HW 2,3,4 question 17

[Holland Smith 3C]

I followed the steps from the hint, but am still having trouble with this problem. I started by finding the molar mass for fluorine (18.998) and divided by avogadro's constant and multiplied by 2. after that, I plugged in the values given (h using kg not j), the speed (442.4 m.s-1) and the value that I found previously. if anyone understands this I could def use the help, thanks!

[Ruben Adamov 1E]

For me the problem asked for the wavelength of a diatomic oxygen molecule not fluorine. "The average speed of a diatomic oxygen molecule at 25 ∘C is 482.1 m⋅s−1 . What is the average wavelength of an oxygen molecule at this temperature? Assume that the molecule acts as a single particle."
So the first thing I did was write out the formula and my known values. lambda = h/mv. I know v = 482.1 m/s and h = 6.626*10^-34 J/s.
Now all I need is m. The problem states that it is a diatomic oxygen molecule (O2) therefore the molar mass would be 32 g/mol. Now all I have to do is convert g/mol to kg/molecule. (32 g/mol) * (1/6.022*10^23 molecules/mol) * (1kg/1000g) = 5.314*10^-26 kg/molecule.
Now I have every value I need so I can plug it into the equation and find lambda.
Hope this helps!