The Henry's law constants K_H (in kbar) of four gases in water at 298 K are: N2 76.5, O2 34.9, He 145.0, CO2 1.67. At equal partial pressure, which gas has the highest mole-fraction solubility?

NEET levelSingle correct optionDifficulty 1 of 3so113

The Henry's law constants $K_{H}$ (in kbar) of four gases in water at $298 K$ are: $N X_{2}$ 76.5, $O X_{2}$ 34.9, $He$ 145.0, $CO X_{2}$ 1.67. At equal partial pressure, which gas has the highest mole-fraction solubility?

Henry's law gives

x = p / K_{H}

, so at equal partial pressure the gas with the smallest

K_{H}

is the most soluble. The smallest value is 1.67 kbar, which belongs to

CO X_{2}

He

has the largest

K_{H}

and is the least soluble.