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Worksheet about Chemistry Kinetic Molecular Theory Part 4 Study Guide | ||
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| Subject: Chemistry | ||
| 11th Grade | ||
| Term 1 | ||
| Year: 2023/2024 | ||
| Size: 282.8KB | ||
| Number of clicks: 113 | ||
| Publish date:November 05, 2023 | ||
| Added by: Eman | ||
| Last download date: 2024-09-08 16:08:07 | ||
| Updated by: Eman9966 on 2023-11-05 17:45:20 | By: theodor Tracey Barnette | |
| File info: Info Real gases do not always behave perfectly according to the ideal gas law. This is because real gases have intermolecular forces, which are forces that exist between the molecules of a gas. These forces can cause the real gas to behave differently than an ideal gas. Deviations from Ideal Gas Behavior at Low Pressures At low pressures, the intermolecular forces between the molecules of a gas are negligible. Therefore, real gases behave very similar to ideal gases at low pressures. Deviations from Ideal Gas Behavior at High Pressures At high pressures, the intermolecular forces between the molecules of a gas can become significant. These forces can cause the real gas to deviate from ideal gas behavior. One way in which real gases can deviate from ideal gas behavior at high pressures is by having a lower volume than an ideal gas at the same temperature and pressure. This is because the intermolecular forces between the molecules of a real gas can cause the molecules to be attracted to each other. This attraction can cause the molecules to pack closer together, which results in a lower volume. Deviations from Ideal Gas Behavior at High Temperatures At high temperatures, the kinetic energy of the molecules of a gas is high. This high kinetic energy can overcome the intermolecular forces between the molecules of a gas. Therefore, real gases behave more like ideal gases at high temperatures. Real Gas Laws There are a number of real gas laws that take into account the intermolecular forces between the molecules of a gas. One of the most common real gas laws is the van der Waals gas law. The van der Waals gas law is: (P + a/V^2)(V - b) = nRT Where: P is the pressure of the gas in units of pascals (Pa) V is the volume of the gas in units of liters (L) n is the number of moles of gas R is the ideal gas constant, which has a value of 8.314 J/mol·K T is the temperature of the gas in units of Kelvin (K) a is the van der Waals a coefficient, which is a measure of the attractive forces between the molecules of the gas b is the van der Waals b coefficient, which is a measure of the volume of the molecules of the gas The van der Waals gas law is a more accurate description of the behavior of real gases than the ideal gas law. Conclusion Real gases do not always behave perfectly according to the ideal gas law. This is because real gases have intermolecular forces, which are forces that exist between the molecules of a gas. These forces can cause the real gas to behave differently than an ideal gas. At low pressures, real gases behave very similar to ideal gases. At high pressures, real gases can deviate from ideal gas behavior by having a lower volume than an ideal gas at the same temperature and pressure. At high temperatures, real gases behave more like ideal gases. There are a number of real gas laws that take into account the intermolecular forces between the molecules of a gas. The van der Waals gas law is one of the most common real gas laws. | ||
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