Question

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Q.The mole fraction of Helium in a saturated solution at 20℃ is 1.2 × 10^(-6). Find the pressure of Helium above the solution. Given Henry's constant at 20℃ is 144.97 kbar.
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Answer 1

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PH2=KHXH2

XH2=PH2kH

=1bar7.18×103bar

=1.404×10−5

Now,

nH2O in 1L=1000g18

=55.5

Therefore ,

nH255.55=1.404×10−5

nH2=1.79×10−4moles

Hence the solubility of H2 in water is 7.79×10−4mol/L

Answer 2

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$K_H$ $= 144.97 kbar = 144.97 \times 10 ^3 bar$

$p _{He} = K_H x   _{He}$

$p _{He} = (144.97 \times 10 ^3  bar)(1.4 \times 10 ^{-6} )$

$p _{He} = 0.203 bar$

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