The Henry's law constant for O2 at 298 K is 4.2 x 104 bar. A vessel maintained at T = 298 K contains 100 cm3 of H2O(l) and has a "head space", i. e., a volume not filled with liquid, of 500 cm3. If 1.00 bar of O2 is introduced into the head space and the system is allowed to come to equilibrium, what fraction of the O2 that was admitted to the vessel will be in the liquid phase, i. e., dissolved in the H2O(l)? Justify any approximations that you make. Note that the density of H2O(l) at 298 K is 0.997 grams per cm3.