Questions

For an ideal solution of liquids A and B, which of the facts is correct?
Where $k_{H}^{'} s$ stand for Henry's law constants and $p^{*'} s$ are the vapour pressures of pure components.

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k_{H, A} > p_{A}^{*}

and

k_{H, B} > p_{B}^{*}

k_{H, A} < p_{A}^{*}

and

k_{H, B} < p_{B}^{*}

k_{H, A} = p_{A}^{*}

and

k_{H, B} = p_{B}^{*}

k_{H, A} > p_{A}^{*}

and

k_{H, B} < p_{B}^{*}

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detailed solution

Correct option is C

By Henry’s law constant, we know that the the value of solubility is proportional to the mole fraction of the gas,

$p = K_{H} X$

For pure components, For an ideal solution of liquids A and B,

$k_{H, A} = p_{A}^{*}$ and $k_{H, B} = p_{B}^{*}$

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For an ideal solution of liquids A and B, which of the facts is correct?Where kH′s stand for Henry's law constants and p∗′s are the vapour pressures of pure components.