If, at a particular temperature, the average speed of CH4 molecules is 1000 mine/hr, what would be the average speed of CO2 molecules at the same temperature?
To determine the average speed of CO2 molecules at the same temperature, we can use the concept of kinetic theory of gases. According to the kinetic theory, the average speed of gas molecules is directly proportional to the square root of their temperature.
To compare the average speeds of CH4 and CO2 molecules, we need to know the temperature at which they both exist. Without this information, it is not possible to determine their respective average speeds accurately.
However, assuming that both CH4 and CO2 are at the same temperature, we can use the square root of the molecular mass ratio to approximate their average speeds.
The molecular mass of CH4 is approximately 16 g/mol, while the molecular mass of CO2 is approximately 44 g/mol. Thus, the square root of the molecular mass ratio is √(44/16) ≈ 1.87.
If the average speed of CH4 molecules is given as 1000 m/s, we can multiply it by the square root of the molecular mass ratio to estimate the average speed of CO2 molecules:
Average speed of CO2 = Average speed of CH4 × √(44/16)
Using the given average speed of CH4 (1000 m/s), we can calculate:
Average speed of CO2 = 1000 m/s × 1.87 ≈ 1870 m/s.
Therefore, the estimated average speed of CO2 molecules would be approximately 1870 m/s at the same temperature, assuming they are both at the same temperature and applying the square root of the molecular mass ratio.