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Q.

The vapour pressures of A and B at $25^{o} C$ are 90mm Hg and 15 mm Hg respectively. If A and B are mixed such that the mole fraction of A in the mixture is 0.6, then the mole fraction of B in the vapour phase $x \times 10^{- 1}$ The value x is _______. (Nearest Integer)

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Detailed Solution

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Total pressure of mixture $= P_{T o t a l} = X_{A} \times P_{A}^{o} + X_{B} \times P_{B}^{o} = 90 \times 0.6 + 15 \times 0.4 = 60 m m$

Mole fraction of B in vapour phase, $(X_{B}^{'}) = \frac{X_{B}^{'} \times P_{B}^{o}}{P_{T o t a l}}$

$∴ X_{B}^{'} = \frac{0.4 \times 15}{60} = 0.1 = 1 \times 10^{- 1}$

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The vapour pressures of A and B at 25oC are 90mm Hg and 15 mm Hg respectively. If A and B are mixed such that the mole fraction of A in the mixture is 0.6, then the mole fraction of B in the vapour phase x×10−1 The value x is _______. (Nearest Integer)