Real gases deviate from ideal gas behavior, especially at high pressures and low temperatures. The ideal gas law assumes that gas particles have no volume and experience no intermolecular forces. However, real gas particles do have volume and experience attractive and repulsive forces. The van der Waals equation accounts for these deviations by introducing correction factors for pressure and volume. Understanding these deviations is crucial for accurate calculations involving real gases.
Match the term with its definition:
| Term | Definition |
|---|---|
| 1. Compressibility Factor (Z) | A. Intermolecular forces that cause gases to deviate from ideal behavior. |
| 2. Van der Waals Equation | B. A measure of how much a real gas deviates from ideal gas behavior; equal to $PV/nRT$. |
| 3. Intermolecular Forces | C. The volume excluded by a mole of gas particles. |
| 4. Excluded Volume | D. An equation of state that modifies the ideal gas law to account for real gas behavior. |
| 5. Ideal Gas Law | E. The equation of state of a hypothetical ideal gas, given as $PV = nRT$. |
Real gases deviate from ideal behavior due to two main factors: the __________ of gas particles and the presence of __________. The __________ equation modifies the ideal gas law to account for these factors by introducing correction terms $a$ and $b$. The term $a$ accounts for __________ forces, while the term $b$ accounts for __________. These deviations are most significant at __________ pressures and __________ temperatures.
Explain how the compressibility factor, Z, indicates the deviation of a real gas from ideal behavior. What does it mean if Z > 1? What does it mean if Z < 1? Provide a specific example of a gas and conditions where it would exhibit non-ideal behavior. 💡
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