maximum deviation from ideal gas is expected from

In the field of thermodynamics, the concept of an ideal gas serves as a fundamental model to understand and analyze the behavior of gases under various conditions.

However, it is essential to recognize that real gases deviate from this idealized behavior to some extent.

In this article, we will delve into the factors that contribute to the maximum deviation from the ideal gas law, shedding light on the complexities of real gas behavior.

Short answer:

Topic: maximum deviation from ideal gas is expected from

Answer: Real gases deviate the most from ideal gas behavior due to factors like intermolecular forces, particle volume, non-negligible pressure, and extreme temperature and pressure conditions.

Understanding the Ideal Gas Law

To comprehend the deviation of real gases from the ideal gas law, let's first revisit the fundamental principles of the ideal gas model.

The ideal gas law, represented by the equation $PV = nRT$, relates the pressure (P), volume (V), temperature (T), and the amount of gas in moles (n) in a closed system. It assumes that gas particles are point masses with no volume, exhibit no intermolecular forces, and undergo elastic collisions.

Deviations from the Ideal Gas Law

1. Intermolecular Forces:

One of the most significant factors contributing to the deviation of real gases from ideality is the presence of intermolecular forces. Unlike ideal gases, real gases experience attractive and repulsive forces between their particles. 

These intermolecular forces become more pronounced as the gas molecules come closer together or at lower temperatures. Consequently, the measured pressure and volume differ from the ideal gas predictions.

2. Particle Volume:

In contrast to the assumption of point-like particles in the ideal gas law, real gas molecules occupy a finite volume.

At high pressures and low temperatures, the volume occupied by gas molecules becomes significant compared to the overall volume of the system.

As a result, the available space for particle movement and collision decreases, leading to deviations from ideal gas behavior.

3. Non-Negligible Pressure:

The ideal gas law assumes that the size of the gas molecules is negligible compared to the distance between them. However, at high pressures, the volume occupied by the gas molecules becomes significant, leading to a compressed state where the particles are closer together.

This crowding effect increases the frequency of intermolecular collisions, causing the pressure to deviate from the ideal gas predictions.

4. Van der Waals Equation:

To account for the deviations observed in real gases, Dutch physicist Johannes van der Waals introduced a modified equation of state.

The Van der Waals equation incorporates corrections for intermolecular forces and particle volume, expressed as $(P + a(n/V)^2)$$(V - nb) = nRT$. The parameters 'a' and 'b' adjust the ideal gas parameters to account for attractive forces and particle volume, respectively.

5. Temperature and Pressure Extremes:

At extremely low temperatures or high pressures, the deviations from the ideal gas law become more prominent.

When a gas is cooled to near its boiling point or subjected to high pressure, the intermolecular forces dominate, causing the gas to exhibit behavior that significantly diverges from the idealized model.

Conclusion

While the ideal gas law provides a useful framework for understanding gas behavior under normal conditions, it is crucial to recognize that real gases deviate from this idealized model.

Factors such as intermolecular forces, particle volume, non-negligible pressure, and extreme temperature and pressure conditions significantly impact the behavior of real gases.

The introduction of modified equations of state, like the Van der Waals equation, helps to account for these deviations and improve the accuracy of gas calculations.

By considering these factors, scientists and engineers can better predict and analyze the behavior of real gases in a wide range of practical applications.