The Henry's Law constant for Helium, Hydrogen, Nitrogen and Oxygen at $293 K$ are $144.97 k B a r, 69.16 k B a r, 76.48 k B a r a n d 34.86 k B a r$ respectively.
Then which of the following gas will have the highest solubility in water at the given temperature of $293 K$ and atmospheric pressure?

Helium

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Hydrogen

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Nitrogen

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Oxygen

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Solution

The correct option is D Oxygen
Characteristics of Henry’s Law Constant:
1. Same unit as that of Pressure
2.Different G-L system have different values of henry's law constant.
3. It increases with temperature
4. It depends on intermolecular forces between gas-liquid.
5. Its value decreases with increase in solubility.
Henry's Law :
$p = K_{H} \times χ$
At a given pressure :
$K_{H} \propto \frac{1}{χ}$
More the value of Henry's law constant, lesser is the solubility of gas inside a given solvent.
Since value of Henry's law constant for oxygen is the least, so it will have the maximum value of solubility or mole fraction $(χ)$

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