volume, and temperature are directly proportional to each other according to the ideal gas law. Ideal gases also do not condense into liquids or solids under normal conditions. Real gases, on the other hand, do not always behave as predicted by the ideal gas law. They may deviate from the law at high pressures or low temperatures due to the interactions between gas particles. Real gases can also condense into liquids or solids under certain conditions.

Intermolecular Forces

One of the key differences between ideal gas and real gas is the presence of intermolecular forces. Ideal gases do not experience any intermolecular forces because their particles are assumed to have no volume and do not interact with each other. This simplifies the analysis of ideal gases and allows scientists to make accurate predictions based on the ideal gas law. Real gases, on the other hand, experience intermolecular forces such as van der Waals forces, dipole-dipole interactions, and hydrogen bonding. These forces cause real gases to deviate from the ideal gas law under certain conditions.

Volume

Another difference between ideal gas and real gas is their volume. Ideal gases are assumed to have zero volume, meaning their particles do not take up any space. This assumption allows scientists to simplify calculations and make accurate predictions based on the ideal gas law. Real gases, however, have volume and their particles occupy space. This volume must be taken into account when analyzing the behavior of real gases, especially at high pressures and low temperatures where the volume of gas particles becomes significant.

Pressure

Pressure is another attribute that distinguishes ideal gas from real gas. Ideal gases follow the ideal gas law perfectly, meaning their pressure is directly proportional to their temperature and volume. This relationship allows scientists to make accurate predictions about the behavior of ideal gases under various conditions. Real gases, on the other hand, may deviate from the ideal gas law at high pressures or low temperatures. The interactions between gas particles can cause the pressure of real gases to differ from what is predicted by the ideal gas law.

Temperature

Temperature plays a crucial role in the behavior of both ideal gas and real gas. Ideal gases follow the ideal gas law, which states that the temperature of a gas is directly proportional to its pressure and volume. This relationship allows scientists to make accurate predictions about the behavior of ideal gases at different temperatures. Real gases, however, may deviate from the ideal gas law at low temperatures. The interactions between gas particles become more significant at low temperatures, causing real gases to behave differently than ideal gases.

Conclusion

In conclusion, ideal gas and real gas are two models used to study the behavior of gases. Ideal gases follow the ideal gas law perfectly and do not interact with each other, while real gases deviate from the ideal gas law due to their interactions. Understanding the differences between ideal gas and real gas is essential for scientists to make accurate predictions about the behavior of gases under different conditions.