Neon would have the highest average molecular speed at the same temperature because it has the lowest molar mass among the given options, according to the kinetic theory of gases.
The average molecular speed of a gas is determined by its temperature and molar mass. According to the kinetic theory of gases, the root mean square speed of gas molecules is proportional to the square root of their temperature and inversely proportional to the square root of their molar mass. In other words, lighter molecules at the same temperature will, on average, move faster than heavier ones.
Comparing the provided gases at the same temperature:
- Dinitrogen monoxide (N2O): ~44 g/mol
- Sulfur dioxide (SO2): ~64 g/mol
- Nitrogen dioxide (NO2): ~46 g/mol
- Argon (Ar): ~40 g/mol
- Carbon tetrafluoride (CF4): ~88 g/mol
- Neon (Ne): ~20 g/mol
Neon has the lowest molar mass among the options, making it the gas with the highest average molecular speed at the given temperature. The relationship between molar mass and average molecular speed highlights the impact of mass on the kinetic behavior of gases, with lighter gases exhibiting higher average speeds under similar conditions.