What are two assumptions made by ideal gas laws that are violated by real gases?

The ideal gas law is a simplified model that describes the behavior of gases under certain conditions. However, real gases often deviate from this model due to specific assumptions. Here are two key assumptions that are typically violated:

1. Negligible Volume of Gas Particles

The ideal gas law assumes that the volume occupied by gas particles themselves is insignificant compared to the volume of the container. In reality, gas molecules do have a finite size, and at high pressures, their volume becomes significant, leading to deviations from ideal behavior.

2. No Intermolecular Forces

Another assumption is that there are no attractive or repulsive forces between gas molecules. In real gases, especially at low temperatures or high pressures, these intermolecular forces can affect the behavior of the gas, causing it to deviate from the predictions of the ideal gas law.

Summary

• Real gases have a measurable volume.
• Intermolecular forces impact gas behavior.

Understanding these differences helps in applying the ideal gas law more accurately in real-world situations.