Which of the following best describes the behavior of real gases compared to ideal gases?

The behavior of real gases compared to ideal gases is best described by the idea that real gases deviate from ideal gas equations under certain conditions. Ideal gases are modeled based on assumptions that simplify their behavior, such as having no intermolecular forces and occupying no volume. However, real gases do not completely adhere to these assumptions due to their molecular structure and interactions.

At high pressures and low temperatures, real gases tend to show significant deviations from ideal behavior. In these conditions, the volume of gas molecules becomes significant relative to the space they occupy, and intermolecular forces can cause attractions or repulsions that are not accounted for in the ideal gas law. This leads to differences in behavior, such as lower pressures than predicted by the ideal gas law or reduced volumes.

Understanding these deviations is crucial for accurately predicting the behavior of gases in practical applications, such as chemical reactions under varying conditions. This helps chemists and engineers make better predictions and adjustments in real-world scenarios.