Kinetic Theory of Gas
The Kinetic Theory of gases is a classical model of gases, according to which gases are composed of molecules/particles that are in random motion. While undergoing this random motion, kinetic energy in molecules can assume random velocity across all directions. It also says that the constituent particles/molecules undergo elastic collision, which means that the total kinetic energy remains constant before and after the collision. The average kinetic energy of the particles also determines the pressure of the gas.
P-V Diagram
A P-V diagram is a very important tool of the branch of physics known as thermodynamics, which is used to analyze the working and hence the efficiency of thermodynamic engines. As the name suggests, it is used to measure the changes in pressure (P) and volume (V) corresponding to the thermodynamic system under study. The P-V diagram is used as an indicator diagram to control the given thermodynamic system.
What effect does an increase in temperature have on the volume of a gas that is not in a closed container?
Volume of the gas increases as the temperature increases. According to the kinetic theory of gases, particles are free to move in any direction at any speed.
When the temperature increases, the gas molecules will attain more kinetic energy and they will move with increased speed in all possible directions. As a result the range of the gas molecule increases and they can travel to long distances.
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