If He(g) has an average kinetic energy of 7590 J/mol under certain conditions, what is the root mean square speed of F2(g) molecules under the same conditions?
To find the root mean square (rms) speed of F2(g) molecules, we can use the kinetic theory of gases equation:
v(rms) = √(3RT/M)
where:
- v(rms) represents the root mean square speed
- R is the gas constant (8.314 J/(mol·K))
- T is the temperature in Kelvin
- M is the molar mass of the gas
In this case, we need the molar mass of F2(g). The molar mass of an element is equal to the atomic mass in grams/mol. The molar mass of fluorine is approximately 19 g/mol. Since F2 represents a molecule of fluorine, the molar mass of F2(g) is 2 times the molar mass of fluorine, which is 38 g/mol.
Now, we have all the necessary information to calculate the rms speed of F2(g). However, we need the temperature at which the average kinetic energy of He(g) is given.
Could you provide the temperature at which the average kinetic energy of He(g) is measured, or any other relevant information?