N2 gas is bubbled through water at 298K. How many moles of N2 gas would dissolve in 1L water assumed that partial pressure of gas is = 0.987 bar and KH = 76.48 K .
KH = 76.48kbar = 76480bar
P = KH × x x= 0.98976480=1.293 ×10−5. This is the mole fraction of N2 gas dissolved in water
Volume of water = 1L = 1000mL Taking density as 1g/mL, mass of 1L =1000g Moles of water in 1L = 1000/18=55.56 Let us take the moles of nitrogen as x Total moles = moles of N2 + moles of water = x + 55.56 mole fraction of N2 1.293 ×10−5= xx+55.561.293 ×10-5x + 1.293 ×10-5 × 55.56 =x x(1-1.293 ×10-5) = 1.293 ×10-5 × 55.56 x=7.17 ×10-4mol = 0.717mmoles