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The Kinetic Molecular Theory of Gas I- Gaseous Video Lecture | Chemistry for GRE Paper II
FAQs on The Kinetic Molecular Theory of Gas I- Gaseous Video Lecture - Chemistry for GRE Paper II
| 1. What is the Kinetic Molecular Theory of Gas? |  |
Ans. The Kinetic Molecular Theory of Gas is a theory that explains the behavior of gas molecules based on their motion. It states that gas molecules are in constant motion, move in straight lines until they collide with each other or the walls of the container, and that their average kinetic energy is directly proportional to the temperature of the gas.
| 2. How does the Kinetic Molecular Theory explain the pressure of a gas? | |
Ans. According to the Kinetic Molecular Theory, the pressure of a gas is caused by the collision of gas molecules with the walls of the container. As the gas molecules move and collide, they exert a force on the walls, resulting in a pressure. The more frequent and energetic the collisions, the higher the pressure of the gas.
| 3. What are the assumptions of the Kinetic Molecular Theory of Gas? | |
Ans. The assumptions of the Kinetic Molecular Theory of Gas are:
1. Gas molecules are considered to be small, hard spheres with negligible volume.
2. Gas molecules are in constant, random motion.
3. Gas molecules undergo elastic collisions with each other and the walls of the container.
4. There are no attractive or repulsive forces between gas molecules, except during collisions.
| 4. How does the Kinetic Molecular Theory explain the temperature of a gas? | |
Ans. The Kinetic Molecular Theory explains temperature as the average kinetic energy of the gas molecules. As the temperature of a gas increases, the average kinetic energy of the gas molecules also increases. This is because higher temperatures result in greater molecular motion and faster average speeds of the gas molecules.
| 5. Can the Kinetic Molecular Theory be applied to all gases? | |
Ans. The Kinetic Molecular Theory can be applied to most gases under normal conditions. However, at very high pressures or low temperatures, the behavior of gases may deviate from the assumptions of the theory. In such cases, more advanced theories, such as the Van der Waals equation, may be used to describe the behavior of gases more accurately.
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