That is interesting, and I accept the correction. However, there is only a small change in the gas equilibrium pressure (16%) for a hydrostatic pressure of 100 atm. Moreover, if I understand the first page correctly (I can't access the full article), water equilibrated with gas at 1 atm is subjected to hydrostatic pressure, and the equilibrium gas pressure increases, i.e. the solubility for a given gas pressure decreases. That is what I would expect qualitatively, at high pressure there will be less free volume, so less capacity to dissolve gas. What this means is that the Henry's Law constant decreases slightly with increasing hydrostatic pressure.
But, OP, let's be clear. Henry's Law does not say "at higher pressure, more gas particles are forced through the water/gas interface into the liquid phase and are dissolved by the liquid (this is henry's law)" - at least, not if you're interpreting that to mean that dissolved concentration is proportional to hydrostatic pressure. It says that the concentration of dissolved gas is proportional to the partial pressure of that gas. It's just that the constant of proportionality varies slightly with the hydrostatic pressure. You are not given the information in the question to deal with that, and I guess you're not intended to - at a pressure of 2 atm, the effect will be very small. What I guess you're expected to do, but is absolutely not correct, is to multiply the Henry's Law constant by the hydrostatic pressure. At least, that's what you did, and got the "right" (wrong) answer.