Why the ideal gas law fails in the real world
In short: The ideal gas law assumes particles are dimensionless points that never interact. This video explores why these assumptions fail and how scientists corrected the math to account for molecular volume and intermolecular attraction.
While the ideal gas law is a fundamental tool in chemistry, it ignores two critical realities: atoms and molecules occupy physical space, and they exert attractive forces on one another. To account for these factors, the equation requires specific corrections to both volume and pressure.
In the late 19th century, Dutch scientist Johannes van der Waals developed the necessary correction factors to transform the ideal gas law into a model that accurately describes real gases. His work was so significant that he was eventually awarded a Nobel Prize.
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Sources
- Summary by Intellect · source: Real Gases: Crash Course Chemistry #14
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