* Kinetic Molecular Theory: Air molecules are in constant random motion. They collide with each other and the walls of the container (the room). The average kinetic energy of these molecules is directly proportional to the absolute temperature.
* Distribution of Speeds: The molecules in a gas don't all move at the same speed. They have a distribution of speeds, with some moving very fast, some very slow, and most somewhere in between.
* Root-Mean-Square (RMS) Speed: We can talk about the average speed of the molecules, but it's not a simple average. The RMS speed gives us a good measure of this average.
To calculate the RMS speed of air molecules:
1. Convert Celsius to Kelvin: 50 degrees Celsius is 323.15 Kelvin (K)
2. Use the formula:
```
v_rms = √(3RT/M)
```
where:
* v_rms is the root-mean-square speed
* R is the ideal gas constant (8.314 J/mol·K)
* T is the temperature in Kelvin
* M is the molar mass of air (approximately 0.029 kg/mol)
Calculation:
```
v_rms = √(3 * 8.314 J/mol·K * 323.15 K / 0.029 kg/mol)
v_rms ≈ 517 m/s
```
Important Note: This calculation gives the RMS speed, which is a kind of average. Individual air molecules will be moving at speeds faster or slower than this average.
