O2is bubbled through water at 293K. Assuming that O2 exerts a partial pressure of 0.98 bar, calculate the solubility of O2 in grams per litre. The value of Henry's Law constant (KH) for O2 is 34.84 kbar

pO2=KHO2

Thus
χO2=pO2​/K=0.098/(34.84*103) =2.81*10-5

No. of moles of H2O in 1L =55.55
χO2 = nO2​/(nO2 + nH2O​) = nO2/​(nO2 +55.55​)
APPROXIMATELY
χO2 =​nO2​/55.55

nO2 =2.81*10-5*55.55 =1.56*10-3 mol

Thus solubility of O2 is = ​1.56*10-3  *32 g/L = 0.05 g/L
 

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