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Worksheet about Chemistry Kinetic Molecular Theory Part 2 Study Guide | ||
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| Subject: Chemistry | ||
| 11th Grade | ||
| Term 1 | ||
| Year: 2023/2024 | ||
| Size: 362.2KB | ||
| Number of clicks: 133 | ||
| Publish date:November 05, 2023 | ||
| Added by: Eman | ||
| Last download date: 2024-09-12 14:45:38 | ||
| Updated by: Eman9966 on 2023-11-05 17:33:54 | By: theodor Tracey Barnette | |
| File info: Part 2: Assumptions of the Kinetic Molecular Theory The kinetic molecular theory is a model of the behavior of gases that explains their properties based on the motion of their atoms and molecules. The theory is based on five assumptions: Matter is made up of tiny particles called molecules. These particles are so small that they cannot be seen with even the most powerful microscopes. Molecules are in constant, random motion. This motion is due to the kinetic energy of the molecules, which is the energy of motion. The average kinetic energy of the molecules of a gas is directly proportional to the absolute temperature of the gas. This means that as the temperature of a gas increases, the average kinetic energy of its molecules also increases. Molecules collide with each other and with the walls of their container. These collisions are perfectly elastic, which means that no energy is lost in the collisions. The volume of a gas is determined by the volume of its container and the number of molecules in the container. The molecules of a gas are spaced far apart from each other, and they do not attract each other. Kinetic Energy and Temperature The average kinetic energy of the molecules in a gas is directly proportional to the absolute temperature of the gas. This means that as the temperature of a gas increases, the average kinetic energy of its molecules also increases. This is why gases expand when heated. The increased kinetic energy of the molecules causes them to collide with the walls of their container more frequently and with more force. This increased pressure causes the gas to expand. Collisions and Diffusion Molecules of a gas are constantly colliding with each other and with the walls of their container. These collisions are perfectly elastic, which means that no energy is lost in the collisions. The collisions cause the molecules to move in all directions, and this movement causes the gas to diffuse. Diffusion is the process by which a gas spreads out and mixes with other gases. Pressure The pressure of a gas is caused by the collisions of the molecules of the gas with the walls of their container. The pressure is directly proportional to the number of collisions per unit time and to the average kinetic energy of the molecules. This means that as the number of molecules in a container increases or as the average kinetic energy of the molecules increases, the pressure of the gas also increases. Implications of the Kinetic Molecular Theory The kinetic molecular theory has a number of implications for the behavior of gases. These implications include: Gases expand to fill their containers. Gases are compressible. Gases diffuse. Gases have low density. Gases have low viscosity. Gases have low heat capacity. Applications of the Kinetic Molecular Theory The kinetic molecular theory is a powerful tool that can be used to explain a wide variety of phenomena. Some of the applications of the theory include: The explanation of the behavior of gases. The development of gas laws. The design of gas appliances. The understanding of atmospheric processes. I hope this helps! | ||
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