The Kinetic Theory of Gases and Temperature
* Kinetic energy is the energy of motion. The faster a molecule moves, the more kinetic energy it has.
* Temperature is a measure of the average kinetic energy of the molecules in a substance.
* The Kinetic Theory of Gases states that the average kinetic energy of gas molecules is directly proportional to the absolute temperature (measured in Kelvin).
Different Molecules in Air
Air is a mixture of gases, primarily nitrogen (N2), oxygen (O2), and smaller amounts of argon (Ar), carbon dioxide (CO2), and other trace gases. While these molecules have different masses, at a given temperature, they will have the same average kinetic energy.
Why the Same Average Kinetic Energy?
* Collisions: Gas molecules are constantly colliding with each other and the walls of their container. These collisions transfer energy.
* Equilibrium: Over time, collisions lead to a state of thermal equilibrium. This means that the energy is distributed evenly among all the molecules, regardless of their mass.
* Temperature as a measure: Temperature is the reflection of this equilibrium. When the temperature is the same, the average kinetic energy is the same.
Important Note: While the average kinetic energy is the same, the individual speeds of the molecules will be different. Lighter molecules (like nitrogen) will, on average, move faster than heavier molecules (like carbon dioxide) at the same temperature.
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