Differentiate between Real and Ideal gas? Please explain extensively and give examples.
A gas can be classified as either a real gas or an ideal gas based on its behavior under certain conditions. The main difference between the two lies in the assumptions made about the gas particles and the interactions between them.
An ideal gas is a theoretical concept that assumes certain conditions to simplify calculations and make them more manageable. The assumptions for an ideal gas include:
1. The gas particles have negligible volume: In an ideal gas, the volume occupied by the gas particles themselves is considered to be insignificant compared to the total volume of the gas. This assumption allows for easier calculations and simplifies the ideal gas law equation.
2. The gas particles do not interact with each other: In an ideal gas, the gas particles are assumed to have no interactions or attractions between them. This means that there are no intermolecular forces present, such as van der Waals forces or hydrogen bonding. As a result, the ideal gas particles move independently and do not influence each other's behavior.
3. The gas particles undergo elastic collisions: In an ideal gas, the collisions between gas particles and the walls of the container are assumed to be perfectly elastic. This means that there is no loss of kinetic energy during the collisions, and the total energy of the system remains constant.
On the other hand, a real gas takes into account the deviations from these ideal conditions. Real gases behave differently from ideal gases under certain conditions, such as high pressures or low temperatures. The behavior of real gases is influenced by factors such as the volume occupied by the gas particles, intermolecular forces, and the compressibility of the gas.
Examples of real gases include gases such as nitrogen, oxygen, and carbon dioxide. These gases deviate from ideal gas behavior at high pressures or low temperatures. For instance, at high pressures, the volume occupied by the gas particles becomes significant, and the intermolecular forces between the particles start to play a role. This leads to deviations from the ideal gas law and requires more complex equations, such as the van der Waals equation, to accurately describe the behavior of the gas.
In summary, the main difference between real and ideal gases lies in the assumptions made about the gas particles and their interactions. Ideal gases are theoretical concepts that simplify calculations by assuming negligible volume, no intermolecular forces, and elastic collisions. Real gases, on the other hand, take into account the deviations from these ideal conditions and exhibit different behavior under certain conditions.