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Kinetic Theory of Gases PPT Physics Class 11

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1. What is the kinetic theory of gases?
Ans. The kinetic theory of gases states that gases are made up of tiny particles, either atoms or molecules, that are constantly in motion. These particles move in straight lines until they collide with each other or with the walls of the container.
2. How does temperature affect the kinetic energy of gas particles?
Ans. According to the kinetic theory of gases, as the temperature increases, the average kinetic energy of gas particles also increases. This means that the particles move faster and collide with each other and the container walls more frequently and with greater force.
3. What is the relationship between pressure and volume in the kinetic theory of gases?
Ans. According to the kinetic theory of gases, when the volume of a gas is decreased, the average speed of the gas particles increases because they have less space to move. This increase in particle speed leads to more frequent and forceful collisions with the container walls, resulting in an increase in pressure.
4. How does the number of gas particles affect the pressure of a gas?
Ans. According to the kinetic theory of gases, an increase in the number of gas particles in a given volume leads to more frequent collisions with the container walls, resulting in an increase in pressure. Conversely, a decrease in the number of gas particles leads to fewer collisions and a decrease in pressure.
5. What is the relationship between the root mean square speed of gas particles and temperature?
Ans. The root mean square speed of gas particles is directly proportional to the square root of the temperature. This means that as the temperature increases, the average speed of gas particles also increases. The root mean square speed is a measure of the average kinetic energy of the particles.
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