The following table represents a solubility of a few nonpolar gases in water at 25�C under a total pressure of 1.0 atmospheres. Based on the information provided, what is the most likely solubility value of F2?
So if we take a look here, we have N2O2 and F2N2 has a solubility of 0.6 millimolar, O2 has 1.2 millimolar, and F2 is what we need to find. If you look on your periodic table, you'll see that nitrogen is in Group 5A, Oxygen is in Group 6A and then fluorine is in Group 7A. From the pattern that we see going from nitrogen to oxygen, we can see that the solubility is increasing.
Now this partly is due to the fact that oxygen O2 weighs more than N2 and therefore it's going to be more soluble because it connects to ideas such as intermolecular forces. Now here we're going to say that going from N2 to O2 the mass is increasing, so our solubility increases and we can see that it increases by a lot. It goes from 0.6 to 1.2. Following this pattern, we should expect the solubility to keep on increasing if we go from O2 to F2.
So we should expect the solubility to be higher than 1.2, which means that A&B are out. Now going from N2 to O2 there was a big increase, so we should expect that continued pattern. There should be a big increase. Going from O2 to F2C wouldn't work because going from 1.2 to 1.3 is not a big enough increase. So the best answer here would be option D 4.2 millimolar for the solubility of F2.