Ch.10 - Gases

Brown - Chemistry: The Central Science 14th Edition

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Brown 14th Edition

Ch.10 - Gases

Problema 89

Capitolo 10, Problema 89

(b) List two reasons why the gases deviate from ideal behavior.

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1. Real gases deviate from ideal behavior because the ideal gas law assumes that gas particles are point particles, meaning they occupy no volume. However, in reality, gas particles do have a finite volume. When the pressure of a gas is very high, or the volume is very low, the volume of the gas particles becomes significant compared to the total volume in which the gas is contained. This causes the gas to deviate from ideal behavior.

2. The ideal gas law also assumes that there are no intermolecular attractions or repulsions between gas particles. But in reality, gas particles do experience intermolecular forces. When a gas is at a low temperature or high pressure, these forces become significant, causing the gas to deviate from ideal behavior.

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Ideal Gas Law

The Ideal Gas Law describes the behavior of an ideal gas through the equation PV=nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature. Ideal gases are assumed to have no intermolecular forces and occupy no volume. However, real gases deviate from this behavior under certain conditions, particularly at high pressures and low temperatures.

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01:15

Ideal Gas Law Formula

Intermolecular Forces

Intermolecular forces are the attractive forces between molecules that can affect their behavior in a gas phase. In ideal gas behavior, these forces are negligible, but in real gases, they can lead to deviations from ideality. For example, stronger intermolecular forces can cause gases to condense into liquids, especially at lower temperatures, leading to lower pressures than predicted by the Ideal Gas Law.

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Intermolecular vs Intramolecular Forces

Molecular Volume

Molecular volume refers to the actual space occupied by gas molecules. In the Ideal Gas Law, it is assumed that gas molecules have no volume, but in reality, they do occupy space. At high pressures, the volume of the gas molecules becomes significant compared to the volume of the container, causing deviations from ideal behavior as the gas cannot be compressed indefinitely.

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02:35

Constant-Volume Calorimetry

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