Which of the following is true regarding Henry's Law constant for different aqueous solutions of CO2(g) and O2(g) at a given temperature?
(Assume both the gases have same partial pressure)
A
KH(CO2)=KH(O2)
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B
Cannot be predicted
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C
KH(CO2)>KH(O2)
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D
KH(CO2)<KH(O2)
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Solution
The correct option is DKH(CO2)<KH(O2) CO2 is more soluble in water as compared to O2 because the two C=O bonds in CO2 are more polarized whereas in O2 bonds are not polarized.
Hence more solubility is there for CO2 in polar water molecule
By Henry's Law: p=KH×χ
Here p is the partial pressure of gas over the solution. KH is Henry’s law constant χ is mole fraction of the gas in the solution.
Since χCO2>χO2
So, for p to be same KH(CO2)<KH(O2)