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Kinetic Molecular Theory of Gases Video Lecture | Physics Class 11 - NEET
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FAQs on Kinetic Molecular Theory of Gases Video Lecture - Physics Class 11 - NEET
| 1. What is the Kinetic Molecular Theory of Gases? |  |
Ans. The Kinetic Molecular Theory of Gases is a scientific theory that explains the behavior of gases in terms of the motion of their molecules. It posits that gas particles are in constant, random motion and that the pressure exerted by a gas is due to collisions of these particles with the walls of their container. The theory also assumes that gas particles have negligible volume compared to the volume of the container and that there are no attractive or repulsive forces between them.
| 2. What are the main postulates of the Kinetic Molecular Theory? | |
Ans. The main postulates of the Kinetic Molecular Theory include:
1. Gases consist of a large number of tiny particles (molecules or atoms) that are in constant random motion.
2. The volume of gas particles is negligible compared to the volume of the container.
3. There are no intermolecular forces acting between gas particles, allowing them to move freely.
4. Collisions between gas particles and between particles and the walls of the container are elastic, meaning that no kinetic energy is lost in these collisions.
5. The average kinetic energy of gas particles is directly proportional to the absolute temperature of the gas.
| 3. How does temperature affect the kinetic energy of gas particles? | |
Ans. According to the Kinetic Molecular Theory, the average kinetic energy of gas particles is directly proportional to the absolute temperature of the gas. As temperature increases, the average kinetic energy of the particles also increases, resulting in faster movement and more frequent collisions. Conversely, as temperature decreases, the average kinetic energy and the speed of the gas particles decrease.
| 4. What role do gas volume and pressure play in the behavior of gases according to the Kinetic Molecular Theory? | |
Ans. In the Kinetic Molecular Theory, gas volume and pressure are interconnected through the motion of gas particles. When the volume of a gas decreases (while keeping the temperature constant), the particles have less space to move, leading to more frequent collisions with the walls of the container, which increases pressure. Conversely, if the volume increases, the particles have more room to move, resulting in fewer collisions and lower pressure. This relationship is described by Boyle's Law.
| 5. How does the Kinetic Molecular Theory explain the diffusion of gases? | |
Ans. The Kinetic Molecular Theory explains diffusion as the process by which gas particles spread out and mix due to their constant random motion. When gas particles encounter each other, they collide and scatter in different directions. The higher the temperature, the faster the particles move, enhancing the rate of diffusion. This explains why gases tend to fill the container they are in, moving from areas of higher concentration to lower concentration until evenly distributed.
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Dec 23, 2024 Last updated |
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