Gas Expansion and Work: Effects on Internal Energy and Temperature

In summary, the conversation discusses the amount of work done on and by a gas cylinder when it is lifted from one floor to another, as well as the potential change in internal energy and temperature of the gas. Two cases are considered - when the cylinder is lifted slowly and when it is lifted suddenly and stopped. The conversation also touches upon the concept of work and the change in volume of the gas. The topic of heat is mentioned, with a request for book recommendations due to confusion and many assumptions involved.
  • #1
gandharva_23
61
0
A cylinder containing a gas is lifted from the first floor to the second floor .What is the amount of work done on the gas ? What is the amount of work done by the gas ? Is the internal energy of the gas increased ? Is the temperature of the gas increased ?
consider 2 cases :
case 1 : the cylinder is taken up slowly
case 2 : cylinder is suddenly taken up and stopped
 
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  • #2
One needs to show some effort to answer these questions, please. :smile:

What does it mean to do work on the gas, or for the gas to do work?

Does the 'boundary' of the gas change, i.e. does the volume of gas change?
 
  • #3
Sir i have just started studying heat . did not find it interesting at all . please suggest some good book . What i thought in this question was that the potential energy of the gas molecules will increse so the randomness of gas molecules will change hence the temperature of the gas will increase . But the answer given in the book that i referred was that nothing will change . then i thought it is probably because the tempetature of the gas is only due to the KE of the gas which probably will not change (wont it change ?) and i got totally confused . it is probably the ugliest topic . so many assumptions ...
 

1. What is the Kinetic Theory of Gases?

The Kinetic Theory of Gases is a scientific model that explains the behavior of gases at a microscopic level. It states that gas particles are in constant, random motion and that their kinetic energy is directly proportional to their temperature.

2. What are the main assumptions of the Kinetic Theory of Gases?

The main assumptions of the Kinetic Theory of Gases are:

  • The gas particles are in constant, random motion.
  • The particles have negligible volume compared to the volume of the container they are in.
  • The particles do not exert attractive or repulsive forces on each other.
  • The collisions between particles and with the walls of the container are elastic.
  • The average kinetic energy of the particles is directly proportional to the temperature.

3. How does the Kinetic Theory of Gases explain the relationship between pressure and volume?

According to the Kinetic Theory of Gases, gas particles move in random directions and collide with each other and the walls of the container. When the volume of the container is decreased, the particles have less space to move and collide with each other more frequently. This leads to an increase in pressure. On the other hand, when the volume is increased, the particles have more space to move and collide less frequently, resulting in a decrease in pressure.

4. How does the Kinetic Theory of Gases explain the relationship between temperature and pressure?

The Kinetic Theory of Gases states that the average kinetic energy of gas particles is directly proportional to the temperature. As temperature increases, the particles have more kinetic energy, resulting in faster and more frequent collisions with the walls of the container. This leads to an increase in pressure. Conversely, as temperature decreases, the particles have less kinetic energy and collisions occur less frequently, resulting in a decrease in pressure.

5. How does the Kinetic Theory of Gases explain the behavior of real gases?

The Kinetic Theory of Gases is based on idealized assumptions and does not fully account for the behavior of real gases. However, it can be used as a simplified model to explain the behavior of real gases in most situations. At low temperatures and high pressures, the assumptions of the Kinetic Theory may break down and the behavior of real gases may deviate from the predictions of the theory.

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