If O2
is bubbled through water at 393 K, how many millimoles of O2
gas would be dissolved in 1L of water? Assume that O2
exerts a
pressure of 0.95 bar.
According to Henry's Law :
p = KH x C
KH is the Henry's constant
C is the concentration of oxygen soluble in water
KH for O2 = 46.82 bar at 393 K
C = 0.95/46.82 = 0.0202 M
No. of moles = Molarity x Volume = 0.02 x 1 = 0.0202 Moles of Oxygen
Thus no. of millimoles of oxygen soluble in water = 20.2 millimoles
p = KH x C
KH is the Henry's constant
C is the concentration of oxygen soluble in water
KH for O2 = 46.82 bar at 393 K
C = 0.95/46.82 = 0.0202 M
No. of moles = Molarity x Volume = 0.02 x 1 = 0.0202 Moles of Oxygen
Thus no. of millimoles of oxygen soluble in water = 20.2 millimoles