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The total vapour pressure of a binary solution is given by
\[
P=\left(100 X_{A}+260 X_{B}\right) \mathrm{mm} \mathrm{Hg}
\]
where, \( X_{A} \) and \( X_{B} \) are the mole fractions of components \( A \) and \( B \). This indicates that the:
(a) vapour pressure of solution is less than the pure \( B \) component
(b) vapour pressure of solution is more than that of pure \( A \) component
(c) vapour pressure of pure \( A \) is \( 100 \mathrm{~mm} \mathrm{Hg} \) and that of pure \( B \) is \( 260 \mathrm{~mm} \mathrm{Hg} \)
(d) the vapour pressure of pure \( A \) and \( B \) are \( 260 \mathrm{~mm} \mathrm{Hg} \) and \( 100 \mathrm{~mm} \mathrm{Hg} \) respectively
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