1. The problem statement, all variables and given/known data We know that for dry air, we have: -78.08% mol N2 ; -20.94% mol O2. This is: - Y(N2) = 0.7808 for nitrogen (the molar fraction in vapor) - Y (O2) = 0.2094 for oxygen Knowing that the Henry's law constants are: for N2 and O2 are 6.51 x 10^7 Torr and 3.3 x 10^7 Torr, respectively Calculate the mole fractions of N2 and O2 dissolved in water (xN2 and xO2) under total pressure of 1.000 bar 2. Relevant equations Henry's law: The partial pressure = henry's constant k1 x mole fraction of water (x) P(N2) = K(N2).X(N2) Same for O2. Also, from Raoult's law: Y(N2) = P(N2)/P(tot) Same for oxygen. 3. The attempt at a solution I tried applying the equations, but instead of the expected (x(N2)=0.6), I get really small results such as 0.00000651 I am just wondering if I am doing anything wrong by mixing the vapour molar fraction equation with Henry's law for the molar fractions for water? Thank you.