If the K_{H} values for Ar_{(g)},CO_{2_{(g)}} | vedclass

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(D) According to Henry's law,the solubility of a gas in a liquid is inversely proportional to the Henry's law constant $(K_{H})$,given by the relation

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$Ar < CO_{2} < CH_{4} < HCHO$

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(D) According to Henry's law,the solubility of a gas in a liquid is inversely proportional to the Henry's law constant $(K_{H})$,given by the relation $S \propto \frac{1}{K_{H}}$.Therefore,a lower $K_{H}$ value corresponds to higher solubility.The given $K_{H}$ values are: $Ar = 40.39$,$CO_{2} = 1.67$,$CH_{4} = 0.413$,and $HCHO = 1.83 imes 10^{-5}$.Comparing these values,the order of $K_{H}$ is: $Ar > CO_{2} > CH_{4} > HCHO$.Thus,the increasing order of solubility is: $Ar < CO_{2} < CH_{4} < HCHO$.

If the $K_{H}$ values for $Ar_{(g)}$,$CO_{2_{(g)}}$,$HCHO_{(g)}$ and $CH_{4_{(g)}}$ respectively are $40.39$,$1.67$,$1.83 \times 10^{-5}$ and $0.413$,then identify the correct increasing order of their solubilities.

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