what is the ratio of solubilities of N2 and O2 in H2O at 373K? given that KH(N2) = 12.6 X 104 atm and KH(O2) = 7.01 X 104 atm. assume that P(N2) = 0.8 atm and P(O2) = 0.2 atm.
Given:
KH(N2) = 12.6 X 104 atm
KH(O2) = 7.01 X 104 atm
P(N2) = 0.8 atm
P(O2) = 0.2 atm
Partial pressure of the gas is proportional to mole fraction of the gas in the solution.
X(N2) = p(N2) / kH(N2)
X(O2) = p(O2) / kH (O2)
So ratio of solubilities of N2 and O2:
X(N2) / X(O2) = 0.8 x 7.01 x 104 / 12.6x104 x 0.2
X(N2) / X(O2) = 2.22