(D) Given: $P_A^0 = 50 \ mm \ Hg$, $P_B^0 = 32 \ mm \ Hg$. Mole fraction in liquid phase: $X_A = \frac{1}{1+1} = 0.5$ and $X_B = \frac{1}{1+1} = 0.5$.

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(D) Given: $P_A^0 = 50 \ mm \ Hg$, $P_B^0 = 32 \ mm \ Hg$. Mole fraction in liquid phase: $X_A = \frac{1}{1+1} = 0.5$ and $X_B = \frac{1}{1+1} = 0.5$. Partial pressures: $P_A = P_A^0 \times X_A = 50 \times 0.5 = 25 \ mm \ Hg$ and $P_B = P_B^0 \times X_B = 32 \times 0.5 = 16 \ mm \ Hg$. Total pressure: $P_{total} = P_A + P_B = 25 + 16 = 41 \ mm \ Hg$. Mole fraction of $A$ in vapour phase $(Y_A)$: $Y_A = \frac{P_A}{P_{total}} = \frac{25}{41} \approx 0.6097 \approx 0.61$.

Class 12 Chemistry Solutions Ideal and Non-ideal solution

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Liquids $A$ and $B$ form an ideal solution. The vapour pressure of pure $A$ and $B$ are $50 \ mm \ Hg$ and $32 \ mm \ Hg$ respectively at $300 \ K$. One mole of liquid $A$ is mixed with $1$ mole of liquid $B$. What is the approximate mole fraction of $A$ in the vapour phase?

TS EAMCET 2023 All TS EAMCET

A
$0.39$
B
$0.5$
C
$0.25$
D
$0.61$

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In a binary ideal solution of liquids $A$ and $B$ at a constant temperature,the mole fraction of $A$ in the liquid phase is $0.7$ and in the vapor phase is $0.4$. If $P_A^o + P_B^o = 90 \, mm$,then the vapor pressures of pure liquids $A$ and $B$ at that temperature are respectively:

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What is a non-ideal solution and what is meant by positive deviation from Raoult's law?

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Total vapour pressure of a mixture of $1 \, mol \, X$ $(P_x^o = 150 \, torr)$ and $2 \, mol \, Y$ $(P_y^o = 300 \, torr)$ is $240 \, torr$. In this case:

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$A$ mixture of toluene and benzene forms a nearly ideal solution. Assume $p_{B}^{\circ}$ and $p_{T}^{\circ}$ to be the vapour pressures of pure benzene and toluene,respectively. The slope of the line obtained by plotting the total vapour pressure versus the mole fraction of benzene is $....$

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Solution $A$ contains acetone dissolved in chloroform and solution $B$ contains acetone dissolved in carbon disulphide. The type of deviations from Raoult's law shown by solutions $A$ and $B$,respectively,are:

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Liquids $A$ and $B$ form an ideal solution. The vapour pressure of pure $A$ and $B$ are $50 \ mm \ Hg$ and $32 \ mm \ Hg$ respectively at $300 \ K$. One mole of liquid $A$ is mixed with $1$ mole of liquid $B$. What is the approximate mole fraction of $A$ in the vapour phase?

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In a binary ideal solution of liquids $A$ and $B$ at a constant temperature,the mole fraction of $A$ in the liquid phase is $0.7$ and in the vapor phase is $0.4$. If $P_A^o + P_B^o = 90 \, mm$,then the vapor pressures of pure liquids $A$ and $B$ at that temperature are respectively:

What is a non-ideal solution and what is meant by positive deviation from Raoult's law?

Total vapour pressure of a mixture of $1 \, mol \, X$ $(P_x^o = 150 \, torr)$ and $2 \, mol \, Y$ $(P_y^o = 300 \, torr)$ is $240 \, torr$. In this case:

$A$ mixture of toluene and benzene forms a nearly ideal solution. Assume $p_{B}^{\circ}$ and $p_{T}^{\circ}$ to be the vapour pressures of pure benzene and toluene,respectively. The slope of the line obtained by plotting the total vapour pressure versus the mole fraction of benzene is $....$

Solution $A$ contains acetone dissolved in chloroform and solution $B$ contains acetone dissolved in carbon disulphide. The type of deviations from Raoult's law shown by solutions $A$ and $B$,respectively,are:

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