At 300 K,the vapor pressures of two pure liq | vedclass

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(D) Given: $P_A^0 = 150 \ mm \ Hg$,$P_B^0 = 100 \ mm \ Hg$. Since the mole fractions are equal,$X_A = X_B = 0.5$. Total pressure $P_{total} = P_A^0 X_

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$0.4$

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(D) Given: $P_A^0 = 150 \ mm \ Hg$,$P_B^0 = 100 \ mm \ Hg$. Since the mole fractions are equal,$X_A = X_B = 0.5$. Total pressure $P_{total} = P_A^0 X_A + P_B^0 X_B = (150 	imes 0.5) + (100 	imes 0.5) = 75 + 50 = 125 \ mm \ Hg$. According to Dalton's Law,the partial pressure of $B$ in the vapor phase is $P_B = P_B^0 X_B = 100 	imes 0.5 = 50 \ mm \ Hg$. The mole fraction of $B$ in the vapor phase $(Y_B)$ is given by $Y_B = \frac{P_B}{P_{total}} = \frac{50}{125} = 0.4$.

At $300 \ K$,the vapor pressures of two pure liquids $A$ and $B$ are $150 \ mm \ Hg$ and $100 \ mm \ Hg$,respectively. If the mole fractions of $A$ and $B$ in the solution are equal,then the mole fraction of $B$ in the vapor phase at the same temperature is:

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